CHEM Dr. Babb s Sections Exam #3 Review Sheet
|
|
- Crystal Waters
- 6 years ago
- Views:
Transcription
1 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 acid and BronstedLowry base Identify the Lewis acids and bases in the following reactions. A. BCl 3 + NH 3 < > Cl 3 BNH 3 B. H + + H 2 O < > H 3 O + C. H + + OH < > H 2 O D. Ag+ + 2 NH 3 < > [Ag(NH 3 ) 2 ] Identify the BronstedLowry acids and bases in the following reactions. A. HCO 3 + H 2 O < > H 2 CO 3 + OH B. HCO H 2 O < > CO 3 + H 2 O C. 2 HPO 4 + H 2 PO 4 3 < > PO 4 + H 3 PO 4 D. HCO NaOH < > CO 3 + H 2 O + Na Does H + exist alone in solution? How is H + usually written in acid/base equilibrium? 115. What is a conjugate acid/base pair? How does an acid differ from its conjugate base? How does a base differ from its conjugate acid? 116. For the reaction below, identify the conjugate acid/base pairs. HC 2 H 3 O 2 (aq) + H 2 O < > C 2 H 3 O 2 (aq) + H 3 O + (aq) 117. Give the conjugate acid and conjugate base of each of the following species: NH 3, HSO 4, CO 2 3, and H 2 O Does a strong acid have a strong or weak conjugate base? Does a weak acid have a strong or weak conjugate base? Does a strong base have a strong or weak conjugate acid? Does a weak base have a strong or weak conjugate acid? 119. In an acid/base reaction, to tell which way the equilibrium lies we look at the relative strengths of the two bases involved. Which base gets the H +, the stronger or the weaker base? Which way does the equilibrium lie for the following two reactions? A. HCl + H 2 O < > H 3 O + + Cl B. HC 2 H 3 O 2 (aq) + H 2 O < > C 2 H 3 O 2 (aq) + H 3 O + (aq) K W, ph, poh, K A and K B, Calculation of ph for Strong and Weak Acids and Bases 120. Write the reaction for the dissociation of water. Write the form for the ion product constant of water, K w. What does the value of K w depend on? What are the equilibrium concentrations of H 3 O + and OH in pure water? 121. Define an acidic, basic and neutral solution in terms of the concentrations of H 3 O + and OH If [H 3 O + ]= M, what is the [OH ]? If [OH ]= M, what is the [H 3 O + ]? 123. Write the equations used to calculate ph, poh and pk w. Write the equation that relates ph, poh, and pk w A ph>7 indicates what type of solution, acidic, basic or neutral? A ph<7 indicates what type of solution, acidic, basic or neutral? A ph=7 indicates what type of solution? 125. A. A ph=5.17 indicates what type of solution, acidic, basic or neutral? A poh=8.9 indicates what type of solution, acidic, basic or neutral? A ph=7 indicates what type of solution? B. Which of the solutions shown below is basic? A solution with... i. ph=6.5 iii. [H 3 O + ]= ii. poh=5.5 iv. [OH ]= What is K A? Write the equation that goes along with K A for HCl and HC 2 H 3 O 2. What does K A tell us about the strength of an acid? If K A is small (10 3 ) is the acid weak or strong?
2 127. What is K B? Write the equation that goes along with K B for NH 3. What does K B tell us about the strength of a base? If K B is small (10 3 ) is the base weak or strong? 128. Calculate the [H 3 O + ], [OH ], ph and poh for a 0.25 M HClO 4 solution Calculate the [H 3 O + ], [OH ], ph and poh for a M Ba(OH) 2 solution Calculate the ph of a M HCl solution Calculate the ph of a M Ca(OH) 2 solution Calculate the [H 3 O + ], [OH ], ph, poh and percent ionization for a M HF solution. (K A (HF)= ) 133. The weak acid formic acid HCOOH has a ph of 2.14 when the concentration of HCOOH is 0.30 M. What is the value for the aciddissociation constant K A and what is the percent dissociation of the HCOOH? 134. Calculate the [H 3 O + ], [OH ], ph, poh and percent ionization for a 0.75 M NH 3 solution. (K B (NH 3 )= ) 135. A. Write all of the equilibrium equations established in a solution of 0.25 M H 2 SO 3 and calculate the ph of the solution. (K A1 = ; K A2 = ) B. Write all of the equilibrium equations established in a solution of 0.25 M H 3 PO 4 and calculate the ph of the solution. (K A1 = ; K A2 = ; K A3 = ) Hydrolysis of Salts 136. When a salt is dissolved in water (this process is called hydrolysis of the salt) is the ph of the resulting solution always neutral? 137. The general formula for formation of the salt is ACID + BASE > SALT + H 2 O. Where does the anion of the salt come from, the acid or the base? Where does the cation of the salt come from, the acid or the base? 138. A salt that contains the cation from a strong base and the anion from a strong acid will dissolve in water to give a neutral solution. Explain why using NaCl A salt that contains the cation of a weak base and the anion from a strong acid will dissolve in water to give an acidic solution. Explain why using chemical equations for NH 4 Cl A salt that contains the cation of a strong base and the anion from a weak acid will dissolve in water to give a basic solution. Explain why using chemical equations for KNO A salt that contains a small, highly charged metal cation and the anion from a strong acid will dissolve in water to give an acidic solution. Explain why using chemical equations for AlCl When the following salts are dissolved in water, will the resulting solutions be acidic, basic or neutral. A. KC 2 H 3 O 2 D. NaF G. Zn(NO 3 ) 2 B. NH 4 Br E. K 2 CO 3 H. FeCl 2 C. KClO 4 F. AlBr To do problem 144, K B of F (the conjugate base of HF) is needed. Show how K A for HF and K B for F can be related by K w Calculate the ph of a 0.45 M NaF solution. K A (HF)= HINT: First predict whether this solution should be acidic, basic or neutral. Second write the equations for dissociation of the salt and any equilibrium established. Third calculate either K A or K B for the equilibrium Calculate the ph of 0.75 M NH 4 ClO 4. K B (NH 3 )= HINT: First predict whether this solution should be acidic, basic or neutral. Second, write the equations for dissociation of the salt and any equilibrium established. Third, calculate either K A or K B for the equilibrium. Strength of Acids 146. How does the strength of binary acids (consisting of H and some other nonmetal element)
3 vary within a group? Why? Arrange the following in order of increasing acid strength: HCl, HF, HI, and HBr. Arrange the following in order of increasing acid strength: H 2 S, H 2 Te, and H 2 O How does the strength of binary acids vary within a row? Why? Arrange the following in order of increasing acid strength: HF, H 2 O, NH 3, and CH How does the strength of oxyacids (consisting of H, O and some other element) vary within a series? Arrange the following in order of increasing acid strength: HClO. HClO 3, HClO 2, and HClO 4. How does the strength of an oxyacid vary with the electronegativity of the central atom? Arrange the following in order of increasing acid strength: HOBr, HOCl, and HOI Which of the following equilibria lie mostly on the product side (ie. in an equilibrium mixture which one has product concentrations > reactant concentrations) A. HF + Br < > HBr + F D. H 2 O + H 2 O < > OH + H 3 O + B. NH 2 + H 2 O < > NH 3 + OH E. HBrO 3 + IO 3 < > BrO 3 + HIO 3 C. HClO + ClO 2 < > ClO + HClO 2 Neutralization, Common Ion Effect and Buffers 150. When a strong acid is neutralized by a strong base is the neutralization complete? Write the neutralization reaction for HNO 3 and KOH. What is the value of K n (equilibrium constant for neutralization)? If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic or neutral? 151. When a weak acid is neutralized by a strong base is the neutralization complete? Write the neutralization reaction for HF and KOH. What is the value of K n (equilibrium constant for neutralization)? (K A (HF)= ) If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic or neutral? 152. When a strong acid is neutralized by a weak base is the neutralization complete? Write the neutralization reaction for HClO 4 and NH 3. What is the value of K n (equilibrium constant for neutralization)? (K B (NH 3 )= ) If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic or neutral? 153. When a weak acid is neutralized by a weak base is the neutralization complete? Write the neutralization reaction for HF and NH 3. What is the value of K n (equilibrium constant for neutralization)? (K A (HF)= ; K B (NH 3 )= ) If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic or neutral? 154. What happens to the ph of a solution of M HC 2 H 3 O 2 if a strong electrolyte like NaC 2 H 3 O 2 is added. NOTE: Addition of NaC 2 H 3 O 2 adds a common ion. Use Le Chatelier s principle to predict the direction of the reaction. What will happen to the ph of M HC 2 H 3 O 2 if NaCl is added? 155. What happens to the ph of a solution of M NH 3 if a strong electrolyte like NH 4 Cl is added. NOTE: Addition of NH 4 Cl adds a common ion. Use Le Chatelier s principle to predict the direction of the reaction. What will happen to the ph of M NH 3 if KNO 3 is added? 156. Calculate the ph and % ionization of a solution which is M HC 2 H 3 O 2 and M NaC 2 H 3 O 2. How does the ph of this solution compare to that of M HC 2 H 3 O 2? (K A (HC 2 H 3 O 2 )= ) 157. What is a buffer solution and what is its function? If the following substances are mixed in equimolar amounts, will a buffer solution be formed? A. HF and NaF D. NH 3 and NH 4 Cl G. HF and NaOH B. HC 2 H 3 O 2 and NaC 2 H 3 O 2 E. HCl and KCl H. NH 3 and HCl C. HCN and NaCN F. NaOH and NaCl
4 If equal volumes of the following solutions are mixed, will a buffer solution result? A. 0.2 M HF and 0.1 M NaOH E. 0.5 M NH 3 and 1.0 M HCl B. 0.2 M HF and 0.3 M NaOH F. 0.2 M HCN and 0.2 M KOH C. 0.2 M HF and 0.2 M NaOH G. 0.3 M HOCl and 0.15 M Ba(OH) 2 D. 0.2 M NaF and 0.1 M HCl H. 0.3 M HOCl and 0.1 M Ba(OH) Explain using the HC 2 H 3 O 2 /NaC 2 H 3 O 2 buffer system how a buffer maintains a relatively constant ph when small quantity of acid (HCl) or base (NaOH) is added A buffer solution consists of M HC 2 H 3 O 2 and M NaC 2 H 3 O 2. Calculate the ph of the resulting solution if mol HClO 4 is added to 500. ml of the buffer. The ph of the buffer solution before addition of the HClO 4 was A buffer solution consists of M HC 2 H 3 O 2 and M NaC 2 H 3 O 2. Calculate the ph of the resulting solution if mol NaOH is added to 500. ml of the buffer. The ph of the buffer solution before addition of the NaOH was Derive the HendersonHasselbach equation for a buffer solution consisting of weak acid/conjugate base (HF/NaF) and for a buffer solution consisting of weak base/conjugate acid (NH 3 /NH + 4 ) If the concentrations of acid and conjugate base are equal what is the ph of the buffer solution equal to? 163. A buffer solution is 0.25 M HNO 2 and 0.15 M NaNO 2. What is the ph of the buffer? K A (HNO 2 )= A buffer solution with a ph of 4.0 is needed in an experiment. Which of the following buffer systems should be used? For the chosen buffer system, what concentration ratio of conjugate base:acid should be used to attain ph=4.0? A. HNO 2 /NaNO 2 K A = B. HC 2 H 3 O 2 /NaC 2 H 3 O 2 K A = C. HCOOH/NaCOOH D. C 6 H 5 COOH/NaC 6 H 5 COO K A = K A = E. HCN/NaCN F. NH 3 /NH 4 Cl K A = K B = A buffer with a ph of 9.5 is to be prepared from NH 3 and /NH 4 Cl. What ratio of base to salt would you use? K B (NH 3 )= Explain why dilution of a buffer solution does not change the ph. Does a buffer work best when it s solution is dilute or concentrated (i.e. Which has a better buffer capacity a dilute or concentrated solution)? What concentration ratio of acid/salt or base/salt works best for buffers?
5 CHEM 116Dr. Babb s Sections Answer Key to Exam #3 Review Sheet 112. Lewis Acid (e pair acceptor) Lewis Base (e pair donor) A. BCl 3 NH 3 B. H + H 2 O C. H + OH D. Ag + NH BL Acid (H + donor) BL Base (H + acceptor) where BL=BronstedLowry A. H 2 O HCO 3 B. HCO 3 H 2 O C. 2 HPO 4 H 2 PO 4 D. HCO 3 NaOH (or OH ) 114. H + does not exist alone in solution and is actually associated and surrounded by many water molecules. From now on, H + will be represented as H 3 O Conjugate acid/base pairs have chemical formulas that differ by an H +. To obtain the conjugate acid of a base, add an H + to the chemical formula of the base. To obtain the conjugate base of an acid, subtract an H + from the chemical formula of the acid Acid (reactant side): HC 2 H 3 O 2 Conjugate Base (product side): C 2 H 3 O 2 Base (reactant side): H 2 O Conjugate Acid (product side): H 3 O NH 3 : Conjugate acid = NH 4+ ; Conjugate base = NH 2 HSO 4 : Conjugate acid = H 2 SO 4 2 Conjugate base = SO 4 2 CO 3 : Conjugate acid = HCO 3 Conjugate base = none (no H + to remove) H 2 O: Conjugate acid = H 3 O + Conjugate base = OH 118. Strong acids have weak conjugate bases (i.e. the conjugate base has no tendency to react with water to reform the original strong acid). Weak acids have strong conjugate bases (i.e. the conjugate base has a strong tendency to react with water to reform the original weak acid). Strong bases have weak conjugate acids (i.e. the conjugate acid has no tendency to react with water to reform the original strong base). Weak bases have strong conjugate acids (i.e. the conjugate acid has a strong tendency to react with water to reform the original weak base) The stronger base gets the H + and the equilibrium lies on the side opposite that of the strongest base. A. Eq. lies on the product side (i.e. [Products] > [Reactants]) because of the bases H 2 O and Cl, the H 2 O is the stronger base and thus, the eq. lies on the opposite side. B. Eq. lies on the reactant side (i.e. [Reactants] > [Products]) because of the bases H 2 O and C 2 H 3 O 2, the C 2 H 3 O 2 is the stronger base and thus the eq. lies on the opposite side Eq for dissociation of water: 2 H 2 O(l) < > H 3 O + (aq) + OH (aq); IonProduct constant=k w = [H 3 O + ][OH ] and K w has a value of at 25 C. The numerical value of K W depends only on temperature. In pure water, [H 3 O + ] = [OH ] = M Acidic solution occurs when [H 3 O + ] > M or when [OH ] < M or when [H 3 O + ] > [OH ]. Basic solution occurs when [H 3 O + ] < M or when [OH ] > M or when [H 3 O + ] < [OH ]. Neutral solution occurs when [H 3 O + ] = [OH ] = M All of the above definitions are for 25 C.
6 122. When [H 3 O + ] = M, then [OH ] = M. When [OH ] = M, then [H 3 O + ] = M ph = log [H 3 O + ]; poh = log [OH ]; pk W = logk w = log( ) = 14; ph + poh = ph > 7 indicates a basic solution; ph < 7 indicates an acidic solution; ph = 7 indicates a neutral solution A. ph = 5.17 is an acidic solution; poh = 8.9 has a solution ph = = 5.1 and is an acidic solution. ph = 7 is a neutral solution. B. i. ph = 6.5 is an acidic solution. ii. poh = 5.5 has a solution ph of 8.5 and is a basic solution. iii. [H 3 O + ] = is a basic solution since [H 3 O + ] < M and ph = 9.0. iv. [OH ] = is an acidic solution since [OHG] < M and ph = K A = Acid Dissociation Constant; the higher the value of K A, the stronger the acid; the lower the value of K A, the weaker the acid. HCl + H 2 O < > H 3 O + + Cl this eq. specified by K A for HCl HC 2 H 3 O 2 (aq) + H 2 O < > C 2 H 3 O 2 (aq) + H 3 O + (aq) this eq. specified by K A for HC 2 H 3 O K B = Base Dissociation Constant; the higher the value of K B, the stronger the base; the lower the value of K B, the weaker the base. NH 3 (aq) + H 2 O < > NH + 4 (aq) + OH (aq) this eq. specified by K B for NH [H 3 O + ] = 0.25 M; [OH ] = M; ph = 0.60; poh = [H 3 O + ] = G 12 M; [OH ] = M; ph = 12.00; poh = ph = ph = [H 3 O + ] = M; [OH ] = M; ph = 2.53; poh = 11.47; % Ionization HF = 12% 133. K A = ; % Dissociation of HCOOH = 2.4% 134. [H 3 O + ] = M; [OH ] = M; ph = 11.57; poh = 2.43; % Ionization NH 3 = 0.49% 135. A. H 2 SO 3 (aq) + H 2 O < > HSO 3 (aq) + H 3 O + (aq) K A1 HSO 3 (aq) + H 2 O < > SO 2 3 (aq) + H 3 O + (aq) K A2 B. H 3 PO 4 (aq) + H 2 O < > H 2 PO 4 (aq) + H 3 O + (aq) K A1 H 2 PO 4 (aq) + H 2 O < > HPO 2 4 (aq) + H 3 O + (aq) 2 3 HPO 4 (aq) + H 2 O < > PO 4 (aq) + H 3 O + (aq) 136. No, the ph of the resulting solution can be acidic, basic or neutral depending on the chemical identity of the salt The anion for the salt always comes from the acid; while, the cation for the salt always comes from the base NaCl is a neutral salt. NaCl is a strong electrolyte and dissolves and dissociates 100% as shown here: NaCl(s) > Na + (aq) + Cl (aq). The Na + is a weak conjugate acid of the strong base NaOH. Therefore, Na + has no tendency to react with water (hydrolyze) to reform the original strong base. The Cl is the weak conjugate base of the strong acid HCl. Therefore, Cl has no tendency to react with water (hydrolyze) to reform the original strong acid. The ph of an aqueous solution of this type of salt (containing cation from strong base and anion from strong acid) will be the ph of pure water which is NH 4 Cl is an acidic salt. NH 4 Cl is a strong electrolyte and dissolves and dissociates 100% as shown here: NH 4 Cl(s) > NH + 4 (aq) + Cl (aq). The Cl is the weak conjugate base of the strong acid HCl. Therefore, Cl has no tendency to react with water to reform the original K A2 K A3
7 strong acid. The NH is the strong conjugate acid of the weak base NH 3. Therefore, NH 4 has a tendency to react with water (hydrolyze) to reform the original weak base as shown here: NH 4+ (aq) + H 2 O(l) < > NH 3 (aq) + H 3 O + (aq). During this reaction some H 3 O + is produced resulting in a solution with an acidic ph (ph < 7) KNO 2 is a basic salt. KNO 2 is a strong electrolyte and dissolves and dissociates 100% as shown here: KNO 2 (s) > K + (aq) + NO 2 (aq). The K + is a weak conjugate acid of the strong base KOH. Therefore, K + has no tendency to react with water (hydrolyze) to reform the original strong base. The NO 2 is the strong conjugate base of the weak acid HNO 2. Therefore, NO 2 has a tendency to react with water (hydrolyze) to reform the original weak acid as shown here: NO 2 (aq) + H 2 O(l) < > HNO 2 (aq) + OH (aq). During this reaction some OH is produced resulting in a solution with a basic ph (ph > 7) AlCl 3 is an acidic salt. AlCl 3 is a strong electrolyte and dissolves and dissociates 100% as shown here: AlCl 3 (s) > Al +3 (aq) + 3 Cl (aq). The Cl is the weak conjugate base of the strong acid HCl. Therefore, Cl has no tendency to react with water to reform the original strong acid. The Al +3 being a small, highly charged metal cation exists in solution as Al(H 2 O) +3 6 (aq). The association of the H 2 O s with the Al +3 tends to weaken the OH bond in the H 2 O s making the waters surrounding the aluminum more acidic. Therefore, the +3 Al(H 2 O) 6 species has a tendency to react with water (hydrolyze) as an acid as shown here: +3 Al(H 2 O) 6 (aq) + H 2 O(l) < > Al(H 2 O) 5 OH +2 (aq) + H 3 O + (aq). During this reaction some H 3 O + is produced resulting in a solutions with an acidic ph (ph < 7) A. basic D. basic G. acidic B. acidic E. basic H. acidic C. neutral F. acidic 143. K A K B = K W 144. NaF is a basic salt due to hydrolysis of F. ph = NH 4 ClO 4 is an acidic salt due to hydrolysis of NH + 4. ph = In general, any factor that weakens the bond to hydrogen, makes the substance more acidic. For binary acids within the same group such as HCl, HF, HI, and HBr, the atom bonded to hydrogen (F, Cl, Br, I) becomes larger as proceed down the periodic table and this tends to weaken the bond to H. Thus, binary acids become more acidic as proceed from top to bottom with a column. Most acidic: HI > HBr > HCl > HF :Least acidic; Most acidic: H 2 Te > H 2 S > H 2 O :Least acidic For binary acids within the same row such as CH 4, NH 3, H 2 O, and HF, the atom the hydrogen is bonded to (C, N, O and F) becomes more electronegative as proceed across the row and this tends to weaken the bond to H. Thus these binary acids become more acidic as proceed from left to right within a row. Most acidic: HF > H 2 O > NH 3 > CH 4 :Least acidic In oxyacids, the H is always bonded to one of the oxygens. Any factor that weakens the OH bond, makes the substance more acidic. Within an oxyacid series such as HClO, HClO 3, HClO 2 and HClO 4, as the number of oxygens bonded to the central atom increases, the oxidation number of the central atom increases causing a weakening of the OH bond strength and an increase in the acidity. Most acidic: HClO 4 > HClO 3 > HClO 2 > HClO. For a series of oxyacids with the same number of oxygens but with different central atoms such as HOBr, HOCl, HOI, as the electronegativity of the central atom increases, the OH bond strength weakens and the acidity increases. Most acidic: HOCl > HOBr > HOI :Least acidic Compare strengths of acids on reactant and product sides. The stronger acid has a greater
8 tendency to give up its proton; therefore, the equilibrium will lie on the opposite side from the strongest acid. A. HBr is a stronger acid than HF. Eq lies on side opposite the HBr (i.e. on reactant side); thus, [Reactants] > [Products] and K < 1. B. H 2 O is a stronger acid than NH 3. Eq lies on side opposite the H 2 O (i.e. on product side); thus, [Products] > [Reactants] and K > 1. C. HClO 2 is a stronger acid than HClO. Eq lies on side opposite the HClO 2 (i.e. on reactant side); thus, [Reactants] > [Products] and K < 1. D. H 3 O + is a stronger acid than H 2 O. Eq. lies on side opposite the H 3 O + (i.e. on the reactant side); thus, [Reactants] > [Products] and K < 1. E. HBrO 3 is a stronger acid than HIO 3. Eq. lies on side opposite the HBrO 3 (i.e. on the product side); thus, [Products] > [Reactants] and K > As solid NaC 2 H 3 O 2 is added to M HC 2 H 3 O 2, the [H 3 O + ] decreases and the ph increases. Why? Look at effect of addition of NaC 2 H 3 O 2, a strong electrolyte, on the acetic acid eq. HC 2 H 3 O 2 (aq) + H 2 O(l) < > C 2 H 3 O 2 (aq) + H 3 O + (aq) NaC 2 H 3 O 2 (s) > Na + (aq) + C 2 H 3 O 2 (aq) As NaC 2 H 3 O 2 is added to an eq. mixture of M HC 2 H 3 O 2, the common ion C 2 H 3 O 2 is added which shifts the acetic acid eq. to the left decreasing the [H 3 O + ] and increasing the ph. Addition of NaCl to an eq. mixture of M HC 2 H 3 O 2 has no effect on the ph or acetic acid eq. because NaCl has no ion in common with the acetic acid eq As solid NH 4 Cl is added to M NH 3, the [OH ] decreases, the [H 3 O + ] increases and the ph decreases. Why? Look at effect of addition of NH 4 Cl, a strong electrolyte, on the ammonia eq. NH 3 (aq) + H 2 O(l) < > NH + 4 (aq) + OH (aq) NH 4 Cl(s) > NH + 4 (aq) + Cl (aq) + As NH 4 Cl is added to an eq. mixture of M NH 3, the common ion NH 4 is added which shifts the ammonia eq. to the left decreasing the [OH ] and decreasing the ph. Addition of KNO 3 to an eq. mixture of M NH 3 has no effect on the ph or ammonia eq. because KNO 3 has no ion in common with the ammonia eq For a M HC 2 H 3 O 2 /0.250 M NaC 2 H 3 O 2 : ph = 4.44 and % Ionization = %. For a M HC 2 H 3 O 2 : ph = 2.52 and % Ionization = 0.60% Buffer solution: A solution consisting of a weak acid and the conjugate base (or salt) of the weak acid. OR A solution consisting of a weak base and the conjugate acid (or salt) of the weak base. Function of Buffer: Acts to maintain the ph of the solution at a relatively constant value even with the addition of strong base or strong acid. If the following substances are mixed in equimolar amounts, will a buffer solution be formed? A. HF and NaF; Yes D. NH 3 and NH 4 Cl; Yes B. HC 2 H 3 O 2 and NaC 2 H 3 O 2 ; Yes E. HCl and KCl; No C. HCN and NaCN; Yes F. NaOH and NaCl; No G. HF and NaOH; No H. NH 3 and HCl; No If equal volumes of the following solutions are mixed, will a buffer solution result? A. 0.2 M HF and 0.1 M NaOH; Yes B. 0.2 M HF and 0.3 M NaOH; No C. 0.2 M HF and 0.2 M NaOH; No
9 D. 0.2 M NaF and 0.1 M HCl; Yes E. 0.5 M NH 3 and 1.0 M HCl; No F. 0.2 M HCN and 0.2 M KOH; No G. 0.3 M HOCl and 0.15 M Ba(OH) 2 ; No H. 0.3 M HOCl and 0.1 M Ba(OH) 2 ; Yes 159. ph = ph = HendersonHasselbach equation: ph = pk A + log[base]/[acid] 162. When [Base] = [Acid] then ratio [base]/[acid] = 1 and log(1) = 0 so ph = pk A. Thus, the pk A is the midpoint of the buffer range ph = If a buffer with a ph = 4.0 is needed in an experiment, then a buffer system with a pk A value around 4.0 is needed. pk A A. HNO 2 /NaNO 2 K A = B. HC 2 H 3 O 2 /NaC 2 H 3 O 2 K A = C. HCOOH/NaCOOH K A = D. C 6 H 5 COOH/NaC 6 H 5 COO K A = E. HCN/NaCN K A = F. NH 3 /NH 4 Cl K B = The best buffer system is that given in D because its pk A value is closest to 4.0. To obtain a ph=4.0 using this buffer system, a concentration ratio of base:acid of 0.65 should be used. Therefore, if the [C 6 H 5 COOH] is 1.0 M; the [NaC 6 H 5 COO] should be 0.65 M [NH 3 ]/[NH 4+ ] = 1.7
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 informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationCHAPTER 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 informationAcids 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 informationChapter 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 informationCHEMISTRY 102 Fall 2010 Hour Exam III Page My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
Hour Exam III Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml
More informationSolutions are aqueous and the temperature is 25 C unless stated otherwise.
Solutions are aqueous and the temperature is 25 C unless stated otherwise. 1. According to the Arrhenius definition, an acid is a substance that produces ions in aqueous solution. A. H C. OH B. H + D.
More informationChapter 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 informationProperties 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 informationChapter 16: Acids and Bases
1. Which is not a characteristic property of acids? A) neutralizes bases B) turns litmus from blue to red C) reacts with active metals to produce H 2 (g) D) reacts with CO 2 (g) to form carbonates E) All
More informationChapter 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 informationChapter 16 exercise. For the following reactions, use figure 16.4 to predict whether the equilibrium lies predominantly. - (aq) + OH - (aq)
1 Chapter 16 exercise Q1. Practice exercise page 671 Write the formula for the conjugate acid of the following, HSO 3, F, PO 4 3 and CO. HSO 3 H H 2 SO 4 F H HF PO 4 3 H HPO 4 2 CO H HCO Q2. Practice exercise
More informationUnit 9: Acid and Base Multiple Choice Practice
Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.
More informationChapter 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 informationAP Chemistry: Acid-Base Chemistry Practice Problems
Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases 14.1 The Nature of Acids and Bases Bronsted-Lowry Acid-Base Systems Bronsted acid: proton donor Bronsted base: proton acceptor Bronsted acid base reaction: proton transfer from
More informationHA(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 informationADVANCED 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 informationCHEMISTRY 102 Fall 2010 Hour Exam III. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
1. My answers for this Chemistry 10 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml of 0.30 M HCN by 0.10
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More informationChapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
More informationAcids 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. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationChapter 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 informationThe ph of aqueous salt solutions
The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2
More informationCHEM 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 informationChemistry 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 information1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
More informationAcid / 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 informationAcids 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 informationContents 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 informationAcids and Bases. Slide 1 / 208. Slide 2 / 208. Slide 3 / 208. Table of Contents: Acids and Bases
Slide 1 / 208 Slide 2 / 208 Acids and Bases Table of Contents: Acids and Bases Click on the topic to go to that section Slide 3 / 208 Properties of Acids and Bases Conjugate Acid and Base Pairs Amphoteric
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More informationAcids 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 informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationUnit 4: Acid/Base I. abinotes. I) Introduction to Acids and Bases What is an acid?
Unit 4: Acid/Base I I) Introduction to Acids and Bases What is an acid? http://www.kidsknowit.com/flash/animations/acidsbases.swf What are properties of acids? 1) Acids react with. 2) Acids create when
More informationChapter 18. Acid-Base Equilibria. Acid Base Theories. There are three acid/base theories used to define acids and bases: Arrhenius Theory
116acidbase Chapter 18 AcidBase Equilibria Acid Base Theories There are three acid/base theories used to define acids and bases: 1. 2. 3. Arrhenius Acid Arrhenius Theory Most specific of the three acidbase
More informationAcids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H ], (also thought of as hydronium ion, H O ) when dissolved in water. Acids
More information*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 informationChap 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 informationLecture Presentation. Chapter 16. Acid Base Equilibria. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 16 Acid Base Equilibria John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius An acid is a substance that, when dissolved in water, increases
More informationChemistry 201: General Chemistry II - Lecture
Name Date Chemistry 201: General Chemistry II - Lecture Short-Answer Exam #2, 60 Points Total Form: A Read all directions carefully. Answers not conforming to the directions will be marked as incorrect!
More informationChpt 16: Acids and Bases
Chpt 16 Acids and Bases Defining Acids Arrhenius: Acid: Substances when dissolved in water increase the concentration of H+. Base: Substances when dissolved in water increase the concentration of OH- Brønsted-Lowry:
More informationCHEM 142 Exam 3 Study Guide Chapter 15: Acid-Base Equilibria
CHEM 142 Exam 3 Study Guide Chapter 15: AcidBase Equilibria A. Terminologies and Concepts 1. BronstedLowry definitions acids vs. bases; give examples 2. Amphoteric substances define and give examples 3.
More informationph 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 informationIB 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 informationCHM 152/154 HOUR EXAM II Diebolt Summer multiple choice 52 Parts II and III 73 Total Pts 125
CHM 152/154 HOUR EXAM II Diebolt Summer 2010 pts earned name pts possible multiple choice 52 Parts II and III 73 Total Pts 125 Part One: Multiple choice. Mark the correct answers on the provided scantron
More informationAssignment 16 A incorrect
Assignment 16 A 1- What is the concentration of hydronium ions in a solution with a hydroxide-ion concentration of 2.31 10 4 M at 25 C? a) 4.33 10 11 M b) 2.31 10 4 M c) 2.31 10 18 M d) 2.31 10 10 M (The
More informationChemistry 102 Chapter 15 ACID-BASE CONCEPTS
General Properties: ACID-BASE CONCEPTS ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink Neutralization
More informationI II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is
1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium
More informationChapter 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 informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
More informationACIDS 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 informationWorksheet 4.1 Conjugate Acid-Base Pairs
Worksheet 4.1 Conjugate AcidBase Pairs 1. List five properties of acids that are in your textbook. Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with
More informationChapter 16. Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius
More informationName 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 informationIn the Brønsted-Lowry system, a Brønsted-Lowry acid is a species that donates H + and a Brønsted-Lowry base is a species that accepts H +.
16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 BrønstedLowry Acids and Bases In the BrønstedLowry system, a BrønstedLowry
More informationAP Chemistry CHAPTER 16 STUDY GUIDE Acid-Base Equilibrium
AP Chemistry CHAPTER 16 STUDY GUIDE AcidBase Equilibrium 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
More informationCHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
More informationChem1120pretest2Summeri2015
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 informationSection 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 informationChem 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 informationLewis Acid/Base. Lewis acid is a different way to look at some type of acids. Lewis Acid/base reactions track the electrons rather then the protons.
Acid Base Wrap up topics Lewis acid Bases Structural indicators of the strength of acids Non-metal oxides/ metal oxides Amphoteric substances Acidic properties of swimming pools Schweitzer 1-29-05 Lewis
More informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationChem 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 informationAcids and Bases. Properties of Acids. Properties of Bases. Slide 1 / 174. Slide 2 / 174. Slide 3 / 174
Slide 1 / 174 Acids and Bases PSI Chemistry covers the material approximately up to slide 75. Properties of Acids Slide 2 / 174 Acids release hydrogen ion(s) into (aqueous) solution Acids neutralize bases
More informationNATURE OF ACIDS & BASES
General Properties: NATURE OF ACIDS & BASES ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink
More information11/14/10. 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 information1) What is the Arrhenius definition of an acid? Of a base? 2) What is the Bronsted-Lowry definition of an acid? Of a base?
Problems, Chapter 16 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) What is the Arrhenius definition of an acid? Of a base? An Arrhenius acid is a substance that produces
More informationChem12 Acids : M.C
Chem12 Acids : M.C. 3-260 1) The equation showing the acid form of an indicator reacting with a basic solution is : a) In - (aq) + OH - (aq) -> HIn(aq) + O 2- (aq) b) HIn(aq) + OH - (aq) ->H 2 O(l) + In
More informationUnit 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 informationChem12 Acids : Exam Questions M.C.-100
Chem12 Acids : Exam Questions M.C.-100 1) Given : HPO 4 2- (aq) + NH 4 + (aq) H 2 PO 4 - (aq) + NH 3 (aq), the strongest acid in the above equation is : a) NH 4 + b) HPO 4 2- c) NH 3 d) H 2 PO 4-2)
More informationAcids, 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 informationPart 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 informationChapter 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 informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
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
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 informationLecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
Lecture 10 Professor Hicks Inorganic Chemistry II (CHE152) ph Scale of [H 3 O + ] (or you could say [H + ]) concentration More convenient than scientific notation ph = log [H 3 O + ] still not sure? take
More informationAcid-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 information1. (3) The pressure on an equilibrium mixture of the three gases N 2, H 2 and NH 3
1. (3) The pressure on an equilibrium mixture of the three gases N 2, H 2 and NH 3 N 2 (g) + 3 H 2 (g) 2 NH 3 (g) is suddenly decreased by doubling the volume of the container at constant temperature.
More informationCH 15 Summary. Equilibrium is a balance between products and reactants
CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium
More informationCHM 2046 Test #3 Review: Chapters , 15, & 16
Chapter 14 1. For the following reaction Kc = 0.513 at 500 K. N 2 O 4 (g) 2 NO 2 (g) If a reaction vessel initially contains an N 2 O 4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria
Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More informationAcid Base Review. 2. Identify the acid base conjugate pairs in each of the following reactions according with the Bronsted Lowry framework:
Acid Base Review 1. Identify Lewis Acid, in the following reactions: a. Zn 2 4 H 2 O qwwwwe Zn (H 2 O) 4 2 b. BF 3 F 1 qwwwwe BF 4 1 c. Ag 1 2NH 3 qwwwwe Ag(NH 3 ) 2 1 2. Identify the acid base conjugate
More informationChem1120pretest2Summeri2015
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 informationHomework #7 Chapter 8 Applications of Aqueous Equilibrium
Homework #7 Chapter 8 Applications of Aqueous Equilibrium 15. solution: A solution that resists change in ph when a small amount of acid or base is added. solutions contain a weak acid and its conjugate
More informationAcid-Base Equilibria
Acid-Base Equilibria 1. Classify each of the following species as an acid, a base, or amphoteric in aqueous solution: (a) H 2 O; (b) CH 3 CH 2 ; (c) PO 4 3 ; (d) C 6 H 5 NH 3 2. Write the proton transfer
More informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
More informationAcids, Bases, and Salts Review for Sections
1. Consider the following: Review for Sections 4.1 4.9 I H 2 CO 3 + F HCO 3 + HF 2 II HCO 3 + HC 2 O 4 H 2 CO 3 + C 2 O 4 2 III HCO 3 + H 2 C 6 H 6 O 7 H 2 CO 3 + HC 6 H 5 O 7 The HCO 3 is a base in A.
More informationChemistry 12 Unit 4 Topic A Hand-in Assignment
1 Chemistry 12 Unit 4 Topic A Handin Assignment Answer the following multiplechoice and written response problems on your own paper. Submit your answers for marking. You do not need to show your work for
More informationUnit 6: ACIDS AND BASES
Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationC) SO 4 H H. C) The N-atom is the Lewis base because it accepted a pair of electrons to form the
AP Chemistry Test (Chapters 14 and 15) 1) Which one would hydrolyze water the most? A) Ca 2+ B) NO 3 - C) SO 4 2- H H D) CN - 2) Which one is true about the compound? H B-N H A) The N-atom is the Lewis
More informationHomework #6 Chapter 7 Homework Acids and Bases
Homework #6 Chapter 7 Homework Acids and Bases 20. a) 2H 2O(l) H 3O (aq) OH (aq) K [H 3 O ][OH ] Or H 2O(l) H (aq) OH (aq) K [H ][OH ] b) HCN(aq) H 2O(l) H 3O (aq) CN (aq) K [H 3O ][CN ] [HCN] Or HCN(aq)
More informationJudith Herzfeld 1996,1998. These exercises are provided here for classroom and study use only. All other uses are copyright protected.
Judith Herzfeld 1996,1998 These exercises are provided here for classroom and study use only. All other uses are copyright protected. 3.3-010 According to Bronsted-Lowry Theory, which of the following
More informationChapter 15. Properties of Acids. Structure of Acids 7/3/08. Acid and Bases
Chapter 15 Acid and Bases Properties of Acids! Sour taste! React with active metals! React with carbonates, producing CO 2! Change color of vegetable dyes!blue litmus turns red! React with bases to form
More informationPractice Exam 1: Answer Key
CHM 2046 Practice Exam 1: Answer Key Important: Bubble in A, B or C as the test form code at the top right of your answer sheet. Useful information is provided at the end. VERSION A 1. The reaction A(aq)
More informationDougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria
Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly
More informationCh 7 Practice Problems
Ch 7 Practice Problems 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a eak acid), the equilibrium constant expression is [H ] [NO 2 ] = [HNO ] 2 [H ][N][O] [HNO 2] =
More information