Chapter 17

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

A) 12.1

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

A) 12.40

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

A) 29.5 mL

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

A) 3.09

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.

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

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

A) Q > Ksp

Give the expression for the solubility product constant for Cr2(CO3)3. A) [Cr3+]2[CO32-]3 B) C) D) E) [3Cr3+]3[2CO32-]2

A) [Cr3+]2[CO32-]3

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

B) 1.0 × 10-2

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

B) 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

B) 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

B) 1.48

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 × 107. A) 1.3 × 10-5 M B) 1.6 × 10-2 M C) 1.7 × 10-2 M D) 5.5 × 10-2 M

B) 1.6 × 10-2 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

B) 1.7 × 10-5 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 × 1025, 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

B) 1.9 × 10-26 M

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

B) 11.47

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

B) 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

B) 12.65

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

B) 12.78

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.

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

Gives what happens at high pH for aluminum hydroxide. A) Al(H2O)43+ dissolves B) Al(H2O)2(OH)4- dissolves C) Al(OH)6 dissolves D) Al precipitates E) Al dissolves

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

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

B) As2S3

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

B) CuS

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

B) a solution that is 0.10 M HCN and 0.10 M LiCN

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

B) alizarin

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

C) NiS

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

C) 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.

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

Give the expression for the solubility product constant for PbCl2. A) [Pb2+][Cl-]2 / [PbCl2] B) [PbCl2] / [Pb2+][2Cl-]2 C) [Pb2+][Cl⁻]2 D) [Pb2+]2[Cl-] / [PbCl2] E) [Pb2+]2[ Cl⁻]

C) [Pb2+][Cl⁻]2

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.

C) adding 0.050 moles of HCl

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.

C) butanoate ion

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.

C) 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

C) crystal violet

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

C)10

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

D) 80.0 mL

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

D) 9.26

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

E) 8.14

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

A) 0.50:1

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

A) 1.60

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

A) 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

A) 1.83 × 10-2 M

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).

A) 3.0 × 10-10 M, CuI

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

A) 3.387

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

A) 3.487

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

A) 33.6 mL

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

A) 4.02 × 10-5 M

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 × 103

A) 4.19

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

A) 4.89

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

A) 5.11 × 10-12

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

A) 7.65

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

A) 8.5 × 10-11 M

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

A) 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

A) 9.22 × 10-9 M

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

A) AgCl

Gives what happens at low pH for aluminum hydroxide. A) Al(H2O)63+ dissolves B) Al(H2O)2(OH)4- precipitates C) Al(OH)6 dissolves D) Al precipitates E) Al dissolves

A) Al(H2O)63+ dissolves

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

A) Ba3(PO4)2

Which of the following is TRUE? A) The equivalence point is where the amount of acid equals the amount of base during any acid-base 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.

A) The equivalence point is where the amount of acid equals the amount of base during any acid-base titration.

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.

A) [HCHO2] < [NaCHO2]

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) a solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2

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.

A) adding 0.050 moles of NaOH

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).

A) ethyl alcohol ( alcoholic drinks).

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.

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

Calculate the percent ionization of nitrous acid in a solution that is 0.205 M in nitrous acid (HNO2) and 0.295 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50x10-4 A) 59.0 B) 0.151 C) 17.1 D) 2.72 × 10-3 E) 3.508

B) 0.151

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

B) 1.64

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

B) 1.7 × 10-4 M

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

B) 2.2 × 10-2 g/L

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

B) 2.93

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

B) 3.6 × 10-23

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.

B) 3.6 × 10-35 M, CuS

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

B) 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

B) 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

B) 4.2 × 10-4 M

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

B) 4.35

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

B) 5.6 × 10-9 M

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

B) 8.01

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

B) 9.02

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.

B) 9.10 × 10-4.

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.

B) CuS

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

B) MgCO3, Ksp = 6.82 × 10-6

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

B) Q < Ksp

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.

B) [HCHO2] = [NaCHO2]

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

C) 0.026 g L-1

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

C) 0.1 M CaBr2

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

C) 0.25

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

C) 0.74

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

C) 0.800 M

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 = 4.9x10-10 for HCN A) 2.0 × 10-10 M B) 4.9 × 10-10 M C) 1.2 × 10-9 M D) 7.0 × 10-6M

C) 1.2 × 10-9 M

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

C) 1.6 × 10-19

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

C) 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

C) 11.13

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

C) 12.52

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

C) 13.30

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

C) 2.08

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

C) 2.5 × 10-5 M

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

C) 3.16

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

C) 3.57

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

C) 3.69

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

C) 3.97 × 10-11

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

C) 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.

C) 4.59.

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

C) 41.6 mL

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

C) 5.16

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

C) 6.44

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

C) 7.4

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

C) 7.54

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

C) 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

C) 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

C) 8.72

A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF. If the Kf for AlF63- is 7 × 1019, 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

C) 9.1 × 10-19 M

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

C) 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

C) 9.58

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

C) 9.87 × 10-12 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

C) 9.95

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.

C) 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

C) AgCl

Gives what happens at neutral pH for aluminum hydroxide. A) Al(H2O)53+ precipitates B) Al(H2O)4(OH)2- dissolves C) Al(OH)3 precipitates D) Al precipitates E) Al dissolves

C) Al(OH)3 precipitates

Which of the following would be considered a complex ion? A) F- B) PO33- C) AlF6- D) Fe2+ E) NH4+

C) AlF6-

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

C) Fe(OH)3, Ksp = 2.79 × 10-39

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

C) HClO, pKa = 7.54

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.

C) pH will be greater than 7 at the equivalence point.

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

D) 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 after the addition of 30.0 mL of LiOH. A) 0.86 B) 1.21 C) 2.00 D) 1.12 E) 2.86

D) 1.12

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

D) 1.3 × 10-4

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

D) 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

D) 1.53 × 10-6 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

D) 1.96 × 10-6 M

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

D) 11.09

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

D) 12.52

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

D) 12.70

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

D) 2.1 × 10-4 M

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

D) 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

D) 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

D) 2.61 × 10-3 M

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

D) 3.0 × 10-2 M

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

D) 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

D) 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

D) 3.46

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

D) 3.47

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

D) 3.62

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

D) 3.8 × 10-12 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

D) 4.20

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

D) 4.23

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.

D) 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

D) 5.1 × 10-12 M

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

D) 6.2 × 10-12 M

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

D) 7.06

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

D) 7.42

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

D) 9.37

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.

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

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

D) Lewis base

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

D) 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.

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

Give the expression for the solubility product constant for BaF2. A) [BaF2] / [Ba2+][2F-]2 B) [Ba2+][F-]2 / [BaF2] C) [Ba2+]2[ F⁻] D) [Ba2+][F⁻]2 E) [Ba2+][ F⁻]

D) [Ba2+][F⁻]2

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.

D) [HCHO2] > [NaCHO2]

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

D) calcium carbonate

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.

D) nitrous acid

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.

D) pH will be equal to 7 at the equivalence point.

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

D) phenolphthalein

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

E) 1.6 × 10-4

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

E) 2.30 × 10-6 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

E) 3.0 × 10-4 M

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

E) 3.76

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

E) 3.97

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

E) 4.60

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

E) 5.28

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

E) 6.00 × 10-39

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

E) 6.33

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

E) 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

E) 7.00

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

E) 7.54

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

E) 8.00 × 10-48

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

E) 8.11 mL

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

E) 8.98

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

E) FeS

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

E) HClO2, Ka = 1.1 × 10-2

Give the expression for the solubility product constant for Ca3(PO4)2. A) [Ca2+]3[PO4^3-]2 / Ca3(PO4)2 B) Ca3(PO4)2 / [3Ca2+]3[2PO4^3-]2 C) [3Ca2+]2[2PO4^3-]3 / Ca3(PO4)2 D) [ Ca2+]2[ PO43-]3 E) [Ca2+]3[PO43-]2

E) [Ca2+]3[PO43-]2

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

E) alizarin yellow R

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

E) 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

E) significant amounts of both a weak acid and its conjugate base