CHEM Ch. 16 & 17

The molar solubility of CaF2 is 2.15 × 10^-4 M in pure water. Calculate the Ksp for CaF2. A) 1.63 × 10^-12 B) 8.05 × 10^-9 C) 3.97 × 10^-11 D) 4.47 × 10^-12 E) 5.31 × 10^-10

3.97 × 10^-11

A 25.0-mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of benzoic acid is 6.3 × 10^-5. A) 4.19 B) 6.5 × 10^-5 C) 4.20 D) 3.38 E) 2.4 × 10^3

4.19

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6 × 10^-12. A) 1.8 × 10^-10 M B) 5.6 × 10^-9 M C) 2.4 × 10^-6 M D) 1.1 × 10^-4 M

5.6 × 10^-9 M

Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10^-2) and 0.15 M HClO (Ka = 2.9 × 10^-8). A) 4.18 B) 9.82 C) 12.55 D) 1.39 E) 3.55

1.39

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A) 7.1 × 10^-5 M B) 4.2 × 10^-10 M C) 8.7 × 10^-10 M D) 6.5 × 10^-5 M E) 1.4 × 10^-10 M

1.4 × 10^-10 M

Determine the pH of a 0.232 M Ca(OH)2 solution at 25°C. A) 12.73 B) 13.37 C) 13.67 D) 0.333 E) 0.634

13.67

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution before the addition of any KOH. The Ka of HF is 3.5 × 10^-4. A) 4.15 B) 0.70 C) 2.08 D) 3.46 E) 1.00

2.08

What is the pH of a 0.50 M H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10^-4 and Ka2 = 1.0 x 10^-11 A) 2.09 B) 3.89 C) 4.19 D) 5.57

2.09

A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuS) = 1.3 × 10^-36, Ksp(FeS) = 6.3 × 10^-18. A) 1.4 × 10^-16 M, FeS B) 3.6 × 10^-35 M, CuS C) 3.6 × 10^-35 M, FeS D) 1.4 × 10^-16 M, CuS E) No precipitate will form at any concentration of sulfide ion.

3.6 × 10^-35 M, CuS

A solution contains 3.8 × 10^-2 M in Al3+ and 0.29 M in NaF. If the Kf for AlF63- is 7 × 10^19, how much aluminum ion remains at equilibrium? A) 1.1 × 10^-19 M B) 3.1 × 10^-22 M C) 9.1 × 10^-19 M D) 1.9 × 10^-21 M E) 4.4 × 10^-20 M

9.1 × 10^-19 M

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10^-5 for NH3. A) 8.56 B) 9.28 C) 9.95 D) 11.13

9.95

Gives what happens at high pH for aluminum hydroxide. A) Al(H2O)4^3+ dissolves B) Al(H2O)2(OH)4^- dissolves C) Al(OH)6 dissolves D) Al precipitates E) Al dissolves

Al(H2O)2(OH)4^- dissolves

Which of the following is a Lewis acid? A) BCl3 B) CI4 C) NH3 D) CHI3 E) None of the above are Lewis acids.

BCl3

Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00? A) NH4I B) Na2O C) KHCO3 D) Cs Cl

Cs Cl

63) Which of the following compounds will be more soluble in acidic solution than in pure water? A) PbI2 B) CuS C) Ca(ClO4)2 D) CuCl E) None of the above will be more soluble in acidic solution.

CuS

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the soluble ions after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. A) Ba3(PO4)2 B) CdS C) AgCl D) NH4Cl E) FeS

NH4Cl

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 x 10^-10 for HCN A) 2.0 × 10^-10 M B) 4.9 × 10^-10 M C) 1.2 × 10^-9 M D) 7.0 × 10^-6 M

1.2 × 10^-9 M

What is the molar solubility of silver carbonate ( Ag2CO3 ) in water? The solubility-product constant for Ag2CO3 is 8.1 × 10^-12 at 25°C. A) 1.4 × 10^-6 B) 2.0 × 10^-4 C) 4.0 × 10^-6 D) 1.3 × 10^-4 E) 2.7 × 10^-12

1.3 × 10^-4

Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4) = 1.82 × 10^-8. A) 1.82 × 10^-8 M B) 1.35 × 10^-4 M C) 9.1 × 10^-9 M D) 3.31 × 10^-16 M E) 4.48 × 10^-4 M

1.35 × 10^-4 M

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 400.0 mL HBr. A) 1.00 B) 1.40 C) 1.22 D) 1.30 E) 2.11

1.40

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 200.0 mL of HNO3. The Kb of NH3 is 1.8 × 10^-5. A) 6.44 B) 1.48 C) 2.00 D) 12.52 E) 12.00

1.48

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 50.0 mL of LiOH. A) 12.48 B) 0.68 C) 2.35 D) 1.52 E) 3.22

1.52

You have a 0.850 M solution of Na2CrO4 at a given temperature. At what concentration will silver ions need to be added in order for a participate to form? The Ksp for Ag2CrO4 at this temperature is 2.00 × 10^-12. A) 2.35 × 10^-12 M B) 1.37 × 10^-5 M C) 5.02 × 10^-10 M D) 1.53 × 10^-6 M

1.53 × 10^-6 M

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl is 1.8 × 10^-10 and Kf for Ag(NH3)2^+ is 1.7 × 10^7. A) 1.3 × 10^-5 M B)1.6 × 10^-2 M C) 1.7 × 10^-2 M D) 5.5 × 10^-2 M

1.6 × 10^-2 M

What is the molar solubility of zinc oxalate ( ZnC2O4 ) in water? The solubility-product constant for ZnC2O4 is 2.7 × 10^-8 at 25°C. A) 1.4 × 10^-8 B) 5.4 × 10^-8 C) 7.57 D) 2.3 × 10^-4 E) 1.6 × 10^-4

1.6 × 10^-4

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 300.0 mL HBr. A) 1.60 B) 1.30 C) 1.00 D) 12.40 E) 1.12

1.60

Determine the molar solubility of CaSO4 in a solution containing 0.14 M Na2SO4. Ksp (CaSO4) = 2.4 × 10^-5. A) 3.4 × 10^-6 M B) 1.7 × 10^-4 M C) 5.8 × 10^-10 M D) 4.9 × 10^-3 M E) 0.10 M

1.7 × 10^-4 M

Determine the molar solubility for Cd(OH)2 in pure water. Ksp for Cd(OH)2 is 2.0 × 10^-14. A) 2.0 × 10^-14 M B) 1.7 × 10^-5 M C) 6.6 × 10^-8 M D) 3.5 × 10^-6 M E) 2.9 × 10^-6 M

1.7 × 10^-5 M

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10^-5. A) 1.70 B) 6.44 C) 7.56 D) 12.30 E) 2.30

1.70

Determine the molar solubility of BaF2 in pure water. Ksp for BaF2 = 2.45 × 10^-5. A) 1.83 × 10^-2 M B) 1.23 × 10^-5 M C) 2.90 × 10^-2 M D) 4.95 × 10^-3 M E) 6.13 × 10^-6 M

1.83 × 10^-2 M

A solution contains 2.2 × 10^-3 M in Cu2+ and 0.33 M in LiCN. If the Kf for Cu(CN)42- is 1.0 × 10^25, how much copper ion remains at equilibrium? A) 3.8 × 10^-24 M B) 1.9 × 10^-26 M C) 6.7 × 10^-28 M D) 2.9 × 10^-27 M E) 4.6 × 10^-25 M

1.9 × 10^-26 M

Determine the molar solubility for Zn(OH)2 in pure water. Ksp for Zn(OH)2 is 3.00 × 10^-17. A) 3.0 × 10^-17 M B) 7.5 × 10^-18 M C) 3.11 × 10^-6 M D) 1.96 × 10^-6 M E) 5.5 × 10^-19 M

1.96 × 10^-6 M

The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid? A) 4 B) 5 C) 10 D) 15 E) 40

10

Calculate the pH of a 0.800 M KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10^9. A) 2.70 B) 4.40 C) 9.60 D) 11.30

11.30

What is the pOH of a 0.0020 M HNO3 solution? A) 0.0020 B) 0.0040 C) 2.70 D) 11.30

11.30

Calculate the pH of a 0.200 M NaCN solution. The Ka for HCN is 4.9 × 10^-10. A) 3.87 B) 11.31 C) 2.69 D) 10.13

11.31

A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hydrofluoric acid is 6.8 × 10^-4. A) 2.54 B) 11.47 C) 7.00 D) 3.15 E) 3.18

11.47

What is the pH of a solution made by mixing 20.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive. A) 0.48 B) 1.48 C) 12.52 D) 13.52

12.52

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 60.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10^-5 for CH3CO2H. A) 8.26 B) 9.26 C) 11.13 D) 12.52

12.52

Determine the pH of a 0.441 M NaOH solution at 25°C. A) 0.356 B) 13.64 C) 0.441 D) 13.56 E) 0.88

13.64

Determine the molar solubility for Ag2C2O4 in pure water. The Ksp for Ag2C2O4 is 3.5 × 10^-11. A) 1.8 × 10^-11 M B) 1.4 × 10^-6 M C) 5.9 × 10^-6 M D) 2.1 × 10^-4 M E) 3.5 × 10^-6 M

2.1 × 10^-4 M

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2= 4.87 × 10^-17. A) 2.44 × 10^-17 M B) 1.62 × 10^-17 M C) 4.03 × 10^-9 M D) 3.65 × 10^-6 M E) 2.30 × 10^-6 M

2.30 × 10^-6 M

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2= 4.87 × 10^-17. A) 2.44 × 10^-17 M B) 1.62 × 10^-17 M C) 4.03 × 10^-9 M D) 3.65 × 10^-6 M E) 2.30 × 10^-6 M

2.30 × 10^-6 M

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl. Ksp (CuCl) = 1.0 × 10^-6. A) 1.0 × 10^-12 M B) 4.0 × 10^-8 M C) 2.5 × 10^-5 M D) 1.0 × 10^-3 M E) 0.050 M

2.5 × 10^-5 M

Determine the pOH in a 2.58 × 10^-3 M KOH solution. A) 11.4 B) 2.59 C) 9.33 D) 4.67 E) 7.00

2.59

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water. Calculate the Ksp for ZnS. A) 8.0 × 10^-13 B) 3.2 × 10^-12 C) 1.6 × 10^-35 D) 2.6 × 10^-24 E) 6.80 × 10^-5

2.6 × 10^-24

Determine the molar solubility for Al(OH)3 in pure water. Ksp for Al(OH)3 = 1.3 × 10^-33. A) 3.6 × 10^-12 M B) 2.2 × 10^-10 M C) 4.8 × 10^-35 M D) 2.6 × 10^-9 M E) 6.0 × 10^-19 M

2.6 × 10^-9 M

Determine the molar solubility of MgCO3 in pure water. Ksp (MgCO3) = 6.82 × 10^-6. A) 6.82 × 10^-6 M B) 3.41 × 10^-6 M C) 4.65 × 10^-3 M D) 2.61 × 10^-3 M E) 3.25 × 10^-4 M

2.61 × 10^-3 M

What is the hydronium ion concentration of a 0.400 M acetic acid solution with Ka = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O (l) <-> H3O ^+ (aq) + CH3Co2^- (aq) A) 2.7 × 10^-2 M B) 4.2 × 10^-2 M C) 2.7 × 10^-3 M D) 4.2 × 10^-3 M

2.7 × 10^-3 M

What is the pH of a solution prepared by mixing 48.00 mL of 0.25 M H3PO4 with 85.00 mL of 0.85M LiH2PO4? Assume that the volume of the solutions are additive and that Ka = 7.1 × 10^-3 for H3PO4. A) 11.07 B) 2.93 C) 4.31 D) 8.63

2.93

How many of the following are weak acids? HNO2 HClO HNO3 H2PO4⁻ A) 0 B) 1 C) 3 D) 4 E) 2

3

A solution contains 0.021 M Cl⁻ and 0.017 M I⁻. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10^-6, Ksp(CuI) = 5.1 × 10^-12. A) 3.0 × 10^-10 M, CuI B) 3.0 × 10^-10 M, CuCl C) 4.8 × 10^-5 M, CuCl D) 4.8 × 10^-5 M, CuI E) No precipitate will form at any concentration of copper (I).

3.0 × 10^-10 M, CuI

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO3 and 0.10 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10^-12 and 1.2 × 10^-10, respectively. A) 6.5 × 10^-5 M B) 1.3 × 10^-4 M C) 3.2 × 10^-4 M D) 3.0 × 10^-2 M

3.0 × 10^-2 M

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10^-6. A) 2.3 × 10^-5 M B) 8.5 × 10^-7 M C) 1.2 × 10^-2 M D) 0.0750 M E) 3.0 × 10^-4 M

3.0 × 10^-4 M

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HF is 3.5 × 10^-4. A) 3.09 B) 4.11 C) 3.82 D) 3.46 E) 2.78

3.09

The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 × 10-4 at 25.0°C. The [H+] in a 1.6 x 10^-2 M solution of ethylamine is ________ M. A) 3.5 × 10^-12 B) 2.9 × 10^-3 C) 3.1 × 10^-12 D) 3.2 × 10^-3 E) 11.46

3.1 × 10^-12

You wish to prepare an HC2H3O2 buffer with a pH of 5.24. If the pKa of is 4.74, what ratio of C2H3O2⁻/HC2H3O2 must you use? A) 0.10 B) 0.50 C) 0.32 D) 3.16 E) 7.0

3.16

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10^-4. A) 2.08 B) 3.15 C) 4.33 D) 3.46 E) 4.15

3.46

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF. The Ka for HF is 3.5 × 10^4. A) 2.86 B) 9.31 C) 10.54 D) 3.46 E) 4.89

3.46

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2 ) 0.290 M in potassium nitrite (KNO2 ). The acid dissociation constant of nitrous acid is 4.50 ×10^-4 . A) 3.487 B) 3.210 C) 13.86 D) 10.51 E) 4.562

3.487

Determine the molar solubility of BiPO4 in a solution containing 0.358 M K3PO4. The Ksp for BiPO4 is 1.3 × 10^-23. A) 5.7 × 10^-15 B) 3.6 × 10^-23 C) 1.3 × 10^-13 D) 1.5 × 10^-8 E) 8.3 × 10^-18

3.6 × 10^-23

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10^-8. At equilibrium, the molarity of H3O+ in a 0.044 M solution of HClO is A) 3.6 × 10^-5 B) 0.044 C) 2.8 × 10^-10 D) 4.44 E) 1.36

3.6 × 10^-5

What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10^-4. A) 14.23 B) 10.38 C) 5.39 D) 3.62 E) 4.08

3.62

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10^-4. A) 3.22 B) 3.82 C) 3.69 D) 3.09 E) 4.46

3.69

Calculate the pH of a buffer that is 0.040 M HF and 0.080 M NaF. The Ka for HF is 3.5 × 10^-4. A) 2.06 B) 4.86 C) 3.16 D) 3.46 E) 3.76

3.76

Calculate the Ksp for zinc hydroxide if the solubility of Zn (OH)2 in pure water is 2.1 × 10^-4 g/L. A) 9.9 × 10^-18 B) 3.8 × 10^-17 C) 1.5 × 10^-3 D) 2.9 × 10^-3

3.8 × 10^-17

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10^-4. A) 3.46 B) 4.06 C) 2.85 D) 3.63 E) 4.24

4.06

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C. Ksp for TlCl is 1.7 × 10^-4. A) 6.8 × 10^-5 M B) 4.2 × 10^-4 M C) 8.2 × 10^-3 M D) 1.3 × 10^-2 M

4.2 × 10^-4 M

What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10^-5 for CH3CO2H. A) 9.80 B) 8.71 C) 5.29 D) 4.20

4.20

A buffer solution is 0.100 M in both HC7H5O2 and NaC7H5O2 and has a pH of 4.19. Which of the following pH values would you expect from the addition of a small amount of a dilute solution of a strong base? A) 3.89 B) 3.69 C) 5.69 D) 4.49 E) There is not enough information to determine.

4.49

A weak acid is titrated with a strong base to the equivalence point. The pH of the resulting solution is found to be 9.18. The pKa of the acid is A) 9.18. B) 7.00. C) 4.59. D) 2.50. E) 6.28

4.59.

Determine the Ka of an acid that has a pH of 3.29 and a concentration of 0.55 M. A) 4.8× 10^-7 B) 9.5 × 10^-6 C) 8.6 × 10^-11 D) 2.5 × 10^-3 E) 3.6 × 10^-8

4.8× 10^-7

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M formic acid to the equivalence point? The Ka of formic acid is 1.8 × 10^-4. A) 3.82 mL B) 50.0 mL C) 41.6 mL D) 60.1 mL E) 3.57 mL

41.6 mL

The molar solubility of CuI is 2.26 × 10^-6 M in pure water. Calculate the Ksp for CuI. A) 5.11 × 10^-12 B) 4.52 × 10^-6 C) 1.50 × 10^-3 D) 4.62 × 10^-17 E) 1.02 × 10^-11

5.11 × 10^-12

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 100.0 mL of HNO3. The Kb of NH3 is 1.8 × 10^-5. A) 6.58 B) 10.56 C) 8.72 D) 3.44 E) 5.28

5.28

Calculate the pH of a 0.800 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 3.7 × 10^-4. A) 1.76 B) 5.33 C) 8.67 D) 12.23

5.33

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.25? A) 1.78 × 10^-11 M B) 5.62 × 10^-4 M C) 3.25 M D) 10.75 M

5.62 × 10^-4 M

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.24. A) 5.8 × 10^-4 B) 10.76 C) 1.7 × 10^-11 D) 3.2 × 10^-14 E) 1.1 × 10^-13

5.8 × 10^-4

The molar solubility of Ba3(PO4)2 is 8.89 × 10^-9 M in pure water. Calculate the Ksp for Ba3(PO4)2. A) 4.94 × 10^-49 B) 5.55 × 10^-41 C) 5.33 × 10^-37 D) 8.16 × 10^-31 E) 6.00 × 10^-39

6.00 × 10^-39

Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C. A) 4.15 B) 5.15 C) 6.15 D) 7.15 E) 8.15

6.15

Determine the molar solubility for Pb3(PO4)2 in pure water. Ksp for Pb3(PO4)2 is 1.0 × 10^54. A) 4.1 × 10^-28 M B) 5.8 × 10^-10 M C) 1.1 × 10^-11 M D) 6.2 × 10^-12 M E) 1.0 × 10^-54 M

6.2 × 10^-12 M

The pH of an aqueous solution at 25.0°C is 10.20. What is the molarity of H+ in this solution? A) 6.3 × 10^-11 B) 1.6 × 10^-4 C) 3.3 D) 1.0 × 10^-13 E) 1.6 × 10^10

6.3 × 10^-11

Calculate the pH of a buffer that is 1.58 M HClO and 0.099 M NaClO. The Ka for HClO is 2.9 × 10^-8. A) 7.54 B) 6.87 C) 7.74 D) 6.16 E) 6.33

6.33

Calculate the pOH of a solution that contains 2.4 × 10^-8 M H3O⁺ at 25°C. A) 2.40 B) 6.38 C) 7.62 D) 5.38 E) 8.62

6.38

Calculate the pH of a solution formed by mixing 525 mL of 0.50 M H2CO3 with 355 mL of 0.87 M NaHCO3. The Ka for H2CO3 is 4.3× 10^-7. A) 4.63 B) 10.31 C) 6.44 D) 6.30 E) 4.18

6.44

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of A) 6.67 × 10^-10 M, 4.82 B) 6.67 × 10^-10 M, 9.18 C) 6.67 × 10^-11 M, 3.82 D) 6.67 × 10^-11 M, 10.18

6.67 × 10^-11 M, 3.82

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10^-14? A) 6.767 B) 0.465 C) 7.000 D) 7.233 E) 8.446

6.767

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 100.0 mL of 0.20 M KClO. The Ka for HClO is 2.9 × 10^-8. A) 5.99 B) 8.01 C) 7.54 D) 7.06 E) 6.46

7.06

Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C. A) 7.1 × 10^-5 M B) 4.2 × 10^-10 M C) 8.7 × 10^-10 M D) 6.5 × 10^-5 M E) 1.4 × 10^-10 M

7.1 × 10^-5 M

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A) 7.1 × 10^-5 M B) 4.2 × 10^-10 M C) 8.7 × 10^-10 M D) 6.5 × 10^-5 M E) 1.4 × 10^-10 M

7.1 × 10^-5 M

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with Ka = 3.5 x 10^-8? The equation for the dissociation of hypochlorous acid is: HOCl (aq) + H2O (l) <-> H3O^+ (aq) + OCl^- (aq) A) 1.9 × 10^-4 M B) 7.2 × 10^-4 M C) 2.8 × 10^-5 M D) 7.2 × 10^-5 M

7.2 × 10^-5 M

Calculate the pH of a solution that has a concentration of 0.190 M H2S and 0.550 M KHS? The Ka of H2S is 1.1 × 10^-7. A) 11.02 B) 7.49 C) 3.22 D) 7.42

7.42

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 300.0 mL of 0.20 M KClO. The Ka for HClO is 2.9 × 10^-8. A) 5.99 B) 8.01 C) 7.54 D) 7.06 E) 6.46

7.54

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO) and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10^-8. A) 13.88 B) 6.46 C) 8.49 D) 7.30 E) 7.54

7.54

Calculate the pH of a solution that contains 2.4 × 10^-8 M H3O⁺ at 25°C. A) 2.40 B) 6.38 C)7.62 D) 5.38 E) 8.62

7.62

You have 2.00 L of a buffer solution which is composed of 0.250 M HClO and 0.650 M KClO. Calculate the pH of the solution after the addition of 265 mL of 1.00 M HCl. The Ka for HClO is 3.0 × 10^-8. A) 7.65 B) 11.65 C) 7.89 D) 11.14 E) 4.66

7.65

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of nitrous acid is 4.6 × 10^-4. A) 10.35 mL B) 10.65 mL C) 3.35 mL D) 7.00 mL E) 8.11 mL

8.11 mL

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? Ka = 6.76 × 10^-4 for HF. A) 1.74 B) 5.75 C) 8.25 D) 12.26

8.25

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.1567 M NaOH? Ka =1.8 × 10^-4 for formic acid. A) 2.24 B) 5.66 C) 8.34 D) 11.76

8.34

What is the pH of a solution made by mixing 5.00 mL of 0.10 M acetic acid with 5.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10^-5 for CH3CO2H. A) 5.28 B) 7.00 C) 8.72 D) 10.02

8.72

Determine the [H3O⁺] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10^-8. A) 1.1 × 10^-10 M B) 7.7 × 10^-9 M C) 1.3 × 10^-6 M D) 4.9 × 10^-4 M E) 8.8 × 10^-5 M

8.8 × 10^-5 M

A 25.0-mL sample of 0.150 M hydrocyanic acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hydrocyanic acid is 4.9 × 10^-10. A) 9.04 B) 1.34 C) 5.32 D) 9.37 E) 9.25

9.37

Calculate the pH of a 1.60 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 × 10^-5. A) 2.27 B) 4.53 C) 9.47 D) 11.73

9.47

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10^-5. A) 8.25 B) 9.18 C) 9.50 D) 10.12 E) 10.83

9.50

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 35.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10^-5 for NH3. A) 8.93 B) 9.26 C) 9.58 D) 11.32

9.58

What is the pH of a 1.2 M pyridine solution that has Kb = 1.9 × 10^-9? The equation for the dissociation of pyridine is C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH-(aq). A) 4.32 B) 8.72 C) 9.68 D) 10.68

9.68

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3. Ksp (Al(OH)3) = 1.3 × 10^-33. A) 2.6 × 10^-9M B) 5.2 × 10^-31 M C) 9.87 × 10^-12 M D) 1.04 × 10^-29 M E) 6.5 × 10^-35 M

9.87 × 10^-12 M

Which of the following weak acids has the strongest conjugate base? A) acetic acid, Ka = 1.8 × 10^-5 B) nitrous acid, Ka = 4.5 × 10^-4 C) dihydrogen phosphate ion, Ka = 6.2 × 10^-8 D) hydrocyanic acid, Ka = 4.0 × 10^-10 E) benzoic acid, Ka = 6.3 × 10^-5

hydrocyanic acid, Ka = 4.0 × 10^-10

Determine the pOH of a 0.348 M Ca(OH)2 solution at 25°C. A) 13.08 B) 13.54 C) 13.84 D) 0.157 E) 0.458

0.157

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10^-5 for CH3CO2H. A) 0.50:1 B) 0.94:1 C) 1.1:1 D) 2.0:1

0.50:1

What is the Ksp of Cu(OH)2 if the molar solubility at 25°C is 3.42x10^-7 M? A) 3.3 × 10^-12 B) 4.2 × 10^-13 C) 1.6 × 10^-19 D) 1.3 × 10^-4

1.6 × 10^-19

Calculate the pOH of a solution that contains 3.9 × 10^-4 M H3O⁺ at 25°C. A) 4.41 B) 3.41 C) 10.59 D) 9.59 E) 0.59

10.59

The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10^-10. What is the pH of an aqueous solution of 0.040 M sodium cyanide (NaCN)? A) 10.96 B) 3.04 C) 9.0 × 10^-4 D) 1.1 × 10^-11 E) 2.0 × 10^-11

10.96

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine, CH3NH2, with 15.00 mL of 0.10 M methylammonium chloride, CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10^-4 for methylamine. A) 10.04 B) 10.57 C) 11.09 D) 11.78

11.09

What is the pH of the resulting solution if 35 mL of 0.432 M methylamine, CH3NH2, is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10^-11 for CH3NH3+. A) 2.91 B) 3.95 C) 10.05 D) 11.09

11.09

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8 × 10^-5. A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55

11.13

What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10^-5? The equation for the dissociation of NH3 is NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq). A) 1.87 B) 2.87 C) 11.13 D) 10.13

11.13

Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10^-5. A) 5.480 B) 2.740 C) 8.520 D)11.260 E) 12.656

11.260

A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH. Determine the pH of the solution after the addition of 75.0 mL of LiOH. A) 12.1 B) 2.65 C) 11.35 D) 1.89 E) 13.06

12.1

A 8.0 × 10^-3 M aqueous solution of at 25.0°C has a pH of A) 12.20 B) 1.80 C) 1.6 × 10^-2 D) 6.3 × 10^-13 E) 11.90

12.20

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The Ka of HF is 3.5 × 10^-4. A) 12.40 B) 9.33 C) 5.06 D) 8.94 E) 12.00

12.40

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 400.0 mL of KOH. The Ka of HF is 3.5 × 10^-4. A) 13.08 B) 12.60 C) 13.85 D) 12.30 E) 12.78

12.60

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 100.0 mL of LiOH. A) 13.13 B) 12.65 C) 1.35 D) 0.87 E) 12.95

12.65

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 100.0 mL HBr. A) 2.00 B) 12.00 C) 1.30 D) 12.70 E) 7.00

12.70

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive. A) 12.67 B) 12.78 C) 12.95 D) 13.25

12.78

What is the pH of a 0.040 M Ba(OH)2 solution? A) 1.10 B) 1.40 C) 12.60 D) 12.90

12.90

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution before the addition of any HBr. A) 12.86 B) 13.00 C) 13.30 D) 0.70 E) 1.00

13.30

Determine the pH of a 0.00598 M HClO4 solution. A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558

2.223

Identify the compound that is acid-insoluble. A) PbCl2 B) As2S3 C) FeS D) Ca3(PO4)2 E) LiCl

As2S3

The stomach excretes ________ to kill microorganisms and to activate enzymes that break down food. A) CH3COOH B) HBr C) LiHCO3 D) HCl E) HNO3

HCl

Which of the following acids (listed with pKa values) and their conjugate base would form a buffer with a pH of 8.10? A) HC7H5O2, pKa = 4.19 B) H2SO3, pKa = 1.77 C) HClO, pKa = 7.54 D) HCN, pKa = 9.31 E) HNO2, pKa = 3.34

HClO, pKa = 7.54

Which of the following acids is the strongest? The acid is followed by its Ka value. A) HF, 3.5 × 10^-4 B) HBrO, 2.9 × 10^-9 C) HNO2, 4.6 × 10^-4 D) H COOH, 1.8 × 10^-4 E) HClO2, 1.1 × 10^-2

HClO2, 1.1 × 10^-2

Which of the following acids (listed with Ka values) and their conjugate base would form a buffer with a pH of 2.34? A) C6H5COOH, Ka = 6.5 × 10^-5 B) HN3, Ka = 2.5 × 10^-5 C) HClO, Ka = 2.9 × 10^-8 D) HF, Ka = 3.5 × 10^-4 E) HClO2, Ka = 1.1 × 10^-2

HClO2, Ka = 1.1 × 10^-2

Identify the weakest acid. A) HF B) HCl C) HBr D) HI E) Not enough information is available

HF

Which of the following is a strong acid? A) C6H5CO2H B) HF C) HI D) NH4+ E) H2O

HI

Which of the following acids is the weakest? The acid is followed by its Ka value. A) HF, 3.5 × 10^-4 B) HIO, 2.3 × 10^-11 C) HNO2, 4.6 × 10^-4 D) H5COOH, 6.5 × 10^-5 E) HClO2, 1.1 × 10^-2

HIO, 2.3 × 10^-11

Which of the following species is amphoteric? A) HPO4- B) H3O+ C) PO43- D) Cl- E) None of the above are amphoteric.

HPO4-

Which of the following species is amphoteric? A) CO32- B) HF C) NH4⁺ D) HPO42- E) None of the above are amphoteric

HPO42-

A ligand is a molecule or ion that acts as a A) Lewis acid B) Brønsted-Lowry acid C) Arrhenius base D) Lewis base E) conjugate base

Lewis base

Which of the following is a Brønsted-Lowry acid? A) NH4+ B) CI4 C) NH2- D) BF3 E) I2

NH4+

Which of the following solutions is a good buffer system? A) a solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2 B) a solution that is 0.10 M HBr and 0.10 M LiC2H3O2 C) a solution that is 0.10 M HI and 0.10 M NH4+ D) a solution that is 0.10 M LiOH and 0.10 M KOH E) None of the above are buffer systems

a solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2

Which of the following solutions is a good buffer system? A) a solution that is 0.10 M NaCl and 0.10 M HCl B) a solution that is 0.10 M HCN and 0.10 M LiCN C) a solution that is 0.10 M NaOH and 0.10 M HNO3 D) a solution that is 0.10 M HNO3 and 0.10 M NaNO3 E) a solution that is 0.10 M HCN and 0.10 M K Br

a solution that is 0.10 M HCN and 0.10 M LiCN

Formic acid (HCO2H, Ka = 1.8 × 10^-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point? A) 0.0134 M B) 0.0476 M C) 0.0567 M D) 0.0676 M

0.0676 M

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution before the addition of any LiOH. A) 1.74 B) 1.05 C) 0.74 D) 0.57 E) 1.57

0.74

Determine the Ka of an acid that has a pH of 4.67 and a concentration of 0.448 M. A) 5.8 × 10^-8 B) 3.3 × 10^-11 C) 9.9 × 10^-5 D) 4.6 × 10^-7 E) 1.0 × 10^-9

1.0 × 10^-9

What is the pH of a solution made by mixing 40.00 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive. A) 0.64 B) 1.64 C) 12.36 D) 13.36 E) 10.00

1.64

Calculate the pH of a buffer that is 0.080 M HF and 0.040 M NaF. The Ka for HF is 3.5 × 10^-4. A) 2.06 B) 4.86 C) 3.16 D) 3.56 E) 3.76

3.16

Calculate the pH of a solution that is 0.111 M in sodium formate (NaHCO2) and in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10^-4. A) 3.387 B) 4.103 C) 14.36 D) 10.61 E) 5.296

3.387

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2. The Ka for HCHO2 is 1.8 × 10^-4. A) 3.87 B) 3.74 C) 10.53 D) 3.47 E) 10.13

3.47

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10^-4. A) 3.34 B) 3.46 C) 3.57 D) 3.63 E) 2.89

3.57

What is the hydronium ion concentration of an acid solution that has a pH of 5.5? A) 2.8 × 10^-9 M B) 3.6 × 10^-6 M C) 1.5 x10^-11 M D) 3.6 x10^-3 M

3.6 × 10^-6 M

Calculate the pH for an aqueous solution of pyridine that contains 2.15 x 10^-4 hydroxide ion. A) 4.65 × 10^-11 B) 2.15 × 10^-4 C) 3.67 D) 10.33

3.67

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HC7H5O2 is 6.5 × 10^-5. A) 4.19 B) 5.03 C) 4.41 D) 3.34 E) 3.97

3.97

How many milliliters of 0.175 M of Ba(OH)2 are required to titrate 78.5 mL of 0.0750M H I to the equivalence point? A) 33.6 mL B) 67.3 mL C) 135 mL D) 78.5 mL

33.6 mL

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-4 M in hydroxide ion. A) 4.00 × 10^-9 M B) 4.00 × 10^-10 M C) 4.00 × 10^-11 M D) 5.00 × 10^-11 M

4.00 × 10^-11 M

Determine the molar solubility of Pb(IO3)2 in pure water. Ksp for Pb(IO3)2 = 2.60 × 10^-13. A) 4.02 × 10-5 M B) 9.35 × 10-6 M C) 5.08 × 10-7 M D) 6.48 × 10-5 M E) 2.23 × 10-6 M

4.02 × 10-5 M

Calculate the pH of a 0.020 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10^-7 and Ka2 = 5.6 × 10^-11. A) 1.70 B) 4.03 C) 6.37 D) 10.25

4.03

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.20 M HCl? Ka = 3.0 × 10^-8 for HOCl. A) 0.70 B) 3.39 C) 3.76 D) 4.23

4.23

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10^-5 for CH3CO2H. A) 2.87 B) 4.35 C) 4.75 D) 5.14

4.35

Calculate the pH of a solution that contains 3.9 × 10^-5 M H3O⁺ at 25°C. A) 5.41 B) 4.41 C) 9.59 D) 8.59 E) 0.59

4.41

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 x 10^-2 M A) 4.44 × 10^-12 M and 2.65 B) 4.44 × 10^-12 M and 11.35 C) 4.44 × 10^-13 M and 1.65 D) 4.44 × 10^-13 M and 12.35

4.44 × 10^-13 M and 12.35

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2. The Ka for HC7H5O2 is 6.5 × 10^-5. A) 4.19 B) 9.69 C) 4.49 D) 4.31 E) 10.51

4.49

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10^-13. A) 8.8 × 10^-7 M B) 3.9 × 10^-13 M C) 5.8 × 10^-5 M D) 5.1 × 10^-12 M E) 0.150 M

5.1 × 10^-12 M

Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4. A) 7.61 × 10^-5 B) 0.0450 C) 5.16 D) 0.743 E) 3.76

5.16

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 200.0 mL HBr. A) 2.62 B) 2.00 C) 1.48 D) 12.52 E) 7.00

7.00

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point). A) 0.97 B) 13.03 C) 2.76 D) 11.24 E) 7.00

7.00

Identify the pH of normal blood. A) 6.9 B) 7.1 C) 7.4 D) 7.6 E) 7.9

7.4

The molar solubility of Ag2S is 1.26 × 10^-16 M in pure water. Calculate the Ksp for Ag2S. A) 1.59 × 10^-32 B) 1.12 × 10^-8 C) 6.81 × 10^-63 D) 3.78 × 10^-12 E) 8.00 × 10^-48

8.00 × 10^-48

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO. The Ka for HClO is 2.9 × 10^-8. A) 5.99 B) 8.01 C) 7.54 D) 7.06 E) 6.46

8.01

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10^-4. A) 9.62 B) 7.00 C) 3.46 D) 10.54 E) 8.14

8.14

Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3. The Ksp for Ag2CrO4 is 2.0 × 10^-12. A) 8.5 × 10^-11 M B) 4.2 × 10^-5 M C) 1.9 × 10^-2 M D) 7.2 × 10^-5 M E) 1.3 × 10^-11 M

8.5 × 10^-11 M

Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. A) 1.2 × 10^-5 B) 8.5 × 10^-6 C) 2.7 D) 4.9 × 10^-7 E) 5.4 × 10^-3

8.5 × 10^-6

Calculate the pH of a buffer that is 0.200 M H3BO3 and 0.122 M KH2BO3. The Ka for H3BO3 is 5.8 × 10^-10. A) 8.93 B) 9.02 C) 10.77 D) 9.46 E) 3.52

9.02

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3. The Kb for NH3 is 1.8 × 10^-5. A) 9.06 B) 9.45 C) 4.55 D) 4.74 E) 9.26

9.06

Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 × 10^-17. A) 9.22 × 10^-9 M B) 4.26 × 10^-17 M C) 8.51 × 10^-17 M D) 2.77 × 10^-6 M E) 4.40 × 10^-6 M

9.22 × 10^-9 M

Determine the pH of a 0.580 M KCH3CO2 solution at 25°C. The Ka of CH3CO2H is 1.80 × 10^-5. A) 9.25 B) 4.75 C) 7.00 D) 12.5 E) 1.47

9.25

Which of the following is TRUE? A) An effective buffer has a [base]/[acid] ratio in the range of 10 - 100. B) A buffer is most resistant to pH change when [acid] = [conjugate base] C) An effective buffer has very small absolute concentrations of acid and conjugate base. D) A buffer can not be destroyed by adding too much strong base. It can only be destroyed by adding too much strong acid. E) None of the above are true.

A buffer is most resistant to pH change when [acid] = [conjugate base]

Which one of the following statements is TRUE? A) A buffer is an aqueous solution composed of two strong bases. B) A buffer can absorb an unlimited amount of base. C) A buffer resists pH change by neutralizing added acids and bases. D) A buffer does not change pH when strong base is added. E) All of the above are true.

A buffer resists pH change by neutralizing added acids and bases.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl. A) Ba3(PO4)2 B) CuS C) AgCl D) NH4Cl E) NiS

AgCl

Gives what happens at low pH for aluminum hydroxide. A) Al(H2O)6^3+ dissolves B) Al(H2O)2(OH)4^- precipitates C) Al(OH)6 dissolves D) Al precipitates E) Al dissolves

Al(H2O)6^3+ dissolves

Gives what happens at neutral pH for aluminum hydroxide. A) Al(H2O)5^3+ precipitates B) Al(H2O)4(OH)2^- dissolves C) Al(OH)3 precipitates D) Al precipitates E) Al dissolves

Al(OH)3 precipitates

Which one of the following salts, when dissolved in water, produces the solution with the lowest pH? A) NaI B) KI C) MgI2 D) AlI3

AlI3

Which one of the following salts, when dissolved in water, produces the solution with the highest pH? A) KHSO4 B) RbClO4 C) BaO D) CH3CH3NH3Br

BaO

Define buffer capacity. A) Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness. B) Buffer capacity is the amount of acid that can be added until all of the base is used up. C) Buffer capacity is the amount of base that can be added until all of the acid is used up. D) Buffer capacity is the amount of acid that can be added until all of the acid is used up. E) Buffer capacity is the amount of base that can be added until all of the base is used up.

Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; and OH- to a pH of 8. A) Ba3(PO4)2 B) CdS C) AgCl D) NH4Cl E) FeS

FeS

Identify the acid that is in car batteries. A) H2SO4 B) HNO3 C) H2CO3 D) CH3COOH E) HCl

H2SO4

Which of the following compounds will have the highest molar solubility in pure water? A) PbSO4, Ksp = 1.82 × 10^-8 B) MgCO3, Ksp = 6.82 × 10^-6 C) AgCl, Ksp = 1.77 × 10^-10 D) PbS, Ksp = 9.04 × 10^-29 E) HgS, Ksp = 1.60 × 10^-54

MgCO3, Ksp = 6.82 × 10^-6

Which of the following is a weak base? A) NH(CH3)2 B) N2 C) NaOH D) CH2CH2 E) None of the above are weak bases.

NH(CH3)2

Which of the following is a Brønsted-Lowry base? A) CH4 B) HCN C) NH3 D) I2 E) None of the above are Brønsted-Lowry bases

NH3

All of the following cations are considered acidic EXCEPT A) Fe2+ B) Na+ C) Al3+ D) NH4+ E) V2+

Na+

Which one of the following salts, when dissolved in water, produces the solution with the highest pH? A) NaI B) NaBr C) NaCl D) NaF

NaF

Identify the base that is in Drano. A) LiOH B) NaOH C) NaHCO3 D) Li2CO3 E) NH3

NaOH

Identify the compound that is base-insoluble. A) PbCl2 B) Sb2S3 C) NiS D) Ca3(PO4)2 E) KCl

NiS

Give the equation for an unsaturated solution in comparing Q with Ksp. A) Q > Ksp B) Q < Ksp C) Q = Ksp D) Q ≠ Ksp E) none of the above

Q < Ksp

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10^-10. A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B) Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl. C) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution. D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. E) There is not enough information to say anything about this solution.

Silver chloride will precipitate out of solution, leaving a saturated AgCl solution.

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89, which of the following is TRUE? A) [HCHO2] < [NaCHO2] B) [HCHO2] = [NaCHO2] C) [HCHO2] > [NaCHO2] D) [HCHO2] >> [NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2

[HCHO2] < [NaCHO2]

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.74, which of the following is TRUE? A) [HCHO2] > [NaCHO2] B) [HCHO2] = [NaCHO2] C) [HCHO2] < [NaCHO2] D) [HCHO2] < <[NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

[HCHO2] = [NaCHO2]

Identify the indicator that has two endpoints. A) phenol red B) alizarin C) m-nitrophenol D) phenolphthalein E) alizarin yellow R

alizarin

Identify the indicator that can be used at the highest pH. A) alizarin B) thymol blue C) methyl red D) thymolphthalein E) alizarin yellow R

alizarin yellow R

Give the characteristics of a strong acid. A) ionizes completely in aqueous solutions B) has equilibrium far to the right C) has a polar bond D) has a weaker bond to hydrogen E) all of the above

all of the above

If an equal number of moles of the weak acid HF and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral? A) acidic B) basic C) neutral D) There is insufficient information provided to answer this question.

basic

Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves. A) hydrochloric acid B) sodium hydroxide C) sodium chloride D) calcium carbonate E) sodium bicarbonate

calcium carbonate

A Lewis base A) donates electrons. B) accepts electrons. C) donates a proton. D) accepts a proton. E) donates more than one proton.

donates electrons.

Identify the food that is not acidic. A) soft drink B) apple C) egg white D) soda E) wine

egg white

A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution. The Ka of nitrous acid is 4.5 × 10^-4. A) H2O B) H3O+ C) nitrite D) nitrous acid E) This is a buffer solution: the pH does not change upon addition of acid or base.

nitrous acid

Identify the most common indicator. A) alizarin B) bromophenol blue C) phenol red D) phenolphthalein E) thymolphthalein

phenolphthalein

Calculate the percent ionization of nitrous acid in a solution that is 0.205 M in nitrous acid and 0.295 M in potassium nitrite (HNO2 ). The acid dissociation constant of nitrous acid is 4.50 z 10^-4 A) 59.0 B) 0.151 C) 17.1 D) 2.72 × 10^-3 E) 3.508

0.151

Determine the molar solubility of AgBr in a solution containing 0.200 M NaBr. Ksp (AgBr) = 7.7 × 10^-13. A) 8.8 × 10^-7 M B) 1.54 × 10^-13 M C) 5.8 × 10^-5 M D) 3.8 × 10^-12 M E) 0.200 M

0.200 M

Determine the [OH⁻] concentration in a 0.235 M LiOH solution. A) 4.25 × 10^-14 M B) 0.470 M C) 2.13 × 10^-14 M D) 0.118 M E) 0.235 M

0.235 M

You wish to prepare an HC2H3O2 buffer with a pH of 4.14. If the pKa of is 4.74, what ratio of C2H3O2⁻/HC2H3O2 must you use? A) 0.10 B) 0.60 C) 0.25 D) 3.98 E) 4.0

0.25

Determine the [OH-] concentration of a 0.153 M Ba(OH)2 solution at 25°C. A) 3.27 × 10^-14 M B) 0.153 M C) 0.306 M D) 6.53 × 10^-14 M E) 0.0765 M

0.306 M

Determine the pOH of a 0.141 M RbOH solution at 25°C. A) 0.851 B) 13.15 C) 0.141 D) 13.86 E) 0.28

0.851

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10^-5. A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60

4.60

A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of sodium butanoate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The Ka of butanoic acid is 1.36 × 10^-3. A) H2O B) H3O+ C) butanoate ion D) butanoic acid E) This is a buffer solution: the pH does not change upon addition of acid or base.

butanoate ion

When titrating a strong monoprotic acid with KOH at 25°C, the A) pH will be less than 7 at the equivalence point. B) pH will be greater than 7 at the equivalence point. C) titration will require more moles of base than acid to reach the equivalence point. D) pH will be equal to 7 at the equivalence point. E) titration will require more moles of acid than base to reach the equivalence point.

pH will be equal to 7 at the equivalence point.

When titrating a weak monoprotic acid with NaOH at 25°C, the A) pH will be less than 7 at the equivalence point. B) pH will be equal to 7 at the equivalence point. C) pH will be greater than 7 at the equivalence point. D) titration will require more moles of base than acid to reach the equivalence point. E) titration will require more moles of acid than base to reach the equivalence point.

pH will be greater than 7 at the equivalence point.

When titrating a monoprotic strong acid with a weak base at 25°C, the A) pH will be 7 at the equivalence point. B) pH will be greater than 7 at the equivalence point. C) titration will require more moles of the base than acid to reach the equivalence point. D) titration will require more moles of acid than base to reach the equivalence point. E) pH will be less than 7 at the equivalence point.

pH will be less than 7 at the equivalence point.

Identify a good buffer. A) small amounts of both a weak acid and its conjugate base B) significant amounts of both a strong acid and a strong base C) small amounts of both a strong acid and a strong base D) significant amounts of both a weak acid and a strong acid E) significant amounts of both a weak acid and its conjugate base

significant amounts of both a weak acid and its conjugate base

Describe the solubility of Al(OH)3 with respect to pH. A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH B) soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH C) insoluble at low pH,insoluble in pH-neutral solution, and soluble at high pH D) soluble at low pH, in pH-neutral solution, and at high pH E) pH has no effect on the solubility.

soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH

A solution of NaF is added dropwise to a solution that is 0.0158 M in Ba2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10^-6. A) 5.4 × 10^-5 B) 1.0 × 10^-2 C) 2.7 × 10^-8 D) 2.6 × 10^-3 E) 1.1 × 10^-4

1.0 × 10^-2

An aqueous solution at 25.0°C contains [H+] = 0.090 M. What is the pH of the solution? A) 1.05 B) -1.05 C) 13.0 D) 0.0900 E) 1.10 × 10^-13

1.05

Calculate the concentration of bicarbonate ion, HCO3-, in a 0.030 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10^-7 and Ka2 = 5.6 × 10^-11. A) 1.1 × 10^-4 M B) 4.3 × 10^-7 M C) 1.3 × 10^-8 M D) 5.6 × 10^-11 M

1.1 × 10^-4 M

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20? A) 6.31 × 10^-10 M B) 1.58 × 10^-5 M C) 4.80 M D) 9.20 M

1.58 × 10^-5 M

What is the pH of a 0.020 M HClO4 solution? A) 0.020 B) 0.040 C) 1.70 D) 12.30

1.70

Determine the pOH of a 0.00598 M HClO4 solution. A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558

11.777

Calculate the solubility (in g/L) of silver chromate in water at 25°C if the Ksp for Ag2CrO4 is 1.1 × 10^-12. A) 3.5 × 10^-4 g/L B) 2.2 × 10^-2 g/L C) 2.7 × 10^-2 g/L D) 3.4 × 10^-2 g/L

2.2 × 10^-2 g/L

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of to the equivalence point? A) 29.5 mL B) 0.332 mL C) 4.57 mL D) 0.208 mL E) 21.2 mL

29.5 mL

Calculate the pH of a buffer that is 0.115 M HC2H3O2 and 0.160 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10^-5. A) 4.89 B) 8.81 C) 4.74 D) 5.15 E) 4.60

4.89

Calculate the pH of a solution that contains 7.8 × 10^-6 M OH⁻ at 25°C. A) 1.28 B) 5.11 C) 12.72 D) 8.89 E) 9.64

8.89

Determine the pH of a 0.22 M NaF solution at 25°C. The Ka of HF is 3.5 × 10^-5. A) 10.20 B) 5.10 C) 8.90 D) 11.44 E) 2.56

8.90

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3. The Kb for NH3 is 1.8 × 10^-5. A) 9.13 B) 9.25 C) 9.53 D) 4.74 E) 8.98

8.98

What volume of 5.00 × 10^-3 M HNO3 is needed to titrate 40.00 mL of 5.00 × 10^-3 M Ca(OH)2 to the equivalence point? A) 5.00 mL B) 20.0 mL C) 40.0 mL D) 80.0 mL

80.0 mL

If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25°C, the best choice would be an acid component with a Ka equal to A) 9.10 × 10^-2. B) 9.10 × 10^-4. C) 9.10 × 10^-6. D) 9.10 × 10^-8. E) 9.10 × 10^-10.

9.10 × 10^-4.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 50.0 mL of HNO3. The Kb of NH3 is 1.8 × 10^-5. A) 4.74 B) 7.78 C) 7.05 D) 9.26 E) 10.34

9.26

Determine the pH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 × 10^-9. A) 4.59 B) 9.41 C) 4.71 D) 10.14 E) 9.29

9.29

What is the pH of a 0.84 M solution of a base that has a Kb = 7.3 × 10^-10? A) 4.11 B) 7.29 C) 9.39 D) 10.98

9.39

Which of the following is TRUE? A) The equivalence point is where the amount of acid equals the amount of base during any acidbase titration. B) At the equivalence point, the pH is always 7. C) An indicator is not pH sensitive. D) A titration curve is a plot of pH vs. the [base]/[acid] ratio. E) None of the above are true.

The equivalence point is where the amount of acid equals the amount of base during any acidbase titration.

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE? A) [HCHO2] < [NaCHO2] B) [HCHO2] = [NaCHO2] C) [HCHO2] << [NaCHO2] D) [HCHO2] > [NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

[HCHO2] > [NaCHO2]

A Lewis acid A) donates electrons. B) accepts electrons. C) donates a proton. D) accepts a proton. E) donates more than one proton

accepts electrons.

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M NaC2H3O2. Which of the following actions will destroy the buffer? A) adding 0.050 moles of NaC2H3O2 B) adding 0.050 moles of HC2H3O2 C) adding 0.050 moles of HCl D) adding 0.050 moles of NaOH E) None of the above will destroy the buffer.

adding 0.050 moles of HCl

A 1.0 L buffer solution is 0.050 M HC2H3O2 and 0.250 M KC2H3O2. Which of the following actions will destroy the buffer? A) adding 0.050 moles of NaOH B) adding 0.050 moles of HCl C) adding 0.050 moles of HC2H3O2 D) adding 0.050 moles of KC2H3O2 E) All of the above will destroy the buffer.

adding 0.050 moles of NaOH

A solution with a hydroxide ion concentration of 4.15 × 10^-6 M is ________ and has a hydrogen ion concentration of ________. A) acidic, 2.41 × 10^-8 M B) acidic, 2.41 × 10^-9 M C) basic, 2.41 × 10^-8 M D) basic, 2.41 × 10^-9 M

basic, 2.41 × 10^-9 M

An important buffer in the blood is a mixture of A) sodium chloride and hydrochloric acid. B) hydrochloric acid and sodium hydroxide. C) carbonic acid and bicarbonate ion. D) acetic acid and bicarbonate ion. E) acetic acid and carbonate ion.

carbonic acid and bicarbonate ion.

Identify the indicator that can be used at the lowest pH. A) 2,4-dinitrophenol B) thymol blue C) crystal violet D) thymolphthalein E) methyl red

crystal violet

Animals will lick up ethylene glycol (antifreeze) due to its sweet taste. The antidote for ethylene glycol poisoning is the administration of A) ethyl alcohol ( alcoholic drinks). B) isopropyl alcohol (rubbing alcohol). C) mineral oil (laxative). D) vinegar. E) sodium bicarbonate (baking soda).

ethyl alcohol ( alcoholic drinks)

Determine the solubility for CuC2O4(s) in pure water. Ksp for is 2.9 × 10^-8. A) 0.0036 g L-1 B) 0.069 g L-1 C) 0.026 g L-1 D) 0.18 g L-1 E) 0.0083 g L-1

0.026 g L-1

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH3 (Kb = 1.8 × 10^-5) is NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq). A) 3.0 M B) 0.056 M C) 1.8 × 10^-2 M D) 1.0 × 10^-3 M

0.056 M

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C? A) 0.1 M HBr B) 0.1 M NaBr C) 0.1 M CaBr2 D) 0.1 M K NO3

0.1 M CaBr2

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point? A) 0.300 M B) 0.312 M C) 0.800 M D) 1.30 M

0.800 M

Calculate the pH of a 0.80 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 x 10^-8 A) 0.96 B) 0.99 C) 1.82 D) 1.92

0.96

What is the selenide ion concentration [Se2-] for a 0.300 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 x 10^-4 and Ka2 = 1.0x10^-11 A) 6.2 × 10^-3 M B) 1.3 × 10^-4 M C) 3.9 × 10^-5 M D) 1.0 × 10^-11 M

1.0 × 10^-11 M

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 30.0 mL of LiOH. A) 0.86 B) 1.21 C) 2.00 D) 1.12 E) 2.86

1.12

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10^-4 M in calcium ion and 2.33 × 10^-4 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10^-9. A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B) Nothing will happen Ksp > Q for all possible precipitants. C) A precipitate will form as calcium oxalate is not soluble to any extent. D) A precipitate will form since Q > Ksp for calcium oxalate. E) There is not enough information to determine.

A precipitate will form since Q > Ksp for calcium oxalate.

Which of the following compounds solubility will not be affected by a low pH in solution? A) AgCl B) Ca(OH)2 C) SrF2 D) CuS E) CaCO3

AgCl

Which of the following would be considered a complex ion? A) F^- B) PO3^3- C) AlF6- D) Fe^2+ E) NH4+

AlF6-

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. A) Ba3(PO4)2 B) PbS C) AgCl D) NH4Cl E) CoS

Ba3(PO4)2

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl, then H2S and 0.2 M HCl. A) Ba3(PO4)2 B) CuS C) AgCl D) NH4Cl E) CoS

CuS

Which of the following compounds will have the highest molar solubility in pure water? A) SnS, Ksp = 1.0 × 10^-26 B) CuS, Ksp = 1.27 × 10^-36 C) Fe(OH)3, Ksp = 2.79 × 10^-39 D) ZnS, Ksp = 2.0 × 10^-25 E) Ag2S, Ksp = 6.0 × 10^-51

Fe(OH)3, Ksp = 2.79 × 10^-39

Which of the following is a Lewis base? A) AlCl3 B) H2O C) SiCl4 D) C5H12 E) None of the above are Lewis bases.

H2O

Which of the following is a polyprotic acid? A) HBr B) H2SO4 C) HCN D) CH4 E) HC2H3O2

H2SO4

Which of the following is a triprotic acid? A) HCl B) H2SO4 C) H3PO4 D) CF4 E) HC2H3O2

H3PO4

Which of the following is a strong base? A) I- B) NH3 C) CH3OH D) NO3⁻ E) KOH

KOH

Which one of the following will form an acidic solution in water? A) NH4Cl B) KF C) KI D) KNO3 E) None of the above solutions will be acidic.

NH4Cl

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10^-9. A) A precipitate will form since Q > Ksp for calcium oxalate. B) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. C) Nothing will happen since calcium oxalate is extremely soluble. D) Nothing will happen since Ksp > Q for all possible precipitants. E) There is not enough information to determine.

Nothing will happen since Ksp > Q for all possible precipitants.

Give the equation for a saturated solution in comparing Q with Ksp. A) Q > Ksp B) Q < Ksp C) Q = Ksp D) Q ≠ Ksp E) none of the above

Q = Ksp

Give the equation for a supersaturated solution in comparing Q with Ksp. A) Q > Ksp B) Q < Ksp C) Q = Ksp D) Q ≠ Ksp E) none of the above

Q > Ksp

Which of the following bases is the strongest? The base is followed by its Kb. A) (CH3CH2)2NH, 8.6 × 10^-4 B) CH3NH2, 4.4 × 10^-4 C) C6H5NH2, 4.0 × 10^-10 D) NH3, 1.76 × 10^-5 E) C5H5N, 1.7 × 10^-9

(CH3CH2)2NH, 8.6 × 10^-4

Identify the acid that is in vinegar. A) H2SO4 B) HNO3 C) Li2CO3 D) CH3COOH E) HF

CH3COOH

________ is the active component in vinegar. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH

CH3COOH

Which of the following is an Arrhenius base? A) CH3CO2H B) KOH C) CH3OH D) Na F E) More than one of these compounds is an Arrhenius base.

KOH

In a triprotic acid, which Ka has the highest value? A) Ka1 B) Ka2 C) Ka3 D) Kb1 E) Kb2

Ka1

A solution with a hydrogen ion concentration of 3.25 × 10^-5 M is ________ and has a hydroxide ion concentration of ________. A) acidic, 3.08 × 10^-9 M B) acidic, 3.08 × 10^-10 M C) basic, 3.08 × 10^-9 M D) basic, 3.08 × 10^-10 M

acidic, 3.08 × 10^-10 M

Calculate the hydroxide ion concentration in an aqueous solution with a pOH of 9.85 at 25°C. A) 7.1 × 10^-5 M B) 4.2 × 10^-10 M C) 8.7 × 10^-10 M D) 6.5 × 10^-5 M E) 1.4 × 10^-10 M

1.4 × 10^-10 M

Which of the following bases is the weakest? The base is followed by its Kb value. A) HOCH2CH2NH2, 3.2 × 10^-5 B) NH3, 1.76 × 10^-5 C) C5H5N, 1.7 × 10^-9 D) (CH3CH2)3N, 5.2 × 10^-4 E) Since these are all weak bases, they have the same strength.

C5H5N, 1.7 × 10^-9

All of the following anions are considered basic EXCEPT A) F-. B) CN-. C) PO4^3-. D) HPO4^2-. E) Cl-.

Cl-.

Which of the following statements is TRUE? A) A strong acid is composed of a proton and an anion that have a very strong attraction for one another. B) A weak base is composed of a cation and an anion with a very weak attraction between them. C) A strong acid has a strong conjugate base. D) The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid. E) None of the above statements are true.

The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid.

The stronger the acid, then which of the following is TRUE? A) The stronger the conjugate acid. B) The stronger the conjugate base. C) The weaker the conjugate base. D) The weaker the conjugate acid. E) None of the above

The weaker the conjugate base.

Calculate the concentration of H3O⁺ in a solution that contains 6.25 × 10^-9 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. A) 6.38 × 10^-9 M, basic B) 1.60 × 10^-6 M, acidic C) 7.94 × 10^-11 M, acidic D) 7.38 × 10^-3 M, basic E) 4.92× 10^-5 M, acidic

1.60 × 10^-6 M, acidic

Determine the pH of a 0.023 M HNO3 solution. A) 12.36 B) 3.68 C) 1.64 D) 2.30 E) 2.49

1.64

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. A) 1.8 × 10^-10 M, basic B) 1.8 × 10^-10 M, acidic C) 5.5 × 10^-10 M, neutral D) 9.2 × 10^-1 M, acidic E) 9.2 × 10^-1 M, basic

1.8 × 10^-10 M, basic

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C. A) 5.7 × 10^-11 M B) 1.9× 10^-12 M C) 5.4 × 10^-2 M D) 6.4 × 10^-7 M E) 9.5× 10^-3 M

1.9× 10^-12 M

Determine the pH in a 0.235 M NaOH solution. A) 13.76 B) 0.24 C) 13.37 D) 0.63 E) 12

13.37

Determine the Kb for CN⁻ at 25°C. The Ka for HCN is 4.9 × 10^-10. A) 4.9 × 10^-14 B) 2.3 × 10^-9 C) 1.4 × 10^-5 D) 2.0 × 10^-5 E) 3.7 × 10^-7

2.0 × 10^-5

Calculate the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°C. A) 2.1 × 10^-10 M B) 9.7 × 10^-10 M C) 4.7 × 10^-5 M D) 3.8 × 10^-5 M E) 6.3 × 10^-6 M

2.1 × 10^-10 M

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C. A) 2.1 × 10^-10 M B) 9.7 × 10^-10 M C) 4.7 × 10^-5 M D) 3.8 × 10^-5 M E) 6.3 × 10^-6 M

2.1 × 10^-10 M

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10^5. A) 2.26 B) 4.52 C) 11.74 D) 9.48 E) 5.48

2.26

Determine the Ka for CH3NH3⁺ at 25°C. The Kb for CH3NH2 is 4.4 × 10^-4. A) 3.1 × 10^-10 B) 6.8 × 10^-11 C) 5.6 × 10^-10 D) 2.3 × 10^-3 E) 2.3 × 10^-11

2.3 × 10^-11

Calculate the concentration of OH⁻ in a solution that contains 3.9 × 10^-4 M H3O⁺ at 25°C. Identify the solution as acidic, basic, or neutral. A) 2.6 × 10^-11 M, acidic B) 2.6 × 10^-11 M, basic C) 3.9 × 10^-4 M, neutral D) 2.7 × 10^-2 M, basic E) 2.7 × 10^-2 M, acidic

2.6 × 10^-11 M, acidic

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 x 10^-3 hydronium ion. A) 4.65 × 10^-12 M B) 2.15 × 10^-3 M C) 2.67 D) 11.33

2.67

Determine the pOH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10^-5. A) 5.480 B) 2.740 C) 8.520 D) 11.260 E) 12.656

2.740

A container of orange juice at 25°C has a hydronium concentration of 1.78 × 10^-3M. What is the pH of the juice? A) 1.84 B) 3.31 C) 2.75 D) 11.25 E) 7.00

2.75

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-2 M in hydronium ion. A) 2.86 × 10^-5 M B) 2.86 × 10^-10 M C) 2.86 × 10^-13 M D) 3.50 × 10^-13 M

2.86 × 10^-13 M

Which one of the following will form a basic solution in water? A) NaC2H3O2 B) LiCN C) KClO2 D) LiBrO E) All of the above will form basic solutions.

All of the above will form basic solutions.

Which of the following is TRUE? A) A neutral solution contains [H2O] = [H3O⁺] B) A neutral solution does not contain any H3O+ or OH- C) An acidic solution has [H3O⁺] > [OH⁻] D) A basic solution does not contain H3O+ E) None of the above are true

An acidic solution has [H3O⁺] > [OH⁻]

Determine the [OH⁻] concentration in a 0.169 M Ca(OH)2 solution. A) 0.338 M B) 0.169 M C) 5.92 × 10^-14 M D) 2.96 × 10^-14 M E) 0.298 M

0.338 M

Determine the pOH in a 0.235 M NaOH solution. A) 13.76 B) 0.24 C) 13.37 D) 0.63 E) 12

0.63

Determine the [OH-] concentration of a 0.741 M KOH solution at 25°C. A) 1.34 × 10-13 M B) 1.34 × 10-14 M C) 0.741 M D) 7.41 M E) none of the above

0.741 M

What is the concentration of hydroxide ions in pure water at 30.0∘C, if Kw at this temperature is 1.47 × 10^-14? A) 1.00 × 10^-7 M B) 1.30 × 10^-7 M C) 1.47 × 10^-7 M D) 8.93 × 10^-8 M E) 1.21 × 10^-7 M

1.21 × 10^-7 M

Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 × 10^-4. A) 1.1 % B) 1.2 × 10-2 % C) 3.2 % D) 3.5 × 10-2 % E) 4.7 %

3.2 %

Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10^-7 and Ka2 = 5.6 × 10^-11. A) 11.00 B) 10.44 C) 5.50 D) 4.31 E) 3.56

3.56

Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C. A) 2.1 × 10^-10 M B) 9.7 × 10^-10 M C) 4.7 × 10^-5 M D) 3.8 × 10^-5 M E) 6.3 × 10^-6 M

4.7 × 10^-5 M

Determine the pOH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 × 10^-9. A) 4.59 B) 9.41 C) 4.71 D) 10.14 E) 9.29

4.71

Determine the pH of a 0.62 M NH4NO3 solution at 25°C. The Kb for NH3 is 1.76 × 10^-5. A) 2.48 B) 9.27 C) 11.52 D) 4.73 E) 9.45

4.73

Calculate the pOH of a solution that contains 7.8 × 10^-6 M OH⁻ at 25°C. A) 1.28 B) 5.11 C) 12.72 D) 8.89 E) 9.64

5.11

What is the Kw of pure water at 50.0°C, if the pH is 6.630? A) 2.34 × 10^-7 B) 5.50 × 10^-14 C) 2.13 × 10^-14 D) 1.00 × 10^-14 E) There is not enough information to calculate the Kw.

5.50 × 10^-14

Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10^-7 and Ka2 = 5.6 × 10^-11. A) 2.8 × 10^-4 M B) 3.2 × 10^-6 M C) 5.6 × 10^-11 M D) 4.3 × 10^-7 M E) 6.9 × 10^-8 M

5.6 × 10^-11 M

When dissolved in water, which compound is generally considered to be an Arrhenius acid? A) H NO2 B) KOH C) Li F D) CH3OH

H NO2

Identify the weak diprotic acid. A) CH3COOH B) HCOOH C) H3PO4 D) H2SO4 E) H2CO3

H2CO3

What is the conjugate acid of HCO3⁻ ? A) H3O+ B) H2O C) CO32- D) OH⁻ E) H2CO3

H2CO3

________ is found in carbonated beverages due to the reaction of carbon dioxide with water. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH

H2CO3

Which Brønsted-Lowry acid is not considered to be a strong acid in water? A) HI B) HBr C) H2S O3 D) H NO3

H2S O3

Identify the weak diprotic acid. A) HNO3 B) H3PO4 C) H2SO3 D) HClO4 E) H2SO4

H2SO3

Which of these is an example of a polyprotic oxyacid? A) HClO3 B) CH3COOH C) H2SO3 D) H2S E) None of the above

H2SO3

Identify the diprotic acid. A) HNO3 B) HBr C) CH3COOH D) H2SO4 E) HClO4

H2SO4

Which of the following is an Arrhenius acid? A) H2SO4 B) NaOH C) NH2CH3 D) CH3CH3 E) More than one of these is an Arrhenius acid.

H2SO4

Identify the strongest acid. A) H2O B) H2S C) H2Se D) H2Te E) Not enough information is available.

H2Te

Which of the following is not a conjugate acid-base pair? A) NH4+/NH3 B) H3O⁺/OH⁻ C) H2SO3/HSO3⁻ D) C2H3O2⁻/HC2H3O2 E) All of the above are conjugate acid-base pairs.

H3O⁺/OH⁻

Identify the triprotic acid. A) HNO3 B) H3PO4 C) H2CO3 D) HClO4 E) H2SO4

H3PO4

Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4 A) HBrO2 < HBrO4 < HBrO < HBrO3 B) HBrO < HBrO2 < HBrO3 < HBrO4 C) HBrO2 < HBrO3 < HBrO4 < HBrO D) HBrO4 < HBrO2 < HBrO3 < HBrO E) HBrO < HBrO4 < HBrO3 < HBrO2

HBrO < HBrO2 < HBrO3 < HBrO4

Which of the following acids will have the strongest conjugate base? A) HCl B) HClO4 C) HNO3 D) HCN E) HI

HCN

Which of the following is a weak acid? A) HClO4 B) H2SO4 C) HBr D) HCN E) HNO3

HCN

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A) HF, 3.5 × 10^-4 B) HCN, 4.9 × 10^-10 C) HNO2, 4.6 × 10^-4 D) HCHO2, 1.8 × 10^-4 E) HClO2, 1.1 × 10^-2

HCN, 4.9 × 10^-10

Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A) HF, 3.5 × 10^-4 B) HCN, 4.9 × 10^-10 C) HNO2, 4.6 × 10^-4 D) HCHO2, 1.8 × 10^-4 E) HClO2, 1.1 × 10^-2

HClO2, 1.1 × 10^-2

Identify the strongest acid. A) HIO4 B) HIO3 C) HIO2 D) HIO E) Not enough information is given.

HIO4

What is the conjugate base of H2PO4⁻ ? A) HPO42- B) PO43- C) H3PO4 D) H3O+ E) OH⁻

HPO42-

An aqueous solution of ammonia is found to be basic. This observation can be explained by the net ionic equation A) NO3-(aq) + H2O(l) → HNO3(aq) + OH-(aq). B) NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq). C) HNO3(aq) + H2O(l) → NO3-(aq) + H3O+(aq). D) NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq).

NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq).

Identify the base that is in baking soda. A) RbOH B) NaOH C) NaHCO3 D) K2CO3 E) NH3

NaHCO3