Whitten Ch. 18

Calculate the pH of a 0.10 M solution of a hypothetical triprotic acid H3A, with Ka1 = 6.0 × 10−3, Ka2 = 2.0 × 10−8, and Ka3 = 1.0 × 10−14. a. 1.48 b. 1.61 c. 1.66 d. 1.84 e. 2.06

c. 1.66

Which one of the following is a soluble strong electrolyte? a. HNO2 b. H2CO3 c. Ca(OH)2 d. Mg(OH)2 e. BaCO3

c. Ca(OH)2

A 0.10 M solution of which of the following salts is neutral? a. NH4F b. NH4NO2 c. NH4CH3COO d. NH4OCl e. NH4CN

c. NH4CH3COO

Consider solutions of the five indicated salts dissolved in water. Which one could not possibly have the pH designated? Salt Solution pH a. NaCl 7.00 b. NaF 8.16 c. NH4Cl 7.64 d. KCN 9.48 e. NH4NO3 5.90

c. NH4Cl 7.64

The pH of a solution of hydrochloric acid is 2.80. What is the molarity of the acid? a. 6.3 × 10−3 M b. 4.2 × 10−3 M c. 1.6 × 10−3 M d. 6.3 × 10−2 M e. 4.2 × 10−2 M

c. 1.6 × 10−3 M

Calculate the value of [H3O+] in a 0.18 M solution of aqueous aniline. Kb = 4.2 × 10−10 a. 1.2 × 10−9 M b. 8.7 × 10−6 M c. 2.0 × 10−5 M d. 1.0 × 10−7 M e. 4.2 × 10−10 M

a. 1.2 × 10−9 M

The hydronium ion concentration in an aqueous solution at 25oC is 6.1 x 10-2M. What is the pH of this solution? a. 1.21 b. 12.79 c. 8.21 d. 7.90 e. 11.20

a. 1.21

The pH of a solution of Ba(OH)2 is 9.40. What is the molarity of this solution of base? a. 1.3 × 10−5 M b. 1.8 × 10−5 M c. 6.0 × 10−4 M d. 8.3 × 10−4 M e. 2.5 × 10−5 M

a. 1.3 × 10−5 M

What is the value of [OH−] in a 0.015 M CH3COOH solution? Ka = 1.8 × 10−5 a. 1.9 × 10−11 M b. 2.0 × 10−6 M c. 1.0 × 10−9 M d. 5.0 × 10−8 M e. 5.0 × 10−7 M

a. 1.9 × 10−11 M

Calculate the [H3O+] in 0.010 M HOCl solution. Ka = 3.5 × 10−8 a. 1.9 × 10−5 M b. 3.6 × 10−5 M c. 5.8 × 10−5 M d. 4.0 × 10−6 M e. 7.2 × 10−6 M

a. 1.9 × 10−5 M

Calculate the pH in a 0.025 M Ca(OH)2 solution. a. 12.70 b. 12.40 c. 1.30 d. 1.60 e. No way to calculate without Kb

a. 12.70

The pH of a solution is −0.38. What is the concentration of H3O+ ions in this solution? a. 2.4 M b. 0.42 M c. −0.42 M d. 4.2 × 10−7 M e. 11.6 M

a. 2.4 M

What is the hydronium-ion concentration of a 0.0029 M KOH solution? a. 3.4 × 10-12 M b. 2.9 × 10-3 M c. 1.0 × 10-14 M d. 1.0 × 10-7 M e. 2.9 × 10-17 M

a. 3.4 × 10-12 M

What is the [OH−] in a 0.25 M hypobromous acid (HOBr) solution? Ka = 2.5 × 10−9 a. 4.0 × 10−10 M b. 2.5 × 10−9 M c. 1.0 × 10−7 M d. 2.5 × 10−5 M e. 2.0 × 10−10 M

a. 4.0 × 10−10 M

Calculate the pKa for a weak acid, HA, that is 2.3% ionized in 0.080 M solution? a. 4.37 b. 4.71 c. 1.66 d. 2.33 e. 3.09

a. 4.37

What is the concentration of H3O+ ions in a solution in which pH = 4.32? a. 4.8 × 10−5 M b. 6.2 × 10−4 M c. 5.1 × 10−4 M d. 8.6 × 10−5 M e. 3.5 × 10−4 M

a. 4.8 × 10−5 M

Calculate the value of [H3O+] in a 0.010 M HOBr solution. Ka = 2.5 × 10−9 a. 5.0 × 10−6 M b. 5.0 × 10−5 M c. 2.5 × 10−7 M d. 2.5 × 10−11 M e. 5.0 × 10−7 M

a. 5.0 × 10−6 M

What is the pH of a 0.30 M FeCl2 solution? The hydrated ferrous ion is [Fe(OH2)6]2+. For [Fe(OH2)6]2+, Ka = 3.0 × 10−10 a. 5.02 b. 4.41 c. 3.76 d. 3.22 e. 2.86

a. 5.02

Calculate the pH of 0.15 M NH4NO3 solution. a. 5.04 b. 5.20 c. 5.36 d. 8.80 e. 8.96

a. 5.04

The value of Kb for methylamine, (CH3)2NH, is 7.4 × 10−4. What is the pH of a solution containing 0.32 M dimethyl ammonium ion, (CH3)2NH2+? a. 5.68 b. 6.58 c. 8.32 d. 5.43 e. 4.34

a. 5.68

What is the [OCl−] in 0.10 M hypochlorous acid, HOCl? Ka = 3.5 × 10−8 a. 5.9 × 10−5 M b. 8.4 × 10−4 M c. 6.1 × 10−4 M d. 4.2 × 10−6 M e. 3.6 × 10−7 M

a. 5.9 × 10−5 M

How many milligrams of HCl are contained in a 250. mL sample of a solution of hydrochloric acid with pH = 3.15? a. 6.46 mg b. 25.8 mg c. 103 mg d. 2.83 mg e. 0.177 mg

a. 6.46 mg

What is the concentration of A3− ions at equilibrium for a 0.10 M solution of a hypothetical triprotic acid H3A, with Ka1 = 6.0 × 10−3, Ka2 = 2.0 × 10−8, and Ka3 = 1.0 × 10−14? a. 9.1 × 10−21 M b. 6.2 × 10−18 M c. 3.1 × 10−15 M d. 1.0 × 10−14 M e. 4.8 × 10−19 M

a. 9.1 × 10−21 M

Which of the following anions is the strongest base? a. ClO− b. ClO3− c. ClO4− d. Cl− e. I−

a. ClO−

Which of the following acid / base pairs produce basic salts when they react? a. HCN / Ca(OH)2 b. H2SO4 / LiOH c. HCl / NaOH d. Both (a) and (b). e. None of these choices.

a. HCN / Ca(OH)2

Assume that five weak acids, identified only by numbers (I, II, III, IV, and V), have the following ionization constants. Acid Ionization Constant (Ka value) I. 1.0 × 10−3 II. 3.0 × 10−5 III. 2.6 × 10−7 IV. 4.0 × 10−9 V. 7.3 × 10−11 The anion of which acid is the weakest base? a. I b. II c. III d. IV e. V

a. I

Which answer includes all of the following true statements about 0.10 M H3PO4 solution? I. The species present in highest concentration is nonionized H3PO4. II. The species present in highest concentration is H2PO4− ion. III. The species present in lowest concentration is PO43− ion. IV. Ka2 > Ka3 a. I and IV b. II and IV c. I and III d. II and III e. I, III and IV

a. I and IV

Which of the following is the correct equilibrium expression for an aqueous solution of hydrocyanic acid, HCN: a. Ka = [H+][CN-]/[HCN] b. Ka = c. Ka = [H+][CN-] d. Ka = e. Ka = [H+][CN-][HCN]

a. Ka = [H+][CN-]/[HCN]

A 0.10 M solution of which of the following salts is most acidic? a. NH4F b. NH4NO2 c. NH4CH3COO d. NH4OCl e. NH4CN

a. NH4F

Aqueous solutions of one of the following is acidic. Which one? a. NH4NO2 b. NH4CH3COO c. NH4OCl d. NH4OBr e. NH4CN

a. NH4NO2

Which of the following is a soluble, strong base? a. Sr(OH)2 b. NH2OH c. Fe(OH)3 d. Cr(OH)3 e. Be(OH)2

a. Sr(OH)2

If enough base is added to a solution to cause the pH to increase from 7.0 to 9.0, the ____. a. [OH−] increases by a factor of 100 b. [OH−] increases by a factor of 0.010 c. [OH−] increases by 2 M d. [OH−] increases by a factor of 9/7 e. [OH−] increases by a factor of 2

a. [OH−] increases by a factor of 100

Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10-4 Formic acid, HCHO2, 1.7 × 10-4 Lactic acid, HC3H5O3, 1.3 × 10-4 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC7H5O2, 6.3 × 10-5 Given initially equimolar solutions of each weak acid, which solution will have the highest hydronium ion concentration once equilibrium is established? a. cyanic acid b. benzoic acid c. lactic acid d. formic acid e. propionic acid

a. cyanic acid

If 1.0 mole of ammonium cyanide, NH4CN, was dissolved in 1.0 liter of water, the pH of the solution would be ____. For NH3: Kb = 1.8 × 10−5 For HCN: Ka = 4.0 × 10−10 a. greater than 7 b. impossible to predict c. equal to 7 d. less than 7 e. close to 1

a. greater than 7

The molar concentration of the Ca2+ ion is ____ and the molar concentration of OH− ion is ____ in 0.015 M calcium hydroxide. a. 0.015 M; 0.015 M b. 0.015 M; 0.030 M c. 0.030 M; 0.015 M d. 0.030 M; 0.030 M e. not enough information to calculate

b. 0.015 M; 0.030 M

What is the hydronium ion (H3O+) concentration of an aqueous HCl solution that has a pOH of 9.040? a. 7.01 x 10-3 b. 1.10 x 10-5 c. 4.96 x 10-8 d. 3.98 x 10-10 e. 9.12 x 10-10

b. 1.10 x 10-5

Calculate the [H3O+] in 0.030 M potassium fluoride, KF. a. 2.5 × 10−8 M b. 1.5 × 10−8 M c. 8.3 × 10−9 M d. 6.8 × 10−4 M e. 5.5 × 10−9 M

b. 1.5 × 10−8 M

The hydronium ion concentration in an aqueous solution at 25oC is 6.1 x 10-2M. What is the hydroxide ion concentration in this solution? a. 6.1 x 10-2 b. 1.6 x 10-13 c. 6.1 x 10-16 d. 1.3 x 10-6 e. 7.8 x 10-16

b. 1.6 x 10-13

Calculate the acid ionization constant of an unknown monoprotic weak acid, HA, if its salt, NaA, has a (base) hydrolysis constant of 6.2 × 10−9. a. 6.0 × 10−7 b. 1.6 × 10−6 c. 4.5 × 10−7 d. 5.6 × 10−8 e. 4.3 × 10−6

b. 1.6 × 10−6

Calculate the pH of a 0.050 M Fe(NO3)3 solution. The hydrated Fe3+ ion is [Fe(OH2)6]3+. For [Fe(OH2)6]3+, Ka = 4.0 × 10−3 a. 1.76 b. 1.85 c. 1.90 d. 2.02 e. 2.26

b. 1.85

What is the value of the (base) hydrolysis constant for NaNO2, sodium nitrite? Ka = 4.5 × 10−4 for HNO2. a. 4.5 × 10−4 b. 2.2 × 10−11 c. 4.5 × 10−18 d. 4.5 × 1010 e. 2.1 × 10−9

b. 2.2 × 10−11

Calculate the pH of a 0.10 M solution of BeCl2 in water. The hydrated beryllium ion is [Be(OH2)4]2+. For [Be(OH2)4]2+, Ka = 1.0 × 10−5 a. 5.50 b. 3.00 c. 1.57 d. 3.74 e. 1.89

b. 3.00

Calculate the pH of a solution of acetic acid that is 3.0% ionized. Ka = 1.8 × 10−5 a. 2.64 b. 3.24 c. 2.94 d. 4.99 e. 4.70

b. 3.24

What is the pH of 400. mL of solution containing 0.0112 gram of HNO3? a. 4.15 b. 3.35 c. 10.65 d. 3.75 e. 2.95

b. 3.35

What is the hydrogen ion concentration in a solution having a pOH of 3.62? a. 2.6 × 10−11 M b. 4.2 × 10−11 M c. 3.8 × 10−4 M d. 3.8 × 10−4 M e. 5.1 × 10−10 M

b. 4.2 × 10−11 M

What is the pH of a 0.10 M CuCl2 solution? For [Cu(OH2)4]2+, Ka = 1.0 × 10−8 a. 4.40 b. 4.49 c. 4.58 d. 4.63 e. 4.68

b. 4.49

Calculate the value of [H3O+] in a 0.25 M solution of aqueous ammonia. Kb = 1.8 × 10−5 a. 2.1 × 10−3 M b. 4.7 × 10−12 M c. 2.3 × 10−9 M d. 4.3 × 10−10 M e. 2.4 × 10−11 M

b. 4.7 × 10−12 M

Calculate the pH of 0.10 M HCN solution. Ka = 4.0 × 10−10 a. 6.75 b. 5.20 c. 8.42 d. 9.52 e. 10.4

b. 5.20

Dichloroacetic acid is a weak monoprotic acid. A 0.100 M solution of this acid has [H3O+] = 0.0070 M. What is the value of Ka for Cl2HCCOOH? The reaction is Cl2HCCOOH + H2O H3O+ + Cl2HCCOO− a. 1.8 × 10−3 b. 5.3 × 10−4 c. 7.5 × 10−3 d. 1.9 × 103 e. 11.6

b. 5.3 × 10−4

Consider the reaction NH3(aq) + H2O(l) NH4+(aq) + OH-(aq). Kb for NH3 is 1.8 × 10-5 at 25°C. What is Ka for the NH4+ ion at 25°C? a. 5.6 × 104 b. 5.6 × 10-10 c. 1.8 × 10-5 d. 7.2 × 10-12 e. 9.2 × 10-8

b. 5.6 × 10-10

Calculate the pH of 0.020 M (CH3)3NHBr. a. 4.93 b. 5.78 c. 11.57 d. 8.17 e. 4.09

b. 5.78

The pH of a 0.12 M solution of a weak base is 10.30. What is the value of pKb for this weak base? a. 3.70 b. 6.48 c. 10.30 d. 5.44 e. 4.49

b. 6.48

Calculate the [H3O+] in a 0.10 M solution of NH4NO3. a. 1.7 × 10−5 M b. 7.5 × 10−6 M c. 2.2 × 10−6 M d. 5.8 × 10−7 M e. 1.3 × 10−9 M

b. 7.5 × 10−6 M

Calculate the [OH−] in a 0.20 M NH4Cl solution. a. 1.3 × 10−9 M b. 9.5 × 10−10 M c. 1.0 × 10−7 M d. 1.2 × 10−6 M e. 1.7 × 10−4 M

b. 9.5 × 10−10 M

The value of Ka for phenol, C6H5OH, is 1.00 x 10-10. Which of the equations below illustrates this reaction for phenol? a. C6H5OH(aq) + H2O(l) C6H5OH2+(aq) + OH-(aq) b. C6H5OH(aq) + H2O(l) C6H5O-(aq) + H3O+(aq) c. C6H5OH(aq) + OH-(l) C6H5O-(aq) + H2O(l) d. C6H5OH(aq) + H3O+(aq) C6H5OH2+(aq) + H2O(l) e. C6H5O-(aq) + H3O+(aq) C6H5OH(aq) + H2O(l)

b. C6H5OH(aq) + H2O(l) C6H5O-(aq) + H3O+(aq)

Which electrolyte is not correctly matched? a. KClO3 / soluble salt b. HCN / weak base c. Ba(OH)2 / strong soluble base d. HNO3 / strong acid e. (NH4)2SO4 / soluble salt

b. HCN / weak base

For the following reaction, K > 1. C8H10N4O2(aq) + HF(aq) F-(aq) + HC8H10N4O2+(aq) Which is the strongest Brønsted-Lowry acid? a. C8H10N4O2 c. F- b. HF d. HC8H10N4O2+

b. HF

Which of the following has the strongest conjugate base? a. HNO3 b. HF c. HBr d. HCl e. H2SO4

b. HF

Which response contains all the salts whose aqueous solutions are acidic, and no other salts? I. NH4NO3 II. NaCN III. KCl IV. NH4Br V. LiCl VI. CaCl2 VII. CH3NH3Cl VIII. KNO2 IX. NH4CH3COO a. II, III, V, VI, and VIII b. I, IV, and VII c. II, VIII, and IX d. I, IV, VII, and IX e. II and VIII

b. I, IV, and VII

Of the following, which acids are weak acids? I. HBr II. HF III. HNO3 IV. HNO2 V. H2CO3 VI. H3PO4 a. I, II, and III b. II, IV, V, and VI c. I, II, and V d. IV, V, and VI e. another combination

b. II, IV, V, and VI

Which one of the following salts produces basic solutions when it is dissolved in water? a. NaNO3 b. NH4OCl c. NH4Br d. NH4I e. KCl

b. NH4OCl

Given the following acids and their Ka values: Phenol, C6H5OH Ka = 1.00 x 10-10 Acetic acid, CH3COOH Ka = 1.80 x 10-5 Nitrous acid, HNO2 Ka = 4.50 x 10-4 What is the order of increasing base strength for C6H5O-, CH3COO-, and NO2-? a. C6H5O- < NO2- < CH3COO- b. NO2- < CH3COO- < C6H5O- c. CH3COO- < C6H5O- < NO2- d. C6H5O- < CH3COO- < NO2- e. CH3COO- < NO2- < C6H5O-

b. NO2- < CH3COO- < C6H5O-

Which one of the following salts is soluble in water? a. AgCl b. NaClO3 c. BaSO4 d. FeS e. CaCO3

b. NaClO3

Which of the following statements about weak acids is false? a. Weak acids ionize only slightly in dilute aqueous solution. b. The Ka values for weak acids are equal to the pH for dilute solutions. c. Weak acids are much more numerous than strong acids. d. Many weak acids are familiar to us in everyday use. e. The ionization constant for a weak acid does not include a term for the concentration of water.

b. The Ka values for weak acids are equal to the pH for dilute solutions.

Which of the following statements about the hydrolysis of AlCl3 and other metal cations is false? a. The Al3+ ions become hydrated in solution to give [Al(H2O)6]3+. b. The aluminum ion hydrolyzes to give a basic solution. c. The positive Al3+ attracts the negative ends of polar water molecules. d. The hydrated cation will be octahedral. e. Smaller, more highly charged cations hydrolyze to a greater extent than larger, less highly charged cations.

b. The aluminum ion hydrolyzes to give a basic solution.

Which of the following relationships in incorrect? Assume 25°C. a. pH + pOH = 14.00 b. [OH−] = 10pOH c. pKW = −log KW d. [OH−] [H3O+] = 1.0 × 10−14 e. pH = −log [H3O+]

b. [OH−] = 10pOH

Which pH or pOH value is incorrectly matched with its description? a. pH = 1.32 / distinctly acidic b. pOH = 13.8 / distinctly basic c. pOH = 7.8 / slightly acidic d. pH = 12.5 / distinctly basic e. pH = 6.7 / slightly acidic

b. pOH = 13.8 / distinctly basic

Which term is not correctly matched with its description? a. weak acid / partially ionized b. salt / cation of an acid, anion of a base c. strong soluble base / soluble metal hydroxide d. weak base / accepts H+ from an acid e. strong electrolyte / strong acid, strong base, or soluble salt

b. salt / cation of an acid, anion of a base

Calculate the pH of a solution that has the H3O+ concentration of 0.50 M. a. −0.30 b. 13.70 c. 0.30 d. 7.30 e. 0.50

c. 0.30

The pH of a 0.100 M solution of a weak acid, HA, is 3.50. Calculate the percent ionization of the acid in 0.100 M solution. a. 0.016% b. 0.078% c. 0.32% d. 0.68% e. 1.6%

c. 0.32%

Which solution would have the lowest [OH−]? a. pure water b. 0.50 M NH3 c. 0.50 M HCl d. 0.10 M NaOH e. 0.10 M NaCl

c. 0.50 M HCl

Calculate the [SO42−] in 0.20 M H2SO4. a. 4.3 × 10−2 M b. 8.4 × 10−2 M c. 1.1 × 10−2 M d. 6.4 × 10−1 M e. 2.5 × 10−1 M

c. 1.1 × 10−2 M

What is the [OH−] in 0.20 M oxalic acid, (COOH)2, solution? a. 4.1 × 10−10 M b. 7.4 × 10−11 M c. 1.2 × 10−13 M d. 3.2 × 10−12 M e. 3.8 × 10−12 M

c. 1.2 × 10−13 M

The ionization constant for the hypothetical weak acid, HA, is 1.0 × 10−5. What is the equilibrium concentration of [H3O+] in 0.20 M HA solution? a. 4.3 × 10−3 M b. 8.1 × 10−4 M c. 1.4 × 10−3 M d. 1.0 × 10−5 M e. 5.0 × 10−4 M

c. 1.4 × 10−3 M

What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.036 M HCl at 25°C? a. 3.3 b. 1.9 c. 1.5 d. 2.7 e. 3.5

c. 1.5

What is the pH of 0.35 M KOBr solution? a. 8.60 b. 9.06 c. 11.07 d. 11.53 e. 13.54

c. 11.07

Calculate the pH of a 0.10 M solution of aqueous ammonia. Kb = 1.8 × 10−5 a. 9.36 b. 10.89 c. 11.11 d. 12.00 e. 2.89

c. 11.11

The pH of a 0.10 M solution of a monoprotic acid is 2.85. What is the value of the ionization constant of the acid? a. 6.3 × 10−5 b. 3.8 × 10−6 c. 2.0 × 10−5 d. 4.0 × 10−8 e. 7.2 × 10−6

c. 2.0 × 10−5

The pH of a 0.20 M solution of a weak monoprotic acid is 3.70. What is the value of the ionization constant for the acid? a. 7.0 × 10−4 b. 4.0 × 10−6 c. 2.0 × 10−7 d. 1.8 × 10−5 e. 6.1 × 10−5

c. 2.0 × 10−7

Calculate the pH of a 0.308 M ascorbic acid solution, H2C6H6O6 (aq). Ka1 = 7.9 x 10-5 and Ka2 = 1.6 x 10-12 a. 0.511 b. 1.781 c. 2.307 d. 3.425 e. 4.614

c. 2.307

Evaluate the (base) hydrolysis constant for sodium cyanate, NaOCN. a. 3.7 × 10−12 b. 6.4 × 10−9 c. 2.9 × 10−11 d. 4.0 × 10−10 e. 6.8 × 10−10

c. 2.9 × 10−11

Calculate the pH of 3.2 × 10−3 M H2CO3 solution. a. 4.09 b. 4.30 c. 4.44 d. 4.94 e. 5.56

c. 4.44

What is the percent ionization of 0.20 M HNO2? Ka = 4.5 × 10−4 a. 1.0% b. 2.8% c. 4.6% d. 5.3% e. 5.9%

c. 4.6%

The hypothetical weak acid H2A ionizes as shown below. Calculate the [A2−] in 0.20 M H2A. H2A H+ + HA− Ka1 = 1.0 × 10−7 HA− H+ + A2− Ka2 = 5.0 × 10−11 a. 1.0 × 10−7 M b. 5.8 × 10−14 M c. 5.0 × 10−11 M d. 4.6 × 10−13 M e. 3.8 × 10−18 M

c. 5.0 × 10−11 M

Ka for formic acid (HCOOH) is 1.8 x 10-4. What is Kb for the formate ion (HCOO-)? a. 1.8 x 10-4 b. 6.9 x 10-6 c. 5.6 x 10-11 d. 4.1 x 10-9 e. 7.9 x 10-6

c. 5.6 x 10-11

Calculate the pH of 0.14 M NaF solution. a. 8.09 b. 8.12 c. 8.14 d. 8.18 e. 8.21

c. 8.14

Calculate the [OH−] in 0.050 M potassium fluoride, KF. a. 4.7 × 10−7 M b. 6.2 × 10−7 M c. 8.3 × 10−7 M d. 1.4 × 10−6 M e. 2.2 × 10−6 M

c. 8.3 × 10−7 M

Calculate the pH of a 0.050 M solution of hydroxylamine, NH2OH. Kb = 6.6 × 10−9 a. 9.91 b. 9.48 c. 9.26 d. 10.56 e. 8.61

c. 9.26

What is the pH of 0.51 M Ca(CH3COO)2 solution? a. 11.1 b. 9.22 c. 9.38 d. 10.7 e. 4.77

c. 9.38

Which one of the following salts produces neutral solutions when it is dissolved in water? a. NH4F b. LiOCl c. BaBr2 d. CaSO3 e. (NH4)2SO4

c. BaBr2

Which one of the following salts produces basic solutions when it is dissolved in water? a. NH4NO3 b. NaBr c. NaF d. NaNO3 e. NaI

c. NaF

Which one of the following salts is insoluble in water? a. CrCl3 b. AgF c. PbSO4 d. Mn(NO3)2 e. Cu(ClO4)2

c. PbSO4

If additional OH− is added to a sample of pure water, which of the following statements is incorrect? a. The equilibrium position shifts to the left. b. The solution becomes more basic. c. The [H3O+] remains unchanged. d. The [OH−] > [H3O+]. e. The amount of non-ionized H2O increases.

c. The [H3O+] remains unchanged.

Which of the following statements about polyprotic acids is incorrect? a. Polyprotic acids can furnish two or more hydronium ions per molecule. b. It is generally accepted practice to ignore second or third ionizations when calculating the concentration of H3O+. c. The ionizations of polyprotic acids occur simultaneously. d. Successive ionization constants for polyprotic acids generally decrease. e. Phosphoric acid is a typical polyprotic acid.

c. The ionizations of polyprotic acids occur simultaneously.

Calculate the concentrations of H3O+ and OH− ions in a 0.25 M HClO4 solution. a. [H3O+] = 0.25 M; [OH−] = 0.25 M b. [H3O+] = 0.25 M; [OH−] = 4.0 M c. [H3O+] = 0.25 M; [OH−] = 4.0 × 10−14 M d. [H3O+] = 0.50 M; [OH−] = 2.0 × 10−14 M e. [H3O+] = 1.0 × 10−7 M; [OH−] = 1.0 × 10−7

c. [H3O+] = 0.25 M; [OH−] = 4.0 × 10−14 M

At 60°C, Kw = 9.6 × 10−14. What are the concentrations of the H3O+ and OH− ions in pure water that is neutral at 60°C? a. [H3O+] = [OH−] = 4.8 × 10−14 b. [H3O+] = [OH−] = 4.8 × 10−7 c. [H3O+] = [OH−] = 3.1 × 10−7 d. [H3O+] = [OH−] = 1.0 × 10−7 e. [H3O+] = 1.0 × 10−7; [OH−] = 9.6 × 10−7

c. [H3O+] = [OH−] = 3.1 × 10−7

Which one of the following salts produces acidic aqueous solutions? a. sodium chloride b. sodium acetate c. ammonium chloride d. calcium nitrate e. rubidium perchlorate

c. ammonium chloride

When solid NH4NO3 is added to water, the pH ____. a. remains at 7 b. becomes greater than 7 c. becomes less than 7 d. is independent of the amount dissolved e. Can not be determined

c. becomes less than 7

A student measured the pH of a 0.15 M solution of chloroacetic acid (ClCH2COOH) to be 1.86. What is the value of Ka for this acid? a. 0.72 b. 0.16 c. 0.099 d. 0.0014 e. 0.00027

d. 0.0014

The pH of a weak monoprotic acid (HA) is 3.75. If the ionization constant for this acid is 8.9 × 10−6, what is the concentration of the weak acid? a. 0.890 M b. 5.05 M c. 0.0500 M d. 0.00355 M e. 0.00712 M

d. 0.00355 M

A 0.010 M aqueous solution of a weak acid HA has a pH of 5.0. What is the degree of ionization of HA in the solution? a. 1 % b. 0.01 % c. 10 % d. 0.1 % e. 0.001 %

d. 0.1 %

Each response gives a pair of solutions. Which pair of solutions should conduct electrical current equally well because they contain equal numbers of ions? a. 0.10 M NH3 and 0.10 M NH4Cl b. 0.10 M HBr and 0.10 M HF c. 0.10 M NaCl and 0.10 M Na2SO4 d. 0.10 M NaNO3 and 0.10 M HNO3 e. 0.10 M HNO3 and 0.10 M HNO2

d. 0.10 M NaNO3 and 0.10 M HNO3

Consider a solution that is 0.10 M in a weak triprotic acid that is represented by the general formula H3A with the following ionization constants. For H3A: Ka1 = 1.0 × 10−3, Ka2 = 1.0 × 10−8, Ka3 = 1.0 × 10−12 What is the concentration of HA2−? a. 4.5 × 10−3 M b. 1.0 × 10−4 M c. 3.2 × 10−5 M d. 1.0 × 10−8 M e. 6.2 × 10−7 M

d. 1.0 × 10−8 M

Calculate the pH of a solution in which [OH−] = 2.50 × 10−4 M. a. 0.40 b. 3.60 c. −3.60 d. 10.40 e. 13.60

d. 10.40

What is the pH of 500. mL of solution containing 0.0124 gram of Ca(OH)2? a. 2.96 b. 3.17 c. 9.68 d. 10.83 e. 11.04

d. 10.83

Calculate the pH of 0.10 M solution of NaBO2. a. 9.84 b. 12.89 c. 10.48 d. 11.11 e. 2.89

d. 11.11

Calculate the pH of 0.050 M Ba(CN)2 solution. Ba(CN)2 is a soluble ionic compound. a. 2.80 b. 2.96 c. 11.04 d. 11.20 e. 12.40

d. 11.20

Calculate the pH of 0.075 M NaOH. a. 10.40 b. 11.12 c. 11.46 d. 12.88 e. 13.26

d. 12.88

Calculate the [HCN] in a 0.20 M KCN solution. a. 8.9 × 10−6 M b. 1.1 × 10−9 M c. 4.5 × 10−12 M d. 2.2 × 10−3 M e. 5.0 × 10−3 M

d. 2.2 × 10−3 M

What is the [OH−] in 0.20 M sodium cyanate, NaOCN, solution? a. 3.7 × 10−7 M b. 4.6 × 10−7 M c. 5.5 × 10−7 M d. 2.4 × 10−6 M e. 8.7 × 10−7 M

d. 2.4 × 10−6 M

Trimethylamine ionizes as follows in water. What concentration of trimethylammonium ion, (CH3)3NH+, is present in 9.0 × 10−2 M (CH3)3N? Kb = 7.4 × 10−5 (CH3)3N + H2O (CH3)3NH+ + OH− a. 1.6 × 10−4 M b. 5.2 × 10−3 M c. 3.8 × 10−4 M d. 2.6 × 10−3 M e. 2.7 × 10−5 M

d. 2.6 × 10−3 M

Calculate the pH of 0.050 M benzoic acid solution. Ka = 6.3 × 10−5 a. 4.20 b. 1.45 c. 5.50 d. 2.75 e. 2.10

d. 2.75

Calculate the (base) hydrolysis constant for the hypochlorite ion, OCl−. a. 3.5 × 10−8 b. 1.8 × 10−5 c. 5.6 × 10−10 d. 2.9 × 10−7 e. 3.5 × 10−6

d. 2.9 × 10−7

What is the pOH of a solution in which [H3O+] = 3.60 × 10−10 M? a. 8.56 b. 5.44 c. 9.44 d. 4.56 e. 4.32

d. 4.56

Calculate the pH of 0.15 M Co(NO3)2. For [Co(OH2)6]2+, Ka = 5.0 × 10−10 a. 4.52 b. 4.74 c. 4.88 d. 5.06 e. 5.28

d. 5.06

What is the equilibrium constant for the following reaction: HCO2- + H2O HCO2H + OH- The Ka value for HCO2H is 1.8 x 10-4 a. 1.8 x 10-4 b. 4.7 x 10-6 c. 9.2 x 10-8 d. 5.6 x 10-11 e. 6.4 x 10-11

d. 5.6 x 10-11

Calculate the hydrolysis constant for the ammonium ion, NH4+. a. 2.5 × 10−5 b. 1.0 × 10−7 c. 4.0 × 10−10 d. 5.6 × 10−10 e. 5.5 × 10−4

d. 5.6 × 10−10

The [H3O+] = 2.0 × 10−4 M for a 0.020 M solution of a weak acid. Calculate the pKa for this acid. a. 1.70 b. 3.70 c. 2.00 d. 5.70 e. 4.69

d. 5.70

What is the [H3O+] in 0.060 M NH4Cl? a. 8.7 × 10−6 M b. 7.6 × 10−6 M c. 6.6 × 10−6 M d. 5.8 × 10−6 M e. 4.5 × 10−6 M

d. 5.8 × 10−6 M

At 40°C, the ion-product constant of water, Kw, is . What is the pH of pure water at 40°C? a. 7.000 b. 6.190 c. 6.870 d. 6.770 e. none of these

d. 6.770

Which of the following statements is false? a. Solvolysis is the reaction of a substance with the solvent in which it is dissolved. b. Hydrolysis is the reaction of a substance with water. c. The anion of a weak acid reacts with water to form nonionized acid and OH− ions. d. According to Brønsted-Lowry the anions of strong acids are very strong bases. e. The conjugate acid of a strong base is a very weak acid.

d. According to Brønsted-Lowry the anions of strong acids are very strong bases.

Which of the following acid / base pairs produce acidic salts when they react? a. HNO3 / NH3 b. HNO3 / (CH3)3N c. HCl / C6H5NH2 d. All of these choices. e. None of these choices.

d. All of these choices.

Which of the following salts produce acidic solutions? a. Al(NO3)3 b. Co(ClO3)2 c. KCl d. Both (a) and (b). e. All of these choices.

d. Both (a) and (b).

Which of the following acid / base pairs produce neutral salts when they react? a. HClO4 / Ba(OH)2 b. HF / KOH c. HBr / LiOH d. Both (a) and (c). e. All of these choices.

d. Both (a) and (c).

Given the following acids and their Ka values: Hydrocyanic acid, HCN Ka = 4.00 x 10-10 Phenol, C6H5OH Ka = 1.00 x 10-10 Benzoic acid, C6H5COOH Ka = 6.30 x 10-5 What is the order of increasing base strength for CN-, C6H5O-, and C6H5COO-? a. C6H5COO- < C6H5O- < CN- b. C6H5O- < C6H5COO- < CN- c. CN- < C6H5COO- < C6H5O- d. C6H5COO- < CN- < C6H5O- e. CN- < C6H5O- < C6H5COO-

d. C6H5COO- < CN- < C6H5O-

Which one of the following is an insoluble base? a. Ca(OH)2 b. Sr(OH)2 c. Ba(OH)2 d. Cu(OH)2 e. CsOH

d. Cu(OH)2

Which of the following is a strong acid? a. HNO2 b. HClO2 c. HBrO d. HClO3 e. H2SO3

d. HClO3

Which one of the following is a weak acid? a. H2SO4 b. HI c. HBr d. HF e. HClO4

d. HF

We make a 1.0 M solution of an unknown acid, HX. With a pH meter, we determine that the pH of the solution is 5.00. Which of the following statements about the HX is true? a. HX is a strong acid. b. HX is a weak acid with a Ka value of about 10−5. c. HX is a weak acid with a Ka value of about 10−8. d. HX is a weak acid with a Ka value of about 10−10. e. HX would probably be a good acid-base indicator.

d. HX is a weak acid with a Ka value of about 10−10.

Which response includes all the following salts that give acidic aqueous solutions, and no other salts? I. AlCl3 II. Cr(NO3)3 III. FeCl3 IV. CaCl2 V. BiCl3 a. I and II b. I, II, III, and IV c. IV d. I, II, III, and V e. II and IV

d. I, II, III, and V

Which of the following statements about measurement of pH is incorrect? a. The pH of a solution can be determined using a pH meter. b. The pH of a solution can be determined by the indicator method. c. A pH meter is more accurate than an indicator for determining the pH. d. Many indicators are strong acids or strong bases. e. Acid-base indicators have different colors in solutions of different pH.

d. Many indicators are strong acids or strong bases.

Which of the following is not a soluble base? a. Sr(OH)2 b. NaOH c. KOH d. Mn(OH)2 e. CsOH

d. Mn(OH)2

Which one of the following substances is not a strong electrolyte? a. NH4Cl b. H2SO4 c. HNO3 d. NH3 e. Mg(NO3)2

d. NH3

The reaction that occurs when NH4Br dissolves in water is ____. a. NH4+ + OH− NH4OH b. Br− + H3O+ HBr + H2O c. NH3 + H2O NH4+ + OH− d. NH4+ + H2O NH3 + H3O+ e. Br− + H2O HBr + OH−

d. NH4+ + H2O NH3 + H3O+

Which one of the following salts does not give a neutral solution when it is dissolved in water? a. KNO3 b. BaCl2 c. Ca(ClO3)2 d. NH4OH e. NaBr

d. NH4OH

Which one of the following salts produces neutral solutions when it is dissolved in water? a. NaCN b. NaOCl c. NaF d. NaBr e. NaCH3COO

d. NaBr

A 0.10 M solution of which of the following would be most basic? a. RbI b. NH4NO3 c. KCH3COO d. NaCN e. BaCl2

d. NaCN

Calculate the concentrations of H3O+ and OH− ions in a 0.050 M Ba(OH)2 solution. a. [H3O+] = 0.050 M; [OH−] = 0.050 M b. [H3O+] = 1.0 × 10−7 M; [OH−] = 0.10 M c. [H3O+] = 2.0 × 10−13 M; [OH−] = 0.050 M d. [H3O+] = 1.0 × 10−13 M; [OH−] = 0.10 M e. [H3O+] = 0.10 M; [OH−] = 1.0 × 10−13 M

d. [H3O+] = 1.0 × 10−13 M; [OH−] = 0.10 M

In a solution containing only a weak monoprotic acid HA, [H3O+] is ____ [A−]; if the solution is not very dilute, the concentration of nonionized HA is approximately equal to the ____ of the solution. a. greater than; molarity b. less than; molarity c. equal to; pH d. equal to; molarity e. less than; pH

d. equal to; molarity

A 0.0367 M solution of a weak base has a pH of 11.59. What is the identity of the weak base? Weak Base Kb Ethylamine (CH3CH2NH2) 4.7 × 10-4 Hydrazine (N2H4) 1.7 × 10-6 Hydroxylamine (NH2OH) 1.1 × 10-8 Pyridine (C5H5N) 1.4 × 10-9 Aniline (C6H5NH2) 4.2 × 10-10 a. hydrazine b. pyridine c. aniline d. ethylamine e. hydroxylamine

d. ethylamine

If 1.0 mole of ammonium nitrite, NH4NO2, was dissolved in 1.0 liter of water, the pH of the solution would be ____. For NH3: Kb = 1.8 × 10−5 For HNO2: Ka = 4.5 × 10−4 a. greater than 7 b. impossible to predict c. equal to 7 d. less than 7 e. close to 14

d. less than 7

Consider an aqueous solution of ammonium hypochlorite. This is a(n) ____ salt. The resulting solution is ____. a. insoluble; acidic b. soluble; acidic c. insoluble; basic d. soluble; basic e. soluble; neutral

d. soluble; basic

When 14.7 mL of aqueous HBr (strong acid) was added to water, 482 mL of a solution with a pH of 4.23 was produced. What was the molarity of the original HBr solution? a. 140 M b. 1.7 M c. 0.29 M d. 0.13 M e. 0.0019 M

e. 0.0019 M

What is the percent hydrolysis of Fe2+ in a 0.30 M FeCl2 solution? a. 0.20% b. 5.2 × 10−4% c. 0.067% d. 0.044% e. 0.0032%

e. 0.0032%

Consider calculations of [H3O+] in each of the following solutions. Do not go through the calculations. For which calculation is it not reasonable to assume that "x" is much less than the initial concentration? The x represents concentration ionized. a. 0.20 M H2O2 Ka = 2.4 × 10−12 b. 0.010 M HCN Ka = 4.0 × 10−10 c. 0.010 M H2S Ka1 = 1.0 × 10−7, Ka2 = 1.0 × 10−19 d. 1.00 M NH3 Kb = 1.8 × 10−5 e. 0.010 M (COOH)2 Ka1 = 5.9 × 10−2, Ka2 = 6.4 × 10−5

e. 0.010 M (COOH)2 Ka1 = 5.9 × 10−2, Ka2 = 6.4 × 10−5

Calculate the percent hydrolysis of the hypochlorite ion in 0.10 M NaOCl solution. a. 0.0012% b. 0.024% c. 0.056% d. 0.10% e. 0.17%

e. 0.17%

Calculate the pOH of a solution that has the OH− concentration of 0.50 M. a. 0.50 b. 14.30 c. 6.70 d. 13.70 e. 0.30

e. 0.30

The hypothetical weak acid H2A ionizes as shown below. Calculate the [HA−] in 0.20 M H2A. H2A H+ + HA− Ka1 = 1.0 × 10−7 HA− H+ + A2− Ka2 = 5.0 × 10−11 a. 6.3 × 10−5 M b. 1.0 × 10−7 M c. 3.0 × 10−4 M d. 2.2 × 10−6 M e. 1.4 × 10−4 M

e. 1.4 × 10−4 M

What is the pOH of 0.013 M HBr solution? a. 9.66 b. 0.013 c. 1.89 d. 4.34 e. 12.11

e. 12.11

What is the pH of a solution which has a hydroxide ion concentration of 2.5 x 10-2M? a. 1.24 b. 1.60 c. 3.69 d. 10.31 e. 12.40

e. 12.40

Calculate the [OH−] in 0.20 M NaNO2. a. 4.8 × 10−9 M b. 1.4 × 10−8 M c. 1.2 × 10−7 M d. 6.5 × 10−7 M e. 2.1 × 10−6 M

e. 2.1 × 10−6 M

Calculate the ionization constant for a weak acid, HA, that is 1.60% ionized in 0.0950 M solution. a. 2.69 × 10−3 b. 3.77 × 10−2 c. 9.91 × 10−6 d. 1.63 × 10−2 e. 2.47 × 10−5

e. 2.47 × 10−5

What is the [H3O+] in 0.40 M NaCN solution? a. 6.4 × 10−10 M b. 3.3 × 10−11 M c. 1.4 × 10−2 M d. 4.8 × 10−3 M e. 3.2 × 10−12 M

e. 3.2 × 10−12 M

In the laboratory, a general chemistry student measured the pH of a 0.583M solution of HClO3 to be 3.862. What is the experimentally determined value of Ka for HClO3? a. 1.37 x 10-4 b. 2.35 x 10-4 c. 3.11 x 10-7 d. 1.89 x 10-8 e. 3.24 x 10-8

e. 3.24 x 10-8

What is the pH of an aqueous solution of 0.184M carbonic acid, H2CO3? (Ka1 = 4.2 x 10-7, Ka2 = 4.8 x 10-11) a. 2.69 b. 2.80 c. 2.97 d. 3.50 e. 3.56

e. 3.56

What is the pH of 0.025 M CuCl2? For [Cu(OH2)4]2+, Ka = 1.0 × 10−8 a. 6.70 b. 9.20 c. 7.30 d. 3.60 e. 4.80

e. 4.80

What is the pH of a 1.0L solution of 0.445 M hydrocyanic acid, HCN? (Ka = 4.0 x 10-10) a. 3.516 b. 4.250 c. 4.602 d. 4.699 e. 4.875

e. 4.875

The percent ionization of a 0.331M solution of HCN is found to be 0.00337%. What is the pH of this solution? a. 1.992 b. 2.953 c. 3.371 d. 3.992 e. 4.953

e. 4.953

What is the pH of 0.15 M solution of trimethylammonium nitrate, (CH3)3NHNO3, a salt? a. 8.66 b. 9.20 c. 8.88 d. 5.12 e. 5.34

e. 5.34

Calculate the pH of 0.030 M NH4Cl. a. 4.78 b. 4.90 c. 5.12 d. 5.28 e. 5.39

e. 5.39

Calculate the pH of 0.050 M CH3NH3Br. a. 4.70 b. 4.15 c. 5.28 d. 5.35 e. 6.00

e. 6.00

The [OH−] = 1.3 × 10−6 M for a 0.025 M solution of a weak base. Calculate the value of Kb for this weak base. a. 5.2 × 10−5 b. 3.1 × 10−7 c. 7.7 × 10−9 d. 4.0 × 10−8 e. 6.8 × 10−11

e. 6.8 × 10−11

How many moles of nitrous acid, HNO2, are required initially to prepare 2.5 liters of a solution of pH = 3.00? Ka = 4.5 × 10−4 a. 1.8 × 10−4 mol b. 6.2 × 10−2 mol c. 1.7 × 10−4 mol d. 3.6 × 10−4 mol e. 8.0 × 10−3 mol

e. 8.0 × 10−3 mol

Which one of the following salts does not produce an acidic aqueous solution? a. NH4Cl b. NH4NO3 c. NH4Br d. NH4I e. NaNO3

e. NaNO3

Assume that five weak acids, identified only by numbers (I, II, III, IV, and V), have the following ionization constants. Acid Ionization Constant (Ka value) I. 5.0 × 10−3 II. 3.0 × 10−5 III. 2.6 × 10−7 IV. 4.0 × 10−9 V. 7.3 × 10−11 A 0.10 M solution of which acid would have the highest pH? a. I b. II c. III d. IV e. V

e. V

In a sample of pure water, only one of the following statements is always true at all conditions of temperature and pressure. Which one is always true? a. [H3O+] = 1.0 × 10−7 M b. [OH−] = 1.0 × 10−7 M c. pH = 7.0 d. pH + pOH = 14.0 e. [H3O+] = [OH−]

e. [H3O+] = [OH−]

A solution having a pH of 1.4 would be described as ____. a. distinctly basic b. slightly basic c. neutral d. slightly acidic e. distinctly acidic

e. distinctly acidic

A solution in which the pOH is 12.5 would be described as ____. a. distinctly basic b. slightly basic c. neutral d. slightly acidic e. distinctly acidic

e. distinctly acidic

For a given weak acid, HA, the value of Ka ____. a. will change with pH b. cannot be less than 10−7 c. cannot be greater than 10−7 d. does not change with temperature e. is calculated from experimental data

e. is calculated from experimental data

What is the percent hydrolysis of a 0.15 M solution of (CH3)3NHNO3? a. 0.0031% b. 0.0068% c. 0.0094% d. 0.011% e. 0.022%

a. 0.0031%

What is the percent hydrolysis in 0.075 M sodium acetate, NaCH3COO, solution? a. 0.0087% b. 0.012% c. 0.0064% d. 0.0038% e. 0.043%

a. 0.0087%

What is the percent ionization for a 1.0 × 10−3 M solution of pyridine? Kb = 1.5 × 10−9 a. 0.12% b. 1.6% c. 2.8% d. 0.045% e. 0.67%

a. 0.12%

What is the pH of a 0.400 M HNO3 solution? a. 0.40 b. 2.05 c. 0.60 d. 4.12 e. 1.67

a. 0.40

Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10-4 Formic acid, HCHO2, 1.7 × 10-4 Lactic acid, HC3H5O3, 1.3 × 10-4 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC7H5O2, 6.3 × 10-5 Which has the strongest conjugate base? a. propionic acid b. benzoic acid c. lactic acid d. formic acid e. cyanic

a. propionic acid

The value of Kb for methylamine, (CH3)NH2, is 5.0 × 10−4. When methylammonium chloride is dissolved in water, the reaction that occurs is ____, resulting in a solution that is ____. a. (CH3)NH2 + H2O (CH3)NH3+ + OH−; basic b. (CH3)NH3+ + H2O (CH3)NH2 + H3O+; acidic c. (CH3)NH3+ + OH− (CH3)NH2 + H2O; acidic d. (CH3)NH3+ + OH− (CH3)NH2 + H2O; basic e. (CH3)NH2 + H3O+ (CH3)NH3+ + H2O; acidic

b. (CH3)NH3+ + H2O (CH3)NH2 + H3O+; acidic

What is the percent ionization of a 1.8 M HC2H3O2 solution (Ka = 1.8 × 10-5 ) at 25°C? a. 0.57 % b. 0.32 % c. 1.8 % d. 0.18 % e. 0.24 %

b. 0.32 %

When salts derived from ____ acids and ____ bases are dissolved in water, the resulting solution is always acidic. a. strong; strong b. strong; weak c. weak; strong d. weak; weak e. no way to determine without Ka and Kb

b. strong; weak

What is the pH of a 0.38 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid, HC3H5O2, Ka = 1.3 × 10-5 at 25°C.) a. 6.11 b. 4.77 c. 11.10 d. 7.89 e. 9.23

e. 9.23

The value of Ka for benzoic acid, C6H5COOH, is 6.3 × 10−5. When sodium benzoate is dissolved in water, the reaction that occurs is ____, resulting in a solution that is ____. a. Na+ + C6H5COO− NaC6H5COO; neutral b. C6H5COO− + H2O H3O+ + C6H4COO2−; acidic c. C6H5COOH + H2O H3O+ + C6H5COO−; acidic d. No reaction; neutral e. C6H5COO− + H2O CH6H5COOH + OH−; basic

e. C6H5COO− + H2O CH6H5COOH + OH−; basic

Which one of the following salts is insoluble in water? a. Ba(CH3COO)2 b. BaCl2 c. CaCl2 d. Ca(NO3)2 e. Ca3(PO4)2

e. Ca3(PO4)2

Which response lists the species present in the highest concentration in a solution of 0.20 M H3PO4? a. H3PO4, H2PO4−, HPO42− b. H2PO4−, HPO42−, PO43− c. H3PO4, H3O+, OH− d. HPO42−, PO43−, OH− e. H3PO4, H2PO4−, H3O+

e. H3PO4, H2PO4−, H3O+

A 0.10 M solution of which of the following salts is most basic? a. NH4F b. NH4NO2 c. NH4CH3COO d. NH4OCl e. NH4CN

e. NH4CN

Which of the following salts are incorrectly matched with its description? a. NH4CH3COO / neutral b. NaOBr / basic c. NH4OCl / basic d. NH4NO3 / acidic e. NH4CN / acidic

e. NH4CN / acidic

Which one of the following salts produces acidic solutions when it is dissolved in water? a. KCH3COO b. KF c. KOCl d. KBr e. NH4NO3

e. NH4NO3

A 0.10 M solution of which of the following salts is most basic? a. NaF b. NaNO2 c. NaCH3COO d. NaOCl e. NaCN

e. NaCN

Which salt is produced from a strong acid and a strong base? a. LiF b. NaBrO c. NH4NO3 d. NaHCO3 e. NaCl

e. NaCl