CHM 1046 FINAL REVIEW

Size: px
Start display at page:

Download "CHM 1046 FINAL REVIEW"

Transcription

1 CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART II Chapter Description 14 Chemical Equilibrium 15 Acids and Bases 16 Acid-Base Equilibrium 17 Solubility and Complex-Ion Equilibrium 19 Electrochemistry 20 Nuclear Chemistry

2 CH. 14 CHEMICAL EQUILIBRIUM DYNAMIC EQUILIBRIUM: WHEN FORWARD AND REVERSE REACTION RATES ARE THE SAME. *PURE SOLIDS AND LIQUIDS DO NOT APPEAR IN THE EQUILIBRIUM CONSTANT EXPRESSION (ANY K OR Q) THE EQUILIBRIUM CONSTANT K C : THE VALUE OBTAINED FOR THE EQUILIBRIUM-CONSTANT EXPRESSION WHEN EQUILIBRIUM CONCENTRATIONS ARE SUBSTITUTED. THE EQUILIBRIUM CONSTANT KP: THE EQUILIBRIUM CONSTANT EXPRESSION FOR A GASEOUS REACTION IN TERMS OF PARTIAL PRESSURES. FOR GASES: K P = K C (RT) ΔN, WHERE ΔN = DIFFERENCE OF COEFFICIENT. Ch. 14 Chemical Equilibrium

3 CALCULATING VALUES OF K IF 2 OR MORE REACTIONS ARE ADDED TO ACHIEVE A GIVEN REACTION, THE EQUILIBRIUM CONSTANT FOR THE GIVEN EQUATION EQUALS THE PRODUCT OF THE EQUILIBRIUM CONSTANTS (K) OF THE ADDED EQUATIONS. K 1 xk 2 IF REACTION IS REVERSED YOU TAKE THE INVERSE OF ORIGINAL K OF REACTION. 1/K IF MULTIPLIED OR DIVIDED, RAISE K TO THAT POWER. EX: MULTIPLY BY 2 EX: DIVIDE BY 3 K 2 K 1/3 Ch. 14 Chemical Equilibrium

4 USING Q C TO DETERMINE THE DIRECTION OF EQUILIBRIUM REACTION QUOTIENT (Q C ): THE INITIAL REACTION RATE OF A REACTION. ITS NOT A CONSTANT BUT DYNAMIC. THE RELATIONSHIP BETWEEN Q C AND K C GIVES THE DIRECTION OF THE EQUILIBRIUM. IF K C > Q C EQUILIBRIUM IS IN THE FORWARD DIRECTION. IF K C = Q C REACTION IS IN EQUILIBRIUM. IF K C < Q C EQUILIBRIUM IS IN THE REVERSE DIRECTION. IF Q C = 0 ONLY REACTANTS ARE PRESENT. IF Q C = ONLY PRODUCTS ARE PRESENT. Ch. 14 Chemical Equilibrium

5 1. Consider the equilibrium between Dinitrogen Tetroxide and Nitrogen Dioxide: N2O4(g) 2NO2(g) a) What is the value of Kc for this reaction? Kp = at 319 K b) What is value of Kp for the reaction 2NO2 (g) N2O4(g) c) If the equilibrium partial pressure of NO2 (g) is atm, what is the equilibrium partial pressure of N2O4(g)? Ch. 14 Chemical Equilibrium

6 1. Consider the equilibrium between Dinitrogen Tetroxide and Nitrogen Dioxide: N2O4(g) 2NO2(g) a) What is the value of Kc for this reaction? Kp = at 319 K b) What is value of Kp for the reaction 2NO2 (g) N2O4(g) c) If the equilibrium partial pressure of NO2 (g) is atm, what is the equilibrium partial pressure of N2O4(g)? a) K p = K c (RT) Δn Kp K c = (RT) Δn K c = ( x 319 ) 2-1 b) Reaction reversed then take the inverse of Kp 1/ K p = 1/ c) (P NO2 ) 2 Kp = (P N 2O4 ) (0.223) = (P N2O4 ) Ch. 14 Chemical Equilibrium

7 2. If a 2.50 L vessel at 1000 C containes mol CO2, 1.25 mol CF4, and 0.75 mol COF2, in what direction will a net reaction occur to reach the equilibrium? CO2 (g) + CF4 (g) 2COF2 (g) Kc = 1000 K Solution: How do you determine the direction of a reaction in order to reach equilibrium? [COF2] 2 Q c = [CO2] [CF4] [CO2] = mol / 2.5 L = 0.21 M [CF4] = 1.25 mol / 2.5 L = 0.5 M [COF2] = 0.75 mol / 2.5 L = 0.3 M [0.3] 2 Q c = [0.21] [0.5] Kc = 0.50 Ch. 14 Chemical Equilibrium

8 3. Starting with mol each of CO and H2O in a 5.00 L flask, equilibrium is established in the following reaction at 600K: CO(g) + H2O(g) CO2 (g) + H2 (g) Kc = 23.2 at 600K What is the concentration of hydrogen at equilibrium? Ch. 14 Chemical Equilibrium

9 Balanced Equation [CO] = mol/ 5 L = 0.02 M [H2O] = mol / 5 L = 0.02 M CO(g) + H2O(g) CO2 (g) H2 (g) Initial Change - x -x +x +x Equilibrium 0.02-x 0.02-x x x [CO2] [H2] Kc = [CO] [H2O] [X] [X] 23.2 = [0.02-X] [0.02-X] Solution [X] = [0.02-X] 2 *Take the square root of both sides: [X] 4.82 = [0.02-X] X = X = X X 5.82X = X = 0.096/ 5.82 X = SO [H2]= X at equilibrium Ch. 14 Chemical Equilibrium

10 4. The K eq of a reaction is 4x10-7. At equilibrium. a) The products are favored b) The reactants are favored c) The reactants and products are present in equal amounts d) The rate of the forward and reverse reaction are the same Ch. 14 Chemical Equilibrium

11 4. The K eq of a reaction is 4x10-7. At equilibrium. a) The products are favored c) The reactants and products are present in equal amounts d) The rate of the forward and reverse reaction are the same Explanation: Here K eq = K eq << 1 Therefore Reactants are favored!! What if K eq >> 1????? Ch. 14 Chemical Equilibrium

12 4. The K eq of a reaction is 4x10-7. At equilibrium. a) The products are favored c) The reactants and products are present in equal amounts d) The rate of the forward and reverse reaction are the same Explanation: Here K eq = K eq << 1 Therefore Reactants are favored!! What if K eq >> 1????? Products would be favored Ch. 14 Chemical Equilibrium

13 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Shifts RX'N which way? Add PCl 5 Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Add Catalyst Ch. 14 Chemical Equilibrium

14 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Shifts RX'N which way? Right Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Add Catalyst Ch. 14 Chemical Equilibrium

15 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Shifts RX'N which way? Right Right Add Ar Decrease V (or increase P) Increase T Add Catalyst Ch. 14 Chemical Equilibrium

16 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Add Ar Shifts RX'N which way? Right Right No effect Decrease V (or increase P) Increase T Add Catalyst Ch. 14 Chemical Equilibrium

17 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Shifts RX'N which way? Right Right No effect Left High to Low #of moles of Gases 1 mol 2 mol Add Catalyst Ch. 14 Chemical Equilibrium

18 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Shifts RX'N which way? Right Right No effect Left High to Low #of moles of Gases 1 mol 2 mol Right Add Catalyst Ch. 14 Chemical Equilibrium

19 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Add Catalyst Shifts RX'N which way? Right Right No effect Left High to Low #of moles of Gases 1 mol 2 mol Right No effect on equilibrium *Catalysts Lowers Activation Energy only Ch. 14 Chemical Equilibrium

20 5. For the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) H rxn = +111 kj. Fill in the following table: Changes Add PCl 5 Remove Cl 2 Add Ar Decrease V (or increase P) Increase T Shifts RX'N which way? Right Right No effect Left High to Low #of moles of Gases 1 mol 2 mol Right Add Catalyst No effect on equilibrium *Catalysts Lowers Activation Energy only Which of the top changes would cause a change in K? ONLY a change in Temperature can cause a change in K Ch. 14 Chemical Equilibrium

21 Ch. 15 Acids and Bases CH. 15 ACIDS AND BASES Arrhenius Definitions: 1) Acid: substance that when dissolved in water increases [H+] 2) Base: substance that when dissolved in water increases [OH - ] Example: Identify following as Arrhenius Acid/Base HCl NaOH

22 Ch. 15 Acids and Bases CH. 15 ACIDS AND BASES Arrhenius Definitions: 1) Acid: substance that when dissolved in water increases [H+] 2) Base: substance that when dissolved in water increases [OH - ] Example: HCl (Acid) NaOH (Base) Brønsted-Lowry Definitions: 1) Acid: substance that donates a proton, H+, in a reaction 2) Base: substance that accepts a proton, H+, in a reaction Example: Identify following as Bronsted-Lowry Acid/Base :NH 3 HCl

23 Ch. 15 Acids and Bases CH. 15 ACIDS AND BASES Arrhenius Definitions: 1) Acid: substance that when dissolved in water increases [H+] 2) Base: substance that when dissolved in water increases [OH - ] Example: HCl (Acid) NaOH (Base) Brønsted-Lowry Definitions: 1) Acid: substance that donates a proton, H+, in a reaction 2) Base: substance that accepts a proton, H+, in a reaction Example: HCl (Acid) :NH 3 (Base) Lewis Definitions: 1) Acid: is an electron pair acceptor. 2) Base: is an electron pair donor. Example: Identify following as Lewis Acid/Base Ag + :NH 3

24 Ch. 15 Acids and Bases CH. 15 ACIDS AND BASES Arrhenius Definitions: 1) Acid: substance that when dissolved in water increases [H+] 2) Base: substance that when dissolved in water increases [OH - ] Example: HCl (Acid) NaOH (Base) Brønsted-Lowry Definitions: 1) Acid: substance that donates a proton, H+, in a reaction 2) Base: substance that accepts a proton, H+, in a reaction Example: HCl (Acid) :NH 3 (Base) Lewis Definitions: 1) Acid: is an electron pair acceptor. 2) Base: is an electron pair donor. Example: Ag + (Acid) :NH 3 (Base)

25 Ch. 15 Acids and Bases CH. 15 ACIDS AND BASES Arrhenius Definitions: 1) Acid: substance that when dissolved in water increases [H+] 2) Base: substance that when dissolved in water increases [OH - ] Example: HCl (Acid) NaOH (Base) Brønsted-Lowry Definitions: 1) Acid: substance that donates a proton, H+, in a reaction 2) Base: substance that accepts a proton, H+, in a reaction Example: HCl (Acid) :NH 3 (Base) Lewis Definitions: 1) Acid: is an electron pair acceptor. 2) Base: is an electron pair donor. Example: Ag + (Acid) :NH 3 (Base)

26 STRONG ACIDS AND BASES HNO 3 H 2 SO 4 HClO4 GROUP 1A & 2A HYDROXIDE EX: NaOH, Ca(OH) 2 EXCEPT Be(OH) 2 HCl HBr HI H 3 O + or H + Ch. 15 Acids and Bases

27 COMPARING THE STRENGTHS OF GIVEN ACIDS Binary Acids (H-NONMETAL): A. Electronegativity if same period ( EN = strength) EN increases Left to Right B. Atomic size if same group ( atomic size = strength) Atomic size increases Top to Bottom Oxacids (H-O-nonmetal): Electronegativity ( EN = Strength) EN increases Left to Right and Bottom to Top EX: EX: HOCl vs HOBr EX: HI H 2 Te vs HI vs HF Other Groups (H-O-NM-O n ): More Oxygen = Stronger Acid EX: H 3 AsO 4 vs H 3 AsO 3 Carboxylic Acids (RCOOH): A. Resonance (EN) B. Inductive Effect: distance of EN element from COOH group. (Closer = More Acidic) EX: FCH 3 COOH vs FCH 3 CH 2 CH 2 COOH Ch. 15 Acids and Bases

28 Ch. 15 Acids and Bases Strength of Conjugate Acid and Conjugate Bases Strong base gives weak CA and weak base gives strong CA Strong acid gives weak CB and weak acid gives strong CB Reaction is favored in the direction which leads to the formation of weaker acid or base (or CB and CA). Ex: Which side of the following reaction is favored? CH 3 COOH + H 2 O CH 3 COO - + H 3 O +

29 Ch. 15 Acids and Bases Strength of Conjugate Acid and Conjugate Bases Strong base gives weak CA and weak base gives strong CA Strong acid gives weak CB and weak acid gives strong CB Reaction is favored in the direction which leads to the formation of weaker acid or base (or CB and CA). Ex: Which side of the following reaction is favored? CH 3 COOH + H 2 O CH 3 COO - + H 3 O + Answer: Weak Acid Strong C.B.

30 Strength of Conjugate Acid and Conjugate Bases Strong base gives weak CA and weak base gives strong CA Strong acid gives weak CB and weak acid gives strong CB Reaction is favored in the direction which leads to the formation of weaker acid or base (or CB and CA). Ex: Which side of the following reaction is favored? CH 3 COOH + H 2 O CH 3 COO - + H 3 O + Answer: Weak Acid Strong C.B. Weak Base Strong C.A. Therefore the Reactant side (left) is Favored Ch. 15 Acids and Bases

31 1. Identify the acid and base on each side of the following equation: H 2 S + NH 3 NH HS - Ch. 15 Acids and Bases

32 Ch. 15 Acids and Bases 1. Identify the acid and base on each side of the following equation: H 2 S + NH 3 NH HS - ANSWER: Acid + Base C.A. + C.B.

33 2. Which of the following is the strongest Acid? A) HOI B) HOCl C) HOBr Ch. 15 Acids and Bases

34 Ch. 15 Acids and Bases 2. Which of the following is the strongest Acid? A) HOI C) HOBr Answer: HOCl With Oxacids (H-O-nonmetal) We use Electronegativity trend (increases bottom to top in a group) EN= Strength of Acid. EN

35 3. What is the ph of a solution prepared by dissolving mol Ba(OH) 2 in water to give 455 ml of solution? Ch. 15 Acids and Bases

36 3. What is the ph of a solution prepared by dissolving mol Ba(OH) 2 in water to give 455 ml of solution? Ch. 15 Acids and Bases

37 Ch. 15 Acids and Bases 3. What is the ph of a solution prepared by dissolving mol Ba(OH) 2 in water to give 455 ml of solution? Solution: There is more than one way to solve this mol x 2 = 0.05 mol OH mol/0.455 L = M OH - poh = -log [OH - ] poh = -log [0.1099] poh = poh + ph = 14 ph = 14 - poh ph =

38 Ch. 15 Acids and Bases 3. What is the ph of a solution prepared by dissolving mol Ba(OH) 2 in water to give 455 ml of solution? Solution: There is more than one way to solve this mol x 2 = 0.05 mol OH mol/0.455 L = M OH - poh = -log [OH - ] poh = -log [0.1099] poh = poh + ph = 14 ph = 14 - poh ph = OR M OH - K w = [H + ] [OH - ] = 1x x10-14 [H + ] = = 9.1x10-14 M H ph = -log [H + ] ph = -log [9.1x10-14 ]

39 4. A sample of milk is found to have a ph of What is the [OH - ] in this milk? Ch. 15 Acids and Bases

40 4. A sample of milk is found to have a ph of What is the [OH - ] in this milk? Ch. 15 Acids and Bases

41 Ch. 15 Acids and Bases 4. A sample of milk is found to have a ph of What is the [OH - ] in this milk? Solution: There is more than one way to solve this.. ph + poh = 14 poh = poh = 7.75 [OH - ] = 10 -poh [OH - ] = OR [H + ] = 10 -ph [H + ] = [H + ] = 5.62x10-7 K w = [H + ] [OH - ] = 1x x10-14 [OH - ] = = 5.62x10-7

42 CH. 16 ACID-BASE EQUILIBRIUM Acid ionization constant: *Lower value of pka = strong acid *Higher value of pka = weak acid Polyprotic acids: more than one ionizable proton e.g. H 2 SO 4 is diprotic and H 3 PO 4 is triprotic. In a solution there will be more than just the one conjugate acid/base pair. Base ionization constant: *Lower value of pk b = strong Base *Higher value of pk b = weak Base Ch. 16 Acid-Bases Equilibrium

43 Hydrolysis Strong Acid + Strong Base Neutral (ex. NaCl, KNO 3 ) Strong Acid + Weak Base Acidic Solution (ex. NH 4 Cl ) Weak Acid + Strong Base Basic Solution (ex. Na 2 CO 3 ) Weak Acid + Weak Base Depends on K and K b Ch. 16 Acid-Bases Equilibrium

44 Common Ion Effect The common ion in an equilibrium can shift the equilibrium to the opposite side. Ex: adding sodium acetate CH3COONa to the following reaction will increase the concentration of acetate ion thus moving the equilibrium to the left. Ch. 16 Acid-Bases Equilibrium

45 Buffers Buffers are solutions containing weak acid and its conjugate base OR weak base and its conjugate acid. The ph changes slightly with the addition of a little acid or base. Acid Base Indicators: chemicals that change color with ph. ph of buffers can be calculated using The traditional ICE method or by Henderson-Hasselbalch equation Ch. 16 Acid-Bases Equilibrium

46 Buffer Calculation: 1. What is the [H 3 O + ] for a buffer solution that is M in acid and M in the corresponding salt if the weak acid K a = 5.80 x 10 7? Ch. 16 Acid-Bases Equilibrium

47 Buffer Calculation: 1. What is the [H 3 O + ] for a buffer solution that is M in acid and M in the corresponding salt if the weak acid K a = 5.80 x 10 7? Solution: HA(aq) + H2O(l) H 3 O + (aq) + A (aq) pk a = log(5.80 x 10 7 ) = [base] = M and [acid] = M Ch. 16 Acid-Bases Equilibrium

48 Buffer Calculation: 1. What is the [H 3 O + ] for a buffer solution that is M in acid and M in the corresponding salt if the weak acid K a = 5.80 x 10 7? Solution: HA(aq) + H2O(l) H 3 O + (aq) + A (aq) pk a = log(5.80 x 10 7 ) = [base] = M and [acid] = M Ch. 16 Acid-Bases Equilibrium

49 Buffer Calculation: 1. What is the [H 3 O + ] for a buffer solution that is M in acid and M in the corresponding salt if the weak acid K a = 5.80 x 10 7? Solution: HA(aq) + H2O(l) H 3 O + (aq) + A (aq) pk a = log(5.80 x 10 7 ) = [base] = M and [acid] = M [0.600] [0.250] Ch. 16 Acid-Bases Equilibrium

50 Buffer Calculation: 1. What is the [H 3 O + ] for a buffer solution that is M in acid and M in the corresponding salt if the weak acid K a = 5.80 x 10 7? Solution: HA(aq) + H2O(l) H 3 O + (aq) + A (aq) pk a = log(5.80 x 10 7 ) = [base] = M and [acid] = M [0.600] [0.250] ph = log 2.40 ph = = [H 3 O + ] = 10 ph [H 3 O + ] = Ch. 16 Acid-Bases Equilibrium

51 Ch. 17 Solubility Equilibrium CH. 17 Solubility and Complex-Ion Equilibrium The reactant in a solubility equilibrium is a slightly soluble salt and the equilibrium constant for the reaction is the Solubility Product Constant, K sp. Solubility problems are equilibrium problems. Ex: the solubility equilibrium and K sp for the salt SrF 2 (s) are SrF 2 (s) Sr 2+ (aq) + 2 F (aq) K sp = [Sr 2+ ][F ] 2 = 2.0 x *Note that since the reactant is a Solid, its concentration Does Not appear in the K sp expression. The Molar Solubility of a salt in water can be formed by setting up an equilibrium table and solving for x. The Solubility is the same quantity expressed in g/l (rather than M = mol/l).

52 Ch. 17 Solubility Equilibrium Solubility Quotient (Q ip ) Solubility Quotient (Q ip ): determines if precipitation will occur Q ip > K sp precipitation occurs (Supersaturated) Q ip = K sp saturation of solution (Saturated) Q ip < K sp precipitation will not occur (Unsaturated) *In general very small value of K sp indicates complete precipitation)

53 Ch. 17 Solubility Equilibrium Factors Affecting Solubility Common ion effect: Addition of an ion common to a solubility equilibrium will reduce solubility. *Le Châtelier s Principle. Ex: SrF 2 (s) Sr 2+ (aq) + 2 F (aq) Adding fluoride ion, F (aq), to the SrF 2 (s) equilibrium above will shift it left. The shift will increase the amount of SrF 2 (s) in solid form, and thus decrease solubility. Effect of ph on solubility: ph of a solution will affect solubility if the conjugate ion (acid or base) is acidic or basic. Ex: Cl - is very weak conjugate base (CB) and is not considered basic, whereas HCO3 - is a weak CB whose solubility is affected by the ph. *An Anion (CB) of a weak Acid is more soluble in Acidic solutions.

54 Ch. 17 Solubility Equilibrium Comparing Precipitation Of Given Salts If two precipitates are possible, the least soluble salt will precipitate first (the one with the smaller K sp ). Ex: If you add NaOH(aq) to a solution containing equal amounts of Ca 2+ and Mg 2+ *Mg(OH) 2 (s) will precipitate before Ca(OH) 2 (s) since K sp (Mg(OH) 2 ) = 1.2 x < K sp (Ca(OH) 2 ) = 8.0 x 10-6

55 Common Ion Effect: 1. What would be the molar solubility of SrF 2 (s) in a 0.10 M NaF(aq) solution? K sp = 2.0 x Ch. 17 Solubility Equilibrium

56 Ch. 17 Solubility Equilibrium Common Ion Effect: 1. What would be the molar solubility of SrF 2 (s) in a 0.10 M NaF(aq) solution? K sp = 2.0 x We set up an equilibrium (ICE) table, but now we have an initial concentration of fluoride ion:

57 Ch. 17 Solubility Equilibrium Common Ion Effect: 1. What would be the molar solubility of SrF 2 (s) in a 0.10 M NaF(aq) solution? K sp = 2.0 x Balanced Equation SrF 2 (s) Sr 2+ (aq) + 2 F (aq) Initial (M) Change (M) +x +2x Equilibrium (M) x ( x)

58 Ch. 17 Solubility Equilibrium Common Ion Effect: 1. What would be the molar solubility of SrF 2 (s) in a 0.10 M NaF(aq) solution? K sp = 2.0 x Balanced Equation SrF 2 (s) Sr 2+ (aq) + 2 F (aq) Initial (M) Change (M) +x +2x Equilibrium (M) x ( x) We next use the equilibrium concentrations in the table and the K sp value given above, and solve for x. [0.10/ 2.0 x ] = 500,000,000 >>>>1000 Note that since x is small, ( x) ~ 0.10

59 Ch. 17 Solubility Equilibrium Common Ion Effect: 1. What would be the molar solubility of SrF 2 (s) in a 0.10 M NaF(aq) solution? K sp = 2.0 x Balanced Equation SrF 2 (s) Sr 2+ (aq) + 2 F (aq) Initial (M) Change (M) +x +2x Equilibrium (M) x ( x) We next use the equilibrium concentrations in the table and the K sp value given above, and solve for x. [0.10/ 2.0 x ] = 500,000,000 >>>>1000 Note that since x is small, ( x) ~ 0.10 K sp = [Sr 2+ ][F ] x = (x)( 0.10) x = (x)( 0.10) x = x

60 2. Which of the following salts is most soluble in pure water? A) HgS, K sp = 2.0 x B) AgI, K sp = 8.5 x C) PbI 2, K sp = 7.1 x 10-9 D) CuS, K sp = 8.7 x E) ZnS, K sp =1.6 x 10 4 Ch. 17 Solubility Equilibrium

61 Ch. 17 Solubility Equilibrium 2. Which of the following salts is most soluble in pure water? A) HgS, K sp = 2.0 x B) AgI, K sp = 8.5 x C) PbI 2, K sp = 7.1 x 10-9 D) CuS, K sp = 8.7 x E) ZnS, K sp =1.6 x 10 4 The higher the K sp, the more soluble it would be.

62 Ch. 17 Solubility Equilibrium 2. Which of the following salts is most soluble in pure water? A) HgS, K sp = 2.0 x B) AgI, K sp = 8.5 x D) CuS, K sp = 8.7 x E) ZnS, K sp =1.6 x 10 4 The higher the K sp, the more soluble it would be.

63 CH. 19 Electrochemistry Galvanic cell is Spontaneous E cell > 0 G < 0 Ch. 19 Electrochemistry

64 Galvanic/Voltaic Cells Galvanic/Voltaic Cells: A cell that has a spontaneous redox reaction. The terminology of a cell are: Electrode : a metal piece at which the electrochemical reaction takes place. Anode: where oxidation (loss of e - ) occurs. (AN OX) Cathode: where reduction (gain of e - ) occurs. (RED CAT) Half-cell: the reduction or the oxidation part of the cell. Coulomb (C): the unit of electric charge. Volt (V): one joule per coulomb. Voltmeter: measures volts. Cell potential (E cell ): electro-potential difference that moves the electrons from the anode to cathode. *Electrons flow from Anode to Cathode (Mnemonic: A to C in alphabetical order) Galvanic cell is Spontaneous E cell > 0 G < 0 Ch. 19 Electrochemistry

65 Ch. 19 Electrochemistry Standard Electrode Potential: the tendency for reduction to occur at an electrode under the conditions of SHE. More More + - Reduction Potential = Oxidizing Agent = Reduction Reduction Potential = Reducing Agent = Oxidation *Reduction potential = potential of the reduction half reaction. *Oxidation potential = potential of the oxidation half reaction = reverse the sign of the reduction potential. Standard Cell Potential: E o cell = E o (cathode) E o (anode) E o cell = E o (right) E o (left)

66 Ch. 19 Electrochemistry Oxidation-Reduction Oxidation Losing Electrons Reducing Agent Increases In Charge Reduction Gaining Electrons Oxidizing Agent Decreases In Charge

67 1. Identify the following two reactions: A) 1 is oxidation, 2 is reduction B) 1 is reduction, 2 is oxidation C) Neither D) Both oxidation E) Both reduction 1) Cu(s) Cu 2+ (aq) + 2e - 2) 2 Ag + (aq) + 2e - 2 Ag(s) Ch. 19 Electrochemistry

68 1. Identify the following two reactions: 1) Cu(s) Cu 2+ (aq) + 2e - 2) 2 Ag + (aq) + 2e - 2 Ag(s) B) 1 is reduction, 2 is oxidation C) Neither D) Both oxidation E) Both reduction LeO GeR Ch. 19 Electrochemistry

69 2. The following questions are about this cell: Al Al +3 Pb +2 Pb a. Identify the anode and the cathode. b. Write the balanced overall reaction. c. What is the potential of this cell under standard conditions?

70 2. The following questions are about this cell: Al Al +3 Pb +2 Pb a. Identify the anode and the cathode. b. Write the balanced overall reaction. c. What is the potential of this cell under standard conditions? Solution: a. An Ox, LEO (Anode Oxidation, Lose e- Oxidation) Al loses e- and it is on the left, therefore it is the Anode

71 2. The following questions are about this cell: Al Al +3 Pb +2 Pb a. Identify the anode and the cathode. b. Write the balanced overall reaction. c. What is the potential of this cell under standard conditions? Solution: a. An Ox, LEO (Anode Oxidation, Lose e- Oxidation) Al loses e- and it is on the left, therefore it is the Anode Red Cat, GeR (Reduction Cathode, Gain e- Reduction) Pb gain e- and it is on the right, therefore it is the cathode

72 2. The following questions are about this cell: Al Al +3 Pb +2 Pb a. Identify the anode and the cathode. b. Write the balanced overall reaction. c. What is the potential of this cell under standard conditions? Solution: a. An Ox, LEO (Anode Oxidation, Lose e- Oxidation) Al loses e- and it is on the left, therefore it is the Anode Red Cat, GeR (Reduction Cathode, Gain e- Reduction) Pb gain e- and it is on the right, therefore it is the cathode b. 2Al + 3Pb +2 2Al Pb

73 2. The following questions are about this cell: Al Al +3 Pb +2 Pb a. Identify the anode and the cathode. b. Write the balanced overall reaction. c. What is the potential of this cell under standard conditions? Solution: a. An Ox, LEO (Anode Oxidation, Lose e- Oxidation) Al loses e- and it is on the left, therefore it is the Anode Red Cat, GeR (Reduction Cathode, Gain e- Reduction) Pb gain e- and it is on the right, therefore it is the cathode b. 2Al + 3Pb +2 2Al Pb c. E o cell = E o (cathode) E o (anode) E o cell = E o (right) E o (left) E o cell = (-0.13) (-1.66)

74 Ch. 19 Electrochemistry Oxidation- Reduction Reactions in Acidic/Basic Solutions Balance the following redox reactions (a) give the balanced half-reactions; identify the oxidation half-reaction and the reduction half-reaction. (b) give the balanced net reaction. (c) identify the oxidizing agent and the reducing agent. Cl 2 (g) + S 2 O 3 (aq) Cl - (aq) + SO4 (aq) in acid solution.

75 Ch. 19 Electrochemistry Oxidation- Reduction Reactions in Acidic/Basic Solutions Balance the following redox reactions (a) give the balanced half-reactions; identify the oxidation half-reaction and the reduction half-reaction. (b) give the balanced net reaction. (c) identify the oxidizing agent and the reducing agent. Cl 2 (g) + S 2 O 3 (aq) Cl - (aq) + SO4 (aq) in acid solution. 1. Assign Oxidation numbers and determine which is oxidized and which is reduced Cl2(g) + S 2 O 3 (aq) Cl (aq) + SO4(aq) Cl : 0-1 (reduced) S : (Oxidized) S 2 O 3 2S + 3O = 2S + 3() = 2S - 6 = 2S = +4 S = +2 SO 4 S + 4O = S + 4() = S - 8 = S = +6 S = Split into two half reactions (Oxidation and Reduction) S 2 O 3 (aq) SO4 (aq) Cl 2 (g) Cl - (aq)

76 Ch. 19 Electrochemistry 3. Balance both half Reactions 1) Balance all atoms except H and O S 2 O 3 (aq) 2 SO4 (aq) Cl 2 (g) 2 Cl - (aq) 2) Balance O atoms by adding H20 to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) 3) Balance H atoms by adding H + ions to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H + 4) Balance electric charge by adding electrons (e-) to the more positive side S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- Cl 2 (g) + 2 e- 2 Cl - (aq)

77 3. Balance both half Reactions 1) Balance all atoms except H and O S 2 O 3 (aq) 2 SO4 (aq) Cl 2 (g) 2 Cl - (aq) 2) Balance O atoms by adding H20 to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) 3) Balance H atoms by adding H + ions to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H + 4) Balance electric charge by adding electrons (e-) to the more positive side S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- Cl 2 (g) + 2 e- 2 Cl - (aq) 4. Combine the two half reactions and obtain a final balanced equation a. Multiply each half-reaction by a factor to make the number of electrons equal in both reactions so when added electrons cancel out S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- x4 (Cl 2 (g) + 2 e- 2 Cl - (aq)) 4 Cl 2 (g) + 8 e- 8 Cl - (aq) b. Simplify the balanced equation S 2 O 3 (aq) + 5 H Cl2 (g) 2 SO4 (aq) + 10 H + (aq) + 8 Cl - (aq) Ch. 19 Electrochemistry

78 3. Balance both half Reactions 1) Balance all atoms except H and O S 2 O 3 (aq) 2 SO4 (aq) Cl 2 (g) 2 Cl - (aq) 2) Balance O atoms by adding H20 to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) Oxidizing Agent? Reducing Agent? 3) Balance H atoms by adding H + ions to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H + 4) Balance electric charge by adding electrons (e-) to the more positive side S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- Cl 2 (g) + 2 e- 2 Cl - (aq) 4. Combine the two half reactions and obtain a final balanced equation a. Multiply each half-reaction by a factor to make the number of electrons equal in both reactions so when added electrons cancel out S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- x4 (Cl 2 (g) + 2 e- 2 Cl - (aq)) 4 Cl 2 (g) + 8 e- 8 Cl - (aq) b. Simplify the balanced equation S 2 O 3 (aq) + 5 H Cl2 (g) 2 SO4 (aq) + 10 H + (aq) + 8 Cl - (aq) Ch. 19 Electrochemistry

79 Ch. 19 Electrochemistry 3. Balance both half Reactions 1) Balance all atoms except H and O S 2 O 3 (aq) 2 SO4 (aq) Cl 2 (g) 2 Cl - (aq) 2) Balance O atoms by adding H20 to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) 3) Balance H atoms by adding H + ions to one side of the equation S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H + 4) Balance electric charge by adding electrons (e-) to the more positive side S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- Oxidizing Agent? Reducing Agent? Cl 2 (g) S 2 O 3 (aq) Cl 2 (g) + 2 e- 2 Cl - (aq) 4. Combine the two half reactions and obtain a final balanced equation a. Multiply each half-reaction by a factor to make the number of electrons equal in both reactions so when added electrons cancel out S 2 O 3 (aq) + 5 H20 2 SO4 (aq) + 10 H e- x4 (Cl 2 (g) + 2 e- 2 Cl - (aq)) 4 Cl 2 (g) + 8 e- 8 Cl - (aq) b. Simplify the balanced equation S 2 O 3 (aq) + 5 H Cl2 (g) 2 SO4 (aq) + 10 H + (aq) + 8 Cl - (aq)

80 If this was asking to balance in Basic solution, then there are two more steps. 5. Add as many OH - ions to both sides of the equation as there H + ions. S 2 O 3 (aq) + 5 H Cl2 (g) 2 SO4 (aq) + 10 H + (aq) + 8 Cl - (aq) + 10 OH - (aq) 6. each added OH - will react with H + to form H 2 O S 2 O 3 (aq) + 5 H Cl 2 (g) 2 SO4 (aq) + 10 H Cl - (aq) *simplify the equation S 2 O 3 (aq) + 4 Cl2 (g) 2 SO4 (aq) + 5 H Cl - (aq) Ch. 19 Electrochemistry

81 Bibliography Ebbing, D. D., & Gammon, S. D. (2013). General Chemistry. Cengage Learning. General Chemistry Course Information. (2014). Retrieved from Dr. Sapna Gupta:

Contents and Concepts

Contents and Concepts Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid

More information

Chem1120pretest2Summeri2015

Chem1120pretest2Summeri2015 Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has

More information

Chem1120pretest2Summeri2015

Chem1120pretest2Summeri2015 Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward

More information

Chapter Test A. Chapter: Chemical Equilibrium

Chapter Test A. Chapter: Chemical Equilibrium Assessment Chapter Test A Chapter: Chemical Equilibrium In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. A 15.0 ml volume

More information

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion. Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when

More information

Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33

Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with

More information

Acids and Bases Unit 11

Acids and Bases Unit 11 Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid

More information

Chap 16 Chemical Equilibrium HSU FUYIN

Chap 16 Chemical Equilibrium HSU FUYIN Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen

More information

Chemical Equilibrium

Chemical Equilibrium Chemical Equilibrium Many reactions are reversible, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product

More information

Chapter 14. Objectives

Chapter 14. Objectives Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly

More information

CHEMpossible. Final Exam Review

CHEMpossible. Final Exam Review CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a

More information

Dynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state

Dynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state CHEMISTRY 111 LECTURE EXAM III Material PART 1 CHEMICAL EQUILIBRIUM Chapter 14 I Dynamic Equilibrium I. In a closed system a liquid obtains a dynamic equilibrium with its vapor state Dynamic equilibrium:

More information

Acids and Bases. Feb 28 4:40 PM

Acids and Bases. Feb 28 4:40 PM Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to

More information

CHEM Dr. Babb s Sections Exam #3 Review Sheet

CHEM Dr. Babb s Sections Exam #3 Review Sheet CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry

More information

Unit 2 Acids and Bases

Unit 2 Acids and Bases Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions

More information

Chemical Equilibrium

Chemical Equilibrium Chemical Equilibrium Equilibrium Constants For a generic chemical reaction, the equilibrium constant is defined as: aa + bb cc + dd (1) The equilibrium constant, K eq, for a chemical reaction indicates

More information

CHAPTER-7 EQUILIBRIUM ONE MARK QUESTIONS WITH ANSWERS. CHAPTER WEIGHTAGE: 13

CHAPTER-7 EQUILIBRIUM ONE MARK QUESTIONS WITH ANSWERS. CHAPTER WEIGHTAGE: 13 CHAPTER-7 EQUILIBRIUM ONE MARK QUESTIONS WITH ANSWERS. CHAPTER WEIGHTAGE: 13 1.What is a reversible reaction? Ans. The reaction in which both forward and backward reaction takes place simultaneously is

More information

Chemistry 12. Resource Exam B. Exam Booklet

Chemistry 12. Resource Exam B. Exam Booklet Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART

More information

Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.

Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You

More information

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a

More information

(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or

(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH

More information

Chemical Equilibrium. Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B

Chemical Equilibrium. Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B Chemical Equilibrium Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product formation,

More information

Chem1120pretest2Summeri2016

Chem1120pretest2Summeri2016 Chem1120pretest2Summeri2016 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has

More information

Part 01 - Assignment: Introduction to Acids &Bases

Part 01 - Assignment: Introduction to Acids &Bases Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4

More information

ACID BASE EQUILIBRIUM

ACID BASE EQUILIBRIUM ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric

More information

General Chemistry II CHM 1046 E Exam 2

General Chemistry II CHM 1046 E Exam 2 General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of

More information

Chemical Equilibrium. What is the standard state for solutes? a) 1.00 b) 1 M c) 100% What is the standard state for gases? a) 1 bar b) 1.

Chemical Equilibrium. What is the standard state for solutes? a) 1.00 b) 1 M c) 100% What is the standard state for gases? a) 1 bar b) 1. Chemical Equilibrium Equilibrium constant for the reaction: aa + bb + cc + dd + [C ] c [D ] d... equilibrium constant K = [ A] a [B ] b... [] = concentration relative to standard state molarity (M): for

More information

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species 3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates

More information

I. Multiple Choice Questions (Type-I) is K p

I. Multiple Choice Questions (Type-I) is K p Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl

More information

Chapter 16 Acid Base Equilibria

Chapter 16 Acid Base Equilibria Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar

More information

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

All answers are to be done on test paper. If more room is needed use the back side of the paper and indicate.

All answers are to be done on test paper. If more room is needed use the back side of the paper and indicate. 1 Chem 1105-Final Exam Date: August 10, 2016 Instructor: Calvin Howley Time Period: 3 hour Student: Student #: Instructions: Please turn off all cell phones. Only scientific calculators are allowed in

More information

Chapter 10. Acids, Bases, and Salts

Chapter 10. Acids, Bases, and Salts Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and

More information

CHEMISTRY Matter and Change

CHEMISTRY Matter and Change CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen

More information

Grace King High School Chemistry Test Review

Grace King High School Chemistry Test Review CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),

More information

Chapter 10 - Acids & Bases

Chapter 10 - Acids & Bases Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic

More information

Acids Bases and Salts Acid

Acids Bases and Salts Acid Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic

More information

Chem Midterm 4 May 14, 2009

Chem Midterm 4 May 14, 2009 Chem. 101 - Midterm 4 May 14, 009 Name All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures. Only

More information

Properties of Acids and Bases

Properties of Acids and Bases Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus

More information

Chapter 14 Acid- Base Equilibria Study Guide

Chapter 14 Acid- Base Equilibria Study Guide Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and

More information

Part A: Multiple Choice (23 marks total)

Part A: Multiple Choice (23 marks total) Part A: Multiple Choice (23 marks total) Use the answer sheet found at the end of this examination to answer the multiple-choice questions in this section. Shade in the circle that corresponds to your

More information

Advanced Placement Chemistry Chapters Syllabus

Advanced Placement Chemistry Chapters Syllabus As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and

More information

Chapter 4. Reactions in Aqueous Solution

Chapter 4. Reactions in Aqueous Solution Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is

More information

CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).

CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ). CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).

More information

Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria

Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good

More information

Name Date Class ACID-BASE THEORIES

Name Date Class ACID-BASE THEORIES 19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary

More information

Acid / Base Properties of Salts

Acid / Base Properties of Salts Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,

More information

49 56 (8 Q's) Solutions YOU WILL SKIP THIS SECTION ENTIRELY (8 Q's) Organic Chemistry 12 none

49 56 (8 Q's) Solutions YOU WILL SKIP THIS SECTION ENTIRELY (8 Q's) Organic Chemistry 12 none ACS Standardized Exam for CHM 122 Breakdown of Questions by Topic Question # Topic Covered Problem Set Section in ACS Book 1 12 (12 Q's) Kinetics 1, 2 Dynamics 13 24 (12 Q's) Equilibrium 3, 4, 5, 6, 7

More information

Acids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Acids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain

More information

Chemical Equilibrium Chapter 6

Chemical Equilibrium Chapter 6 Chemical Equilibrium Chapter 6 "When a system is in chemical equilibrium, a change in one of the parameters of the equilibrium produces a shift in such a direction that, were no other factors involved

More information

*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base.

*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base. 16.2 Bronsted-Lowry Acids and Bases An acid is a substance that can transfer a proton to another substance. A base is a substance that can accept a proton. A proton is a hydrogen ion, H +. Proton transfer

More information

Chapter 15 - Applications of Aqueous Equilibria

Chapter 15 - Applications of Aqueous Equilibria Neutralization: Strong Acid-Strong Base Chapter 15 - Applications of Aqueous Equilibria Molecular: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) SA-SB rxn goes to completion (one-way ) Write ionic and net ionic

More information

What is the correct name and bonding of BF 3? What is the correct name and bonding of BF 3?

What is the correct name and bonding of BF 3? What is the correct name and bonding of BF 3? What is the correct name and bonding of BF 3? 1. boron trifluoride, covalent compound 2. boron trifluoride, ionic compound 3. boron fluoride, covalent compound 4. boron fluoride, ionic compound What is

More information

5/10/2017. Chapter 10. Acids, Bases, and Salts

5/10/2017. Chapter 10. Acids, Bases, and Salts Chapter 10. Acids, Bases, and Salts Introduction to Inorganic Chemistry Instructor Dr. Upali Siriwardane (Ph.D. Ohio State) E-mail: upali@latech.edu Office: 311 Carson Taylor Hall ; Phone: 318-257-4941;

More information

Chapter 16 Acids and Bases. Chapter 16 Acids and Bases

Chapter 16 Acids and Bases. Chapter 16 Acids and Bases . Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases

More information

Chapter Test B. Chapter: Chemical Equilibrium. following equilibrium system? 2CO(g) O 2 (g) ^ 2CO 2 (g)

Chapter Test B. Chapter: Chemical Equilibrium. following equilibrium system? 2CO(g) O 2 (g) ^ 2CO 2 (g) Assessment Chapter Test B Chapter: Chemical Equilibrium PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. What is

More information

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH

More information

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1

11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1 11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing

More information

Unit 9. Acids, Bases, & Salts Acid/Base Equilibrium

Unit 9. Acids, Bases, & Salts Acid/Base Equilibrium Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals

More information

CHEM 1412 Zumdahl & Zumdahl Practice Exam II (Ch. 14, 15 & 16) Multiple Choices: Please select one best answer. Answer shown in bold.

CHEM 1412 Zumdahl & Zumdahl Practice Exam II (Ch. 14, 15 & 16) Multiple Choices: Please select one best answer. Answer shown in bold. CHEM 1412 Zumdahl & Zumdahl Practice Exam II (Ch. 14, 15 & 16) Multiple Choices: Please select one best answer. Answer shown in bold. 1. Consider the equilibrium: PO -3 4 (aq) + H 2 O (l) HPO 2-4 (aq)

More information

Acids and Bases. Properties, Reactions, ph, and Titration

Acids and Bases. Properties, Reactions, ph, and Titration Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some

More information

Name%% %Period%% % Precipitation+Reaction+Practice+

Name%% %Period%% % Precipitation+Reaction+Practice+ Name%% %Period%% % Precipitation+Reaction+Practice+ 1.%Write%a%balanced%equation%for%the%following%precipitation%reactions,%circle%the%precipitate%that%is% formed:% a) K 3 PO 4 %+%3%Sr(NO 3 ) 2 %% % %

More information

PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS

PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE APRIL 1996 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN)

More information

Chapter 9. Aqueous Solutions and Chemical Equilibria. Classifying Solutions of Electrolytes

Chapter 9. Aqueous Solutions and Chemical Equilibria. Classifying Solutions of Electrolytes Chapter 9 Aqueous Solutions and Chemical Equilibria Classifying Solutions of Electrolytes Electrolytes solutes form ions when dissolved in water (or certain other solvents, e.g. acetonitrile) Strong (weak,

More information

Chapter 16. Acid-Base Equilibria

Chapter 16. Acid-Base Equilibria Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An

More information

Chemistry 12 AUGUST Course Code = CH. Student Instructions

Chemistry 12 AUGUST Course Code = CH. Student Instructions MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2001 Ministry of Education AUGUST 2001 Course

More information

Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions

Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions When a system reaches equilibrium, the [products] and [reactants] remain constant. A + B C + D [5M] [2M] [3M] [1.5M] Rate fwd = Rate rev

More information

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate

More information

ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA

ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while

More information

Unit Nine Notes N C U9

Unit Nine Notes N C U9 Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release

More information

Acids, Bases and Salts

Acids, Bases and Salts (Hebden Unit 4 page 109 182) 182) We will cover the following topics: 1. Definition of Acids and Bases 2. Bronsted-Lowry Acids and Bases 2 1 Arrhenius Definition of Acids and Bases An acid is a substance

More information

15/04/2018 EQUILIBRIUM- GENERAL CONCEPTS

15/04/2018 EQUILIBRIUM- GENERAL CONCEPTS 15/04/018 EQUILIBRIUM- GENERAL CONCEPTS When a system is at equilibrium, the forward and reverse reactions are proceeding at the same rate. The concentrations of all species remain constant over time,

More information

Chapter 14. Acids and Bases

Chapter 14. Acids and Bases Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton

More information

SCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm?

SCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm? SCH4U_08-09 SCH4U: EXAM REVIEW 1. The heat of a reaction is equal to: a. enthalpy (products) + enthalpy (reactants) b. enthalpy (reactants) enthalpy (products) c. enthalpy (products) enthalpy (reactants)

More information

Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs.

Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs. Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs. Ch 18 - Acids and Bases I CAN: 1) Compare properties of acids

More information

Exam 2 Practice (Chapter 15-17)

Exam 2 Practice (Chapter 15-17) Exam 2 Practice (Chapter 15-17) 28. The equilibrium constant Kp for reaction (1) has a value of 0.112. What is the value of the equilibrium constant for reaction (2)? (1) SO2 (g) + 1/2 O2(g) SO3 (g) Kp

More information

Chapter 4 - Types of Chemical Reactions and Solution Chemistry

Chapter 4 - Types of Chemical Reactions and Solution Chemistry Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly

More information

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many

More information

Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions

Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions Chapter 12: Chemical Equilibrium The Extent of Chemical Reactions When a system reaches equilibrium, the [products] and [reactants] remain constant. A + B C + D [5M] [2M] [3M] [1.5M] Rate fwd = Rate rev

More information

Chemistry I Notes Unit 10: Acids and Bases

Chemistry I Notes Unit 10: Acids and Bases Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,

More information

EQUILIBRIUM GENERAL CONCEPTS

EQUILIBRIUM GENERAL CONCEPTS 017-11-09 WHEN THE REACTION IS IN EQUILIBRIUM EQUILIBRIUM GENERAL CONCEPTS The concentrations of all species remain constant over time, but both the forward and reverse reaction never cease When a system

More information

Chapter 10. Acids and Bases

Chapter 10. Acids and Bases Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.

More information

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any

More information

Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)

Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers

More information

Chemistry 12 JANUARY Course Code = CH. Student Instructions

Chemistry 12 JANUARY Course Code = CH. Student Instructions MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education JANUARY 2002 Course

More information

Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta

Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical

More information

Chemical Equilibrium

Chemical Equilibrium Chemical Equilibrium Ch 17 Apr 28 7:40 AM A Reversible reaction is a chemical reaction that can occur in both the forward and the reverse directions N 2 (g) + 3 H 2 (g) 2NH3(g) Apr 16 1:21 PM 1 Equilibrium

More information

ph = pk a + log 10 {[base]/[acid]}

ph = pk a + log 10 {[base]/[acid]} FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt

More information

Chapter 7 Acids and Bases

Chapter 7 Acids and Bases Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7

More information

Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Page 1 of 20 Chapter 16 Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids: taste sour and cause certain dyes to change color. Bases: taste bitter and feel soapy. Arrhenius concept o acids

More information

Chem Practice Exam Two (Chapters 19, 20 and 21)

Chem Practice Exam Two (Chapters 19, 20 and 21) Chem 203 - Practice Exam Two (Chapters 19, 20 and 21) 1. Consider the dissolution of MnS in water (K sp = 3.0 10 14 ). MnS(s) + H 2O(l) Mn 2+ (aq) + HS (aq) + OH (aq) How is the solubility of manganese(ii)

More information

Acids, Bases and Buffers

Acids, Bases and Buffers 1 Acids, Bases and Buffers Strong vs weak acids and bases Equilibrium as it relates to acids and bases ph scale: [H+(aq)] to ph, poh, etc ph of weak acids ph of strong acids Conceptual about oxides (for

More information

Chapter 17: Additional Aspects of Aqueous equilibria. Common-ion effect

Chapter 17: Additional Aspects of Aqueous equilibria. Common-ion effect Chapter 17: Additional Aspects of Aqueous equilibria Learning goals and key skills: Describe the common ion effect. Explain how a buffer functions. Calculate the ph of a buffer solution. Calculate the

More information

Chem 1046 Lecture Notes Chapter 17

Chem 1046 Lecture Notes Chapter 17 Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that

More information

Name. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com

Name. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com Periodic Table Name Academic Chemistry Acids & Bases Notes Unit #14 Test Date: 20 cincochem.pbworks.com Acid Base cincochem.pbworks.com Notes Find ph To go from [H 3 O + ] to ph EXAMPLE: [H 3 O + ] = 3.23

More information

CHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:

CHEM 200/202. Professor Jing Gu Office: EIS-210. All  s are to be sent to: CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS

More information

10.1 Acids and Bases in Aqueous Solution

10.1 Acids and Bases in Aqueous Solution 10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces

More information

HA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]

HA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ] 16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H

More information

Chem 105 Tuesday March 8, Chapter 17. Acids and Bases

Chem 105 Tuesday March 8, Chapter 17. Acids and Bases Chem 105 Tuesday March 8, 2011 Chapter 17. Acids and Bases 1) Define Brønsted Acid and Brønsted Base 2) Proton (H + ) transfer reactions: conjugate acid-base pairs 3) Water and other amphiprotic substances

More information