Mr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
|
|
- Erick Hunter
- 6 years ago
- Views:
Transcription
1 Acids and Bases 1
2 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 balanced acid/base chemical equations. Include: conjugate acid/base pairs, amphoteric behavior. Distinguish between strong and weak acids and bases. Include: electrolytes and nonelectrolytes Describe the relationship between the hydronium and hydroxide ion concentrations in water Include: the ion product of water, K w Formulate an operational definition of ph. Solve problems involving ph. Describe how an acidbase indicator works in terms of colour shifts and Le Chatelier s Principle. Write the equilibrium expression (K a or K b ) from a balanced chemical equation. Use K a or K b to solve problems for ph, percent dissociation and concentration. Predict whether an aqueous solution of a given ionic compound will be acidic, basic or neutral given the formula. Write balanced neutralization reactions involving strong acids and bases. Calculate the concentration or volume of an acid or base from the concentration and volume of an acid or base required for neutralization. Using a standardized acid or base, determine the concentration of an unknown base or acid. Additional KEY Terms monoprotic diprotic amphoteric salt hydrolysis concentrated dilute standard solution end point equivalence point titration Relative Strengths of Acids 2
3 *Acids 1.0 mol/l in water at 25ºC Acid Reaction K a Perchloric acid HClO 4 + H 2 O H 3 O + + ClO 4 very large Hydriodic acid HI + H 2 O H 3 O + + I very large Hydrobromic acid HBr + H 2 O H 3 O + + Br very large Hydrochloric acid HCl + H 2 O H 3 O + + Cl very large Nitric acid HNO 3 + H 2 O H 3 O + + NO 3 very large Sulfuric acid H 2 SO 4 + H 2 O H 3 O + + HSO 4 very large Oxalic acid H 2 C 2 O 4 + H 2 O H 3 O + + HC 2 O x 10 2 Sulfurous acid H 2 SO 3 + H 2 O H 3 O + + HSO x 10 2 Hydrogen sulfate ion HSO 4 + H 2 O H 3 O + + SO x 10 2 Phosphoric acid H 3 PO 4 + H 2 O H 3 O + + H 2 PO x 10 3 Ferric ion 3+ Fe(H 2 O) 6 + H 2 O H 3 O + + Fe(H 2 O) 5 (OH) x 10 3 Hydrogen telluride H 2 Te + H 2 O H 3 O + + HTe 2.3 x 10 3 Hydrofluoric acid HF + H 2 O H 3 O + + F 6.7 x 10 4 Nitrous acid HNO 2 + H 2 O H 3 O + + NO x 10 4 Hydrogen selenide H 2 Se + H 2 O H 3 O + + HSe 1.7 x 10 4 Chromic ion Cr(H 2 O) H 2 O H 3 O + + Cr(H 2 O) 5 (OH) x 10 4 Benzoic acid C 6 H 5 COOH + H 2 O H 3 O + + C 6 H 5 COO 6.6 x 10 5 Hydrogen oxalate ion HC 2 O 4 + H 2 O H 3 O + + C 2 O x 10 5 Acetic acid HC 2 H 3 O 2 + H 2 O H 3 O + + C 2 H 3 O x 10 5 Aluminum ion Al(H 2 O) H 2 O H 3 O + + Al(H 2 O) 5 (OH) x 10 5 Carbonic acid H 2 CO 3 + H 2 O H 3 O + + HCO x 10 7 Hydrogen sulfide H 2 S + H 2 O H 3 O + + HS 1.0 x 10 7 Dihydrogen phosphate ion H 2 PO 4 + H 2 O H 3 O + + HPO x 10 8 Hydrogen sulfite ion HSO 3 + H 2 O H 3 O + + SO x 10 8 Ammonium ion + NH 4 + H 2 O H 3 O + + NH x Hydrogen carbonate ion HCO 3 + H 2 O H 3 O + + CO x Hydrogen telluride ion HTe + H 2 O H 3 O + + Te x Hydrogen peroxide H 2 O 2 + H 2 O H 3 O + + HO x Monohydrogen phosphate HPO 42 + H 2 O H 3 O + + PO x Hydrogen sulfide ion HS + H 2 O H 3 O + + S x Water H 2 O + H 2 O H 3 O + + OH 1.8 x Hydroxide ion OH + H 2 O H 3 O + + O 2 < Ammonia NH 3 + H 2 O H 3 O + + NH 2 very small POLYATOMIC IONS 3
4 NAME FORMULA CHARGE ACETATE CH 3 COO 1 AMMONIUM + NH 4 +1 HYDROGEN CARBONATE (BICARBONATE) HCO 3 1 CARBONATE 2 CO 3 2 CHLORATE ClO 3 1 CHLORITE ClO 2 1 CHROMATE 2 CrO 4 2 DICHROMATE 2 Cr 2 O 7 2 DIHYDROGEN PHOSPHATE H 2 PO 4 1 HYDROGEN PHOSPHATE 2 HPO 4 2 PHOSPHATE 3 PO 4 3 HYDROGEN SULFATE (BISULFATE) HSO 4 1 SULFATE 2 SO 4 2 HYDROGEN SULFITE (BISULFITE) HSO 3 1 SULFITE 2 SO 3 2 HYDRONIUM H 3 O + +1 HYDROXIDE OH 1 PERCHLORATE ClO 4 1 HYPOCHLORITE ClO (OCl ) 1 NITRATE NO 3 1 NITRITE NO 2 1 PERMANGANATE MnO 4 1 THIOCYANATE SCN 1 Patterns for Naming Polyatomic Ions ate ending is the general (base) form. The ending changes depending on the number of oxygen atoms notice the charge remains the same in these cases. ClO 3 chlorate base oxygen atoms ClO 4 perchlorate base + 1 oxygen atom ClO 2 chlorite base 1 oxygen atom ClO hypochlorite base 2 oxygen atoms 4
5 *FOLLOW THE MOVING HYDROGEN ION* 1. Identify the acid, base, conjugate acid and conjugate base for each of the following. a) HClO 4 (aq) + H 2 O (l) H 3 O + (aq) + ClO 4 (aq) b) H 2 SO 3 (aq) + H 2 O (l) H 3 O + (aq) + HSO 3 (aq) c) HC 2 H 3 O 2 (aq) + H 2 O (l) H 3 O + (aq) + C 2 H 3 O 2 (aq) d) H 2 S (g) + H 2 O (l) H 3 O + (aq) + HS (aq) e) HSO 3 (aq) + H 2 O (l) H 3 O + (aq) + SO 3 2 (aq) f) NH 3 (g) + H 2 O (l) NH 4 + (aq) + OH (aq) g) HF (aq) + HSO 3 (aq) F ( aq) + H 2 SO 3 (aq) h) HNO 2 (aq) + HS (aq) NO 2 (aq) + H 2 S (aq) 2. Predict which reactant will accept a hydrogen ion and complete the products for each equation. Label each reactant as an acid or base. List under the first reactant whether it falls under the Arrhenius (A) and/or BronstedLowry (BL) definition of an acids/bases E.g. HBr (aq) + H 2 O (l) H 3 O + (aq) + Br (aq) Acid Base (A and BL) a) HI (aq) + H 2 O (l) b) HF (aq) + H 2 O (l) c) H 2 CO 3 (g) + H 2 O (l) d) CO 3 2 (aq) + H 2 O (l) e) O 2 (aq ) + H 2 O (l) f) HSO 3 (aq) + H 2 O (l) 5
6 Write the dissociation of each of the following in water. Predict whether each of the following will be an electrolyte or nonelectrolyte. 1. NaOH (s) 2. Na 2 CO 3 (s) 3. Mg(OH) 2 (s) 4. C 6 H 12 O 6 (s) 5. HCl (g) 6. K 3 PO 4 (s) 7. H 2 SO 4 (aq) 8. NaC 2 H 3 O 2 (s) 9. (NH 4 ) 2 SO 4 (s) 10. C 2 H 5 OH (l) 11. H 3 PO 4 (aq) 12. CaCl 2 (s) 6
7 1. In each case: i. Complete the acidbase equation with the help of tables if needed. ii. ii. Label the acid, base, CA, CB. iii. Explain whether the reactants or products are favored at equilibrium. a) H 3 PO 4 + C 2 H 3 O 2 b) C 2 H 3 O 2 + HSO 4 c) SO NH 4 + d) HO 2 + H 2 CO 3 e) Al(H 2 O) HSe 2. List the following in decreasing (strongest to weakest) order of strength as bases. a. CO 3 2 b. HCO 3 c. HPO 4 2 d. CH 3 COO e. HSO 3 3. List the following substances in increasing order (weakest to strongest) of strength as acids and bases. Some may be used more than once. F, H 2 PO 4, HSO 4, H 2 S, C 2 H 3 O 2, HNO 2, HTe 7
8 ANSWER THE FOLLOWING QUESTIONS ABOUT Kw AND ION CONCENTRATION: 1. What is the hydroxide ion concentration in a solution with an hydronium concentration of mol/l? 2. What is the [H 3 O + ] in a solution with [OH ] of ? 3. If the [H 3 O + ] in a nitric acid solution is mol/l, what is the [OH ]? 4. If the [OH ] in a sodium hydroxide solution is mol/l, what is [H 3 O + ]? moles of hydrogen chloride gas is dissolved in 2.0 L of water. Write the dissociation equation for this gas and calculate both [H 3 O + ] and [OH ] g of lithium hydroxide is dissolved in 750 ml of water. Write the dissociation equation and calculate both [H 3 O + ] and [OH ] g of calcium hydroxide is dissolved in ml of solution. Write the dissociation equation and calculate both [H 3 O + ] and [OH ]. 8. If the [H 3 O + ] of a barium hydroxide solution is mol/l, calculate the [OH ]. How many grams of barium hydroxide must have been used to make a Litre of this solution? 9. Calculate the [H 3 O + ] in milk of magnesia (magnesium hydroxide) that has an [OH ] of mol/l. Answer Key 1) 1.47 x 10 5 M, 2) 1.76 x M, 3) 5.0 x M, 4) 2.0 x M, 5) M, 8.0 x M 6) 1.79 x M, M 7) 1.48 x M, M 8) 8.6 g, 9) 6.99 x M 8
9 ANSWER THE FOLLOWING QUESTIONS ON ph and poh: 1. Determine the ph of each of the following values a. [H + ] = 1.0 x 10 6 b. [H + ] = 1.0 x 10 8 c. [OH ] = 1.0 x 10 2 d. [OH ] = 1.0 x 10 5 e. [H + ] = 2.0 x 10 3 f. [H + ] = 3.5 x 10 4 g. [OH ] = 7.50 x 10 7 h. [OH ] = 9.0 x Determine the concentration of [H+] of each of the following. a. ph = 7.00 b. poh = 5.00 c. ph = d. poh = e. ph = 3.40 f. poh = 6.10 g. ph = 8.90 h. poh = Determine the poh of the following if the ph is given a. ph = 5.40 b. ph = 8.60 c. ph = 2.90 d. ph = Determine the concentration of the OH ions in solutions with the following ph values. a. ph = 4.10 b. ph = 5.10 c. ph = 1.60 d. ph = Calculate ph of each of the following solutions. a mol/l HCl b M NaOH c. 4.0 x 10 4 M Ba(OH) 2 d mol/l HNO 3 Answers a b c d e f g h a. 1e7 b. 1e9 c. 1e13 d. 1e3 e. 4e4 f. 1.3e8 g. 1.3e9 h a b c d a. 1.3e10 b. 1.3e9 c. 4e13 d. 1.6e5 a b c d
10 ph practice 1) What is the ph and poh of a 1.2 x 10 3 M HBr solution? 2) What is the ph and poh of a 2.34 x 10 5 NaOH solution? 3) What is the ph and poh of a solution made by adding water to 15 grams of hydroiodic acid until the volume of the solution is 2500 ml? 4) What is the ph and poh of a solution that was made by adding 400 ml of water to 350 ml of 5.0 x 10 3 M NaOH solution? 5) What is the ph and poh of a solution with a volume of 5.4 L that contains 15 grams of hydrochloric acid and 25 grams of nitric acid? 6) A swimming pool has a volume of one million liters. How many grams of HCl would need to be added to that swimming pool to bring the ph down from 7 to 4? (Assume the volume of the HCl is negligible) ANSWER KEY 1. ph: 2.9 poh: poh: 4.6 ph: ph: 1.3 poh: poh: 2.7 ph: ph: 0.82 poh: g 10
11 ANSWER THE FOLLOWING DISSOCIATION QUESTIONS: 1. Calculate the concentration of all species in a 0.70 mol/l HNO 3 solution. 2. Determine the [H 3 O + ] in 0.90 mol/l solution of weak acid H 2 S. (K a = 1.0 x 10 7 ) (3.0x 10 4 M) 3. Find the concentration of all species in a 0.10 M solution of NaOH. 4. Determine the concentration of all species in a 0.65 mol/l solution of an ammonia, if the base dissociation constant is 1.8 x (3.4 x 10 3 M) 5. Find the [H + ] in a 0.86 M solution of the weak acid H 2 O 2. (Ka = 2.4 x ) (1.4 x 10 6 M) 6. If [H 3 O + ] = 4.5 x 10 6 mol/l in a 0.45 mol/l solution of the weak acid HX, calculate percent dissociation. (0.001%) 7. Find the percent dissociation in 0.87 M solution of the weak base HPO 4 2 if K b is 1.6 x (0.043%) 11
12 8. Calculate the [H + ] of a 0.38 mol/l weak acid that is dissociated 0.12%. (4.56 x 10 4 M) 9. Determine the K a for an acid, HA, if a 0.45 M solution is dissociated 0.025%. (2.8 x 10 8 ) 10. Calculate the the percent dissociation of a 0.60 mol/l aniline (C 6 H 5 NH 2 ) solution (Kb = ) if it dissociates according to the following equation: (0.0025%) C 6 H 5 NH 2 + H 2 O C 6 H 5 NH OH 11. Determine the Ka for an acid HA if a mol/l solution is dissociated 0.015%. (1.7 x 10 8 ) 12. If [H 3 O + ] = mol/l, calculate the Ka for a weak acid in a solution of 0.80 mol/l of an acid HB. (2.5 x ) 13. Calculate the ph of a 0.10 mol/l solution of hypochlorous acid, HOCl (Ka = ) (4.2) 12
13 14. A 0.20 mol/l solution of the weak base HPO 2 4 has a ph of Find the Kb. (5.0 x ) 15. Calculate the Ka of a weak acid, HX, if a 0.25 mol/l solution has a ph of (6.3 x 10 9 ) 16. At 25 C, a mol/l ammonia solution is 4.3% ionized. Calculate the poh and ph. (3.4, 10.6) 17. Hydrazine (N 2 H 4 ) is a weak base with a Kb of The reaction of hydrazine in water is H 2 NNH 2 + H 2 O H 2 NNH OH Calculate the the ph of a 2.0 mol/l solution of hydrazine. (11) 18. Calculate the percent dissociation of a 0.20 mol/l solution of the weak acid, HNO 2, if the ph of the solution is (0.032%) 13
14 ANSWER THE FOLLOWING DISSOCIATION QUESTIONS: 1. Calculate the original concentration of the weak base, C 2 H 3 O 2 (acetate ion), if [OH ] = 1.5 x 10 5 and K b = 5.6 x (0.4 M) 2. Calculate percent dissociation of a 0.60 M aniline (C 6 H 5 NH 2 ) solution (K b = 3.8 x ) if it dissociates according to the following equation: (0.0025%) C 6 H 5 NH 2 + H 2 O C 6 H 5 NH OH 3. Determine the K a for an acid HA if a M solution is dissociated 0.015%. (1.7 x 10 8 ) 4. Compute the concentration of [OH ] in a 0.75 mol/l solution of Mg(OH) If [H 3 O + ] = 4.5 x mol/l, calculate K a in a solution of 0.80 mol/l of an acid HB. (2.5 x ) 6. Determine the concentration of all species plus the percent dissociation in a 0.60 mol/l ammonia solution. (K b = 1.8 x 10 5 ) (3.3 x 10 3 M, 3.3 x 10 3 M, 0.6 M, 0.55%) 7. Calculate the concentration of a solution of acetic acid (Ka = 1.8 x 10 5 ) with ph = (0.056) 14
15 Are each of the following salts acidic, basic or neutral in water? Explain why. 1. Sodium sulfate 2. Potassium phosphate 3. Sodium nitrate 4. Sodium sulfide 5. Potassium chloride 6. Magnesium nitrate 7. Iron (III) Nitrate 8. Sodium carbonate 9. Potassium oxalate 10. Ammonium iodide 11. Potassium acetate 12. Chromium (III) bromide 13. Potassium dihydrogen phosphate 14. Sodium nitrite 15. Calcium oxide 15
16 ANSWER THE FOLLOWING NEUTRALIZATION QUESTIONS: 1. Write the complete reaction that occurs when the following acid and bases are reacted. a) Hydrochloric acid and sodium hydroxide. b) Sulfuric acid and potassium hydroxide. c) Nitric acid and calcium hydroxide. d) Phosphoric acid and lithium hydroxide. e) Sulfuric acid and aluminum hydroxide. 2. Calculate the concentration of a solution of KOH if ml of the base is needed to neutralize 22.5 ml of mol/l acid HNO Determine the volume of mol/l LiOH required to neutralize 56.0 ml of mol/l H 2 SO What volume of mol/l H 2 SO 4 can be neutralized by 50.0 ml of M NaOH? 5. Calculate the concentration of the acid, if 25.0 ml of H 3 PO 4 is required to neutralize 19.0 ml of mol/l KOH. 6. What volume of mol/l HCl is required to just neutralize 10.0 g of solid NaOH? 7. What volume of mol/l nitric acid is needed to just neutralize 25.0 g of magnesium hydroxide? 8. What mass of calcium hydroxide is needed to just neutralize ml of mol/l HCl? Assume the volume does not change mol/l ml ml mol/l L L g 16
17 Titrations Worksheet 1. I titrated 3.5 ml of NaOH with 25 ml of 5.0 x 10 2 M HCl. Find the concentration of this base and determine its ph. (0.36 M, 13.6) 2. If it took me 25.4 ml of 5.0 mm HCl to titrate 50.0 ml of a strong basic solution with unknown concentration, what were the concentration and ph of the basic solution? (2.54 x 10 3 M, 11.4) 3. How many ml of M NaOH will be required to neutralize 10.0 ml of HCl with a ph of 1.0? (100 ml) 17
18 ANSWER THE FOLLOWING QUESTIONS ON TITRATIONS: 1. A sample of vinegar is titrated with a mol/l sodium hydroxide solution, to determine the concentration of acetic acid. Given the following data, a. Calculate the concentration of acetic acid in the vinegar for each trial. b. Calculate the average concentration over the three trials. (0.830 mol/l) 2. The neutralization of g of an unknown monoprotic solid acid required ml of mol/l NaOH. Calculate the molar mass of the acid. (200 g/mol) 3. A sample of a monoprotic acid (molar mass g/mol) is dissolved in enough water to make ml of solution. A ml aliquot of the acid solution is titrated with a mol/l solution of NaOH. If ml is required to reach the endpoint, what is the mass of the original sample? (3.02 g) 18
19 4. Aspirin tablets are made of acetylsalicylic acid (ASA) and fillers. An Aspirin tablet with mass of g was powdered, suspended in water and titrated with mol/l NaOH solution. If it requires ml of NaOH solution to reach the endpoint, how much ASA does the tablet contain? ASA is a monoprotic acid with a formula of C 9 H 8 O 4. (0.319 g) 5. A student pipetted 25.0 ml of an aqueous solution of an unknown monoprotic acid into an Erlenmeyer flask, added about 25 ml of water and titrated with a standard mol/l sodium hydroxide solution. The ph was measured after each addition. The graph below shows the graph obtained. Use the graph to answer the following questions. a. What was the concentration of the unknown acid? (0.104 mol/l) b. What would be a suitable range for an indicator to change colour for this titration? 19
20 Acids and Bases Review 1. Explain how the Lewis definition of a base is different from that of the Arrhenius definition of a base. Are Arrhenius bases also bases under the Lewis definition? Explain. 2. Determine the type of reaction occurring below. If possible label the conjugate acidbase pair in the appropriate place (Think about what is taking place in the reaction). a. H 2 SO 4 + H 2 O HSO H 3 O b. Ca(OH) HNO 3 Ca(NO 3 ) H 2 O c. NaCl Na + + Cl 3. What s the ph of a 3.3 x 10 5 M NaOH solution? 4. Find the ph of a M acetic acid solution. Ka = 1.8 x 10 5 (3.5) 5. What is the ph of a solution that contains 2.4 x 10 5 moles of hydrobromic acid in 0.50 L of water? (4.3) 20
21 6. What is the ph of a solution that contains 25 moles of nitric acid dissolved in 5000 L of water? (2.30) 7. In a few steps, describe how you would titrate a base of unknown concentration with an acid with concentration of 1 M. 8. I did a titration where it took 50 ml of 0.1 M hydrochloric acid to neutralize 500 ml of a base with unknown concentration. Using this information, what was the concentration of the base? (0.01 M) 9. I did a titration where it took 25 ml of 5 M NaOH to neutralize 1000 ml of an acid with unknown concentration. Using this information, what was the concentration of acid? (0.125 M) 10. If it takes 560 ml of M NaOH to neutralize ml of H 2 SO 4 solution with unknown concentration, what was the original ph of the H 2 SO 4 solution? ( 1.9) 21
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
More informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationUnit #6, Chapter 8 Outline Acids, Bases and ph
Lesson Topics Covered 1&2 Review of Acids from Grade 11 Arrhenius acids and bases, definition chemical properties of acids & bases naming acids and bases Unit #6, Chapter 8 Outline Acids, Bases and ph
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 informationO + (aq) In this reaction, the water molecule is a Brønsted-Lowry base. It accepts a proton from HF to form H 3
AcidBase Reactions Key Terms conjugate base conjugate acid amphoteric neutralization salt In the previous sections, you learned about three acidbase theories: Arrhenius, BrønstedLowry, and Lewis. The BrønstedLowry
More informationA) 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 informationAcids 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 informationUnit 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 informationWelcome to AP Chemistry!
Welcome to AP Chemistry! Students enrolled in AP chemistry will be asked to reinforce skills and knowledge accumulated in the first year chemistry class (Honors Chemistry) during the summer before the
More informationAcids 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 informationAcids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.
Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others
More information1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation
NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
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 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 informationUNIT SEVEN PROBLEM SET CHEMISTRY LEE
CHEMISTRY LEE NAME DATE BLOCK UNIT SEVEN PROBLEM SET Score: Do not cheat by copying the work of another person, or by allowing another person to copy your answers. Cheating results in a 0% grade for both
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 informationACID BASE TEST (2 nd half of class) Acid-base titration lab 2 nd half. Chapter 18 Acids and Bases Campbell Chemistry Name
Date In Class 3/31 Thurs. Equilibrium Test Homework (to be done that night, or before coming to the next class) Watch Acid Base Video 1. What are Acids and Bases? 4/1 Fri Video 1 discussion: Identifying
More informationUnit 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 informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationAnswers to Unit 6, Lesson 01: Review of Acids and Bases. A substance that dissolves in water to produce H+ ions
Answers to Unit 6, Lesson 01: Review of Acids and Bases Property Acids Bases Arrhenius Definition How to recognize from a chemical formula A substance that dissolves in water to produce H+ ions the first
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
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 informationAcid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.
Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators
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 informationUnit 7, Lesson 08: The ph of Salt Solutions, Answers
1. Complete the following chart: Unit 7, Lesson 08: The ph of Salt Solutions, Answers on NH 4 PO 3 3- Parent Acid or Base s the parent strong or weak? Will this ion hydrolyze? f the ion will hydrolyze
More information-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form
NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:
More informationSCH4U Chapter 8 review
Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationREVIEW QUESTIONS Chapter The alcohol in gasohol burns according to the equation shown below:
Chemistry 101 REVIEW QUESTIONS Chapter 4 1. The alcohol in gasohol burns according to the equation shown below: C2H5OH (l) + 3 O2 (g) 2 CO2 (g) + 3 H2O l) How many grams of CO2 are produced when 3.00 g
More informationChapter 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 informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
More informationAcids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh
Honors Chemistry Name Acids and Bases Review Worksheet II Date / / Period Solute Name of Solute Molar Mass grams mole Molarity moles L Normality [H 3 O +1 ] [OH ] ph poh Acidic or Basic 1. HCl Hydrochloric
More informationDue Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment
Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment 2017-2018 You will have a quiz on the first day of school (August 16 th, 2017) on the polyatomic
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 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 informationName: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.
Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following
More informationChapter 16. Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic sour milk, sore muscles acetic vinegar phosphoric soft drinks citric citrus fruits malic apples PROPERTIES OF ACIDS PROPERTIES OF BASES 1. Taste sour 1. Taste bitter 2. react
More informationDuncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) 1. hydro- - HF 2. root of
More informationIndicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus
Unit 9: Acids and Bases Notes Introduction and Review 1. Define Acid: 2. Name the following acids: HCl H2SO4 H2SO3 H2S 3. Bases usually contain 4. Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Properties
More informationCHAPTER Acid & Base
CHAPTER 19 19.1 Acid & Base Common Reactions with Acids Dilute: small amount of solute 1-M Concentrated: large amount of solute Indicator: changes color to show the presence of acids or bases : eat or
More informationU N I T T E S T P R A C T I C E
South Pasadena Honors Chemistry Name 6 Compounds Period Date U N I T T E S T P R A C T I C E Section 1: Multiple Choice. Select the best answer choice for each question. (1 point each) 1. Bonds between
More informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
More informationProblem Solving. ] Substitute this value into the equation for poh.
Skills Worksheet Problem Solving In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationUNIT 5 Assignment Acid-Base EQUILIBRIUM (Chap 4-pg & Chap 15-pg 667 & Chap 16 pg 701)
UNIT 5 Assignment Acid-Base EQUILIBRIUM (Chap 4-pg 161-169 & Chap 15-pg 667 & Chap 16 pg 701) The following refer to H 2 O (l) + 58 kj H + (aq) + OH (aq) Kw=1x10 14 5:1. a) Does the thermodynamic trend
More informationTopic 9: Acids & Bases
Topic 9: Acids & Bases Regents Chemistry Mr. Mancuso Electrolytes Substances that conduct electricity when Include Ability to conduct electricity is due to the presence of Dissociation: ~ 1 ~ Acids and
More informationChapter 14 Acids and Bases
Chapter 14 Acids and Bases General Properties of Acids 1. An acid tastes sour - acidus = Latin, sour; acetum= Latin, vinegar 2. An acid turns indicator dye litmus from blue to red. 3. An acid reacts with
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) Practice: 1. hydro- - HF
More informationINTRODUCTION TO ACIDS AND BASES
INTRODUCTION TO ACIDS AND BASES ALIGNED STANDARDS S.C. 912.P.8.11 Relate acidity and basicity to hydronium and hydroxide concentration and ph. S.C.912.N.1.2 Describe and explain what characterizes science
More informationGrace 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 informationOWL Assignment #2 Study Sheet
OWL Assignment #2 Study Sheet Binary Acid Nomenclature Binary compounds are composed of two elements. When one of the elements is a binary acid can be formed. Examples of this are HCl or H 2 S. When put
More informationCHAPTER 19. Acids, Bases, and Salts Acid Base Theories
CHAPTER 19 Acids, Bases, and Salts 19.1 Acid Base Theories ACIDS tart or sour taste Electrolytes Strong acids are corrosive Acid Facts... indicators will change color Blue litmus paper turns pink react
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 informationAcids 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 informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationINTRODUCTION TO CHEMISTRY: PRACTICE AND STUDY GUIDE E. KENNEDY, REVIEWED BY J. HONG, P. LIPPERT
INTRODUCTION TO CHEMISTRY: PRACTICE AND STUDY GUIDE E. KENNEDY, REVIEWED BY J. HONG, P. LIPPERT CONCEPTS INTRODUCTORY CONCEPTS: DEFINITIONS Intensive property property that is independent of the quantity
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 informationWeek 6 AB Strength, ph, Kw, Acids
Week 6 AB Strength, ph, Kw, Acids Q UEST IO N 1 A 0.1 M solution of an electrolyte has a ph of 4.0. What is the electrolyte? A. a strong acid B. a strong base C. a weak acid D. a weak base E. a salt of
More informationIonic Compound Solubility. Ionic Compound Solubility. Nitrates (NO 3 - ) Chlorates (ClO 3 - ) Ionic Compound Solubility. Ionic Compound Solubility
Nitrates (NO 3 - ) Chlorates (ClO 3 - ) Perchlorates (ClO 4 - ) Acetates (C 2 H 3 O 2 - ) Alkali Metal Compounds (Li +,Na +,K +,Rb +,Cs + ) Ammonium Compounds (NH 4 + ) Chlorides (Cl - ) Bromides (Br -
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 informationHonors Unit 4 Homework Packet
1 Honors Homework Packet Reactions in Aqueous Solutions Part I: Aqueous Solns. Part II: Acid/Base Chemistry Part III: Redox Reactions Name: 2 Molarity of Solutions (pg. 2 & 3) Directions: Solve each of
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationRecall, that water is amphoteric. That is, it can act as both an acid and a base.
C4S: ACID BASE EQULIBRIUM LESSON 2 NOTES: WATER Ionization of Water Recall, that water is amphoteric. That is, it can act as both an acid and a base. HA + H2O(l) H3O + (aq) + A (aq) or B + H2O(l) BH +
More informationDynamic 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 informationAP Chemistry Summer Assignment
AP Chemistry Summer Assignment Due Date: Thursday, September 1 st, 2011 Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number of significant
More informationI. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*
Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in
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 informationChapter 5: Nomenclature
Chem 1025 Prof George W.J. Kenney, Jr Introductory Chemistry, Zumdahl Decoste, 6th ed Last Update: 21July09 Chapter 5: Nomenclature These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the
More informationUnit 9: Acids and Bases Chapter 19
Unit 9: Acids and Bases Chapter 19 I. Introduction In aqueous solutions, the solvent is. Aqueous solutions contain. In the self-ionization of water, the hydrogen ion (H+) exists in solution as the ion.
More information[H+] M [OH-] M ph poh
ph and poh Name: Date: Period: 1. What is ph a measure of? 2. What is the equation used for finding ph? 3. What is the equation that relates to ph and poh? 4. Complete the following table: (first one is
More informationNaming Bases: Bases are named just as any other ionic compound. Name the metal first, then the name of anion.
Name AP Unit 9: Acids and Bases Everything you should know already Naming Acids: Acids are named using a unique classification system. There are 3 general guidelines: If the anion ends in ide name the
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
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 informationCHEM 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 informationProton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College
16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
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 informationNeutral Solutions. Will not change the color of litmus. Colorless in phenolphthalein. - Electron pair donor [OH - ] = 10-7 M MEDIUM
Lecture Notes for Chapter 16: Acids and Bases I. Acids and Bases a. There are several ways to define acids and bases. Perhaps the easiest way to start is to list some of the properties of acids and bases.
More informationAP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry
HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance
More informationObj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH.
Do Now Date: April 13, 2015 Obj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH. HCl + KOH KCl(aq) + H 2 O(l) Practice
More informationReaction Classes. Precipitation Reactions
Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
More informationACID 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 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 informationCh 4-5 Practice Problems - KEY
Ch 4-5 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
More informationChapter 2. The Components of Matter
Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties
More informationHelp! I m Melting, wait...i m dissolving! Notes (Ch. 4)
Aqueous Solutions I. Most reactions happen. II. Aqueous means. III. A solution is a. IV. Dissolving occurs when water and/or. V. Electrolytes:. A. In solution, ionic compounds dissolve into. B. molecular
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 14: ACIDS AND BASES
CHAPTER 14: ACIDS AND BASES Arrhenius Acids and Bases There are a few definitions of acids and bases, some are somewhat narrow and others are much broader. Arrhenius Acids dissociate when dissolved in
More informationPractice Examination #8B
Practice Examination #8B Name: Date: 1. Equal volumes of 0.5 M HCl and 0.5 M NaOH are mixed. The total volume of the resulting mixture is 2 liters. The ph of the resulting solution is 1. A. 1 B. 2 C. 7
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 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 informationDo Now April 24, 2017
Do Now April 24, 2017 Obj: Observe and describe neutralization reactions. Copy: Neutralization is when an acid and base react to product a salt and water. e.g. HCl + NaOH NaCl + H 2 O acid base salt water
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 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 information