Quiz 16: Aqueous Ionic Equilibrium

Fluffy,your prized Himalayan cat,was outside when your dad was changing the antifreeze in the car.Fluffy licked up a large amount of the antifreeze off the driveway.You live many miles from the veterinarian.What could you give Fluffy to drink to counteract the effects of antifreeze? A)mineral oil B)rubbing alcohol C)a strong alcoholic drink D)gasoline E)vegetable oil

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 HF and 0.10 M NaC₂H₃O₂ C)a solution that is 0.10 M HCl and 0.10 M NH₄⁺ D)a solution that is 0.10 M NaOH and 0.10 M KOH E)None of the above are buffer systems.

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 KNO₃ E)a solution that is 0.10 M HCN and 0.10 M NaCl

Which one of the following statements is true? A)A buffer is an aqueous solution composed of two weak acids. B)A buffer can absorb an unlimited amount of acid or base. C)A buffer resists pH change by neutralizing added acids and bases. D)A buffer does not change pH when strong acid or base is added. E)None of the above are true.

If the pK_a 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.

If the pK_a 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.

If the pK_a 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.

You wish to prepare an HC₂H₃O₂ buffer with a pH of 4.24.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use? A)0.10 B)0.50 C)0.32 D)2.0 E)2.8

You wish to prepare an HC₂H₃O₂ buffer with a pH of 5.44.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use? A)0.70 B)0.20 C)1.4 D)5.0 E)1.1

A buffer solution is 0.100 M in both HC₇H₅O₂ and LiC₇H₅O₂ and has a pH of 4.19.Which of the following pH values would you be most likely to see 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.

Calculate the pH of a buffer that is 0.058 M HF and 0.058 M LiF.The K_a for HF is 3.5 × 10^-4. A)2.86 B)9.31 C)10.54 D)3.46 E)4.69

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO.The K_a for HClO is 2.9 × 10^-8. A)7.54 B)6.67 C)3.77 D)6.46 E)7.33

Calculate the pH of a buffer that is 0.105 M HC₂H₃O₂ and 0.146 M KC₂H₃O₂.The K_a for HC₂H₃O₂ is 1.8 × 10^-5. A)4.89 B)9.11 C)4.74 D)9.26 E)4.60

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 K_b for NH₃ is 1.8 × 10^-5. A)9.13 B)9.25 C)9.53 D)4.74 E)8.98

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 K_b for NH₃ is 1.8 × 10^-5. A)9.06 B)9.45 C)4.55 D)4.74 E)9.26

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 K_a for HClO is 2.9 × 10^-8. A)5.99 B)8.01 C)7.54 D)7.71 E)6.46

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 K_a for HC₇H₅O₂ is 6.5 × 10^-5. A)4.19 B)9.69 C)4.49 D)4.31 E)10.51

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 K_a for HCHO₂ is 1.8 × 10^-4. A)3.87 B)3.74 C)10.53 D)3.47 E)10.13

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 K_a for HC₇H₅O₂ is 6.5 × 10^-5. A)4.19 B)5.03 C)4.41 D)3.34 E)3.97

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 K_a for HF is 3.5 × 10^-4. A)3.09 B)4.11 C)3.82 D)3.46 E)2.78

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 K_a for HF is 3.5 × 10^-4. A)3.46 B)4.06 C)2.85 D)3.63 E)4.24

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 K_a for HF is 3.5 × 10^-4. A)3.34 B)3.46 C)3.57 D)3.63 E)2.89

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 cannot 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.

The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid? A)2 B)5 C)10 D)20 E)15

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.

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10? A)HC₇H₅O₂,pK_a = 4.19 B)HF,pK_a = 3.46 C)HClO,pK_a = 7.54 D)HCN,pK_a = 9.31 E)HClO₂,pK_a = 1.96

Which of the following acids (listed with K_a values)and their conjugate base would form a buffer with a pH of 2.34? A)HC₇H₅O₂,K_a = 6.5 × 10^-5 B)HF,K_a = 3.5 × 10^-4 C)HClO,K_a = 2.9 × 10^-8 D)HCN,K_a = 4.9 × 10^-10 E)HClO₂,K_a = 1.1 × 10^-2

A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.050 M LiC₂H₃O₂.Which of the following actions will destroy the buffer? A)adding 0.050 moles of LiC₂H₃O₂ 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.

A 1.0 L buffer solution is 0.050 M HC₂H₃O₂ and 0.250 M LiC₂H₃O₂.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 LiC₂H₃O₂ E)None of the above will destroy the buffer.

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.

When titrating a strong monoprotic acid and 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.

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.

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.

Identify the most common indicator. A)Alizarin B)Thymol blue C)Crystal violet D)Phenolphthalein E)Alizarin yellow R

Identify the indicator that can be used at the lowest pH. A)Alizarin B)Thymol blue C)Crystal violet D)Phenolphthalein E)Alizarin yellow R

Identify the indicator that can be used at the highest pH. A)Alizarin B)Thymol blue C)Crystal violet D)Phenolphthalein E)Alizarin yellow R

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

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

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

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 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

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 K_a of HF is 3.5 × 10^-4. A)4.15 B)0.70 C)2.08 D)3.46 E)1.00

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 K_a of HF is 3.5 × 10^-4. A)2.08 B)3.15 C)4.33 D)3.46 E)4.15

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 K_b of NH₃ is 1.8 × 10^-5. A)4.74 B)9.26 C)11.13 D)13.00 E)12.55

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 K_b of NH₃ is 1.8 × 10^-5. A)4.74 B)7.78 C)7.05 D)9.26 E)10.34

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 K_b of NH₃ is 1.8 × 10^-5. A)1.70 B)6.44 C)7.56 D)12.30 E)2.30

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 K_b of NH₃ is 1.8 × 10^-5. A)6.44 B)1.48 C)2.00 D)12.52 E)12.00

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

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

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

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 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

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 K_a of HF is 3.5 × 10^-4. A)12.40 B)9.33 C)5.06 D)8.94 E)12.00

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 K_a of HF is 3.5 × 10^-4. A)13.08 B)12.60 C)13.85 D)12.30 E)12.78

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 K_b of NH₃ is 1.8 × 10^-5. A)6.58 B)10.56 C)8.72 D)3.44 E)5.28

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 K_a of HF is 3.5 × 10^-4. A)9.62 B)7.00 C)3.46 D)10.54 E)8.14

Which of the following compounds will have the highest molar solubility in pure water? A)PbSO₄, K_sp = 1.82 × 10^-8 B)MgCO₃, K_sp = 6.82 × 10^-6 C)AgI,K_sp = 8.51 × 10^-17 D)PbS,K_sp = 9.04 × 10^-29 E)FeS,K_sp = 3.72 × 10^-19

Which of the following compounds solubility will not be affected by a low pH in solution? A)AgCl B)Mg(OH)₂ C)CaF₂ D)CuS E)BaCO₃

Which of the following compounds will be more soluble in acidic solution than in pure water? A)PbCl₂ B)FeS C)Ca(ClO₄)₂ D)CuI E)None of the above will be more soluble in acidic solution.

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

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

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

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

Determine the molar solubility of PbSO₄ in pure water.K_sp (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

Determine the molar solubility of MgCO₃ in pure water.K_sp (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

Determine the molar solubility of AgI in pure water.K_sp (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

Which of the following compounds will have the highest molar solubility in pure water? A)PbS,K_sp = 9.04 × 10^-29 B)CuS,K_sp = 1.27 × 10^-36 C)Al(OH)₃,K_sp = 3 × 10^-34 D)ZnS,K_sp = 1.6 × 10^-24 E)Ag₂S,K_sp = 8 × 10^-48

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp 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

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp 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

Determine the molar solubility of CaSO₄ in a solution containing 0.100 M Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5. A)4.9 × 10^-3 M B)2.4 × 10^-4 M C)5.8 × 10^-10 M D)1.2 × 10^-5 M E)0.10 M

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.K_sp (CuCl)= 1.0 × 10^-6. A)1.0 × 10^-12 M B)5.0 × 10^-7 M C)2.0 × 10^-5 M D)1.0 × 10^-3 M E)0.050 M

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K_sp (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

Determine the molar solubility of Fe(OH)₂ in pure water.K_sp (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

Determine the molar solubility of Co₃(AsO₄)₂ in pure water.K_sp (Co₃(AsO₄)₂)= 6.80 × 10^-29. A)2.02 × 10^-5 B)2.32 × 10^-6 C)2.15 × 10^-8 D)9.26 × 10^-6 E)9.12 × 10^-7

Calculate the Ksp of Fe₂S₃ in pure water.The molar solubility is 1.05 × 10^-18. A)7.00 × 10^-88 B)1.28 × 10^-90 C)1.40 × 10^-88 D)6.30 × 10^-18 E)exceeds ability of calculator

Determine the molar solubility of BaF₂ in pure water.K_sp (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

The molar solubility of Ag₂S is 1.26 × 10^-16 M in pure water.Calculate the K_sp 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

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF.K_sp (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

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

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

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? K_sp (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.

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? K_sp (CaC₂O₄)= 2.3 × 10^-9. A)A precipitate will form since Q > K_sp 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 K_sp > Q for all possible precipitants. E)There is not enough information to determine.

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? K_sp (CaC₂O₄)= 2.3 × 10^-9. A)Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B)Nothing will happen K_sp > 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 > K_sp for calcium oxalate. E)There is not enough information to determine.

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? K_sp (CuCl)= 1.0 × 10^-6,K_sp (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 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? K_sp (CuS)= 1.3 × 10^-36, K_sp (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.

A ligand is a molecule or ion that acts as a ________. A)Lewis acid B)Br∅nsted-Lowry acid C)Br∅nsted-Lowry base D)Lewis base E)None of the above

A solution contains 2.2 × 10^-3 M in Cu²⁺ and 0.33 M in LiCN.If the K_f for Cu(CN)₄^2- 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

A solution contains 3.8 × 10^-2 M in Al³⁺ and 0.29 M in NaF.If the K_f for AlF₆^3- 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

Match the following. A)half-way to equivalence point of a weak acid/strong base titration B)equivalence point of a strong acid/strong base titration C)equivalence point of a weak base/strong acid titration D)equivalence point of a weak acid/strong base titration -pH = 7

Match the following. A)half-way to equivalence point of a weak acid/strong base titration B)equivalence point of a strong acid/strong base titration C)equivalence point of a weak base/strong acid titration D)equivalence point of a weak acid/strong base titration -pH = pK_a

Match the following. A)half-way to equivalence point of a weak acid/strong base titration B)equivalence point of a strong acid/strong base titration C)equivalence point of a weak base/strong acid titration D)equivalence point of a weak acid/strong base titration -pH > 7

Match the following. A)half-way to equivalence point of a weak acid/strong base titration B)equivalence point of a strong acid/strong base titration C)equivalence point of a weak base/strong acid titration D)equivalence point of a weak acid/strong base titration -pH < 7

Define a buffer.

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

Consider the K_sp values for two compounds: MZ,K_sp = 1.5 × 10^-20 and MZ₂,K_sp = 1.5 × 10^-20.Why don't these compounds have the same molar solubility?

Explain the common ion effect with respect to molar solubility.

Define a complex ion

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide 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 K_a of hydrazoic acid is 1.9 × 10^-5. A)H₂O B)H₃O⁺ C)azide D)hydrazoic acid E)This is a buffer solution: the pH does not change upon addition of acid or base.

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO₂)and 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

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂)and 0.278 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4. A)55.6 B)0.162 C)15.5 D)2.78 × 10^-3 E)3.448

Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10^-4. A)1.12 × 10^-4 B)0.0450 C)4.25 D)0.342 E)5.53

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4. A)14.28 B)10.43 C)5.48 D)3.57 E)4.13

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 K_a of hypochlorous acid is 3.8 × 10^-8. A)13.88 B)6.46 C)8.49 D)7.30 E)7.54

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO₂)and 0.205 M in formic acid (HCO₂H).The K_a of formic acid is 1.77 × 10^-4. A)3.910 B)3.587 C)13.84 D)10.10 E)4.963

A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate 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 K_a of benzoic acid is 1.36 × 10^-3. A)H₂O B)H₃O⁺ C)benzoate ion D)benzoic acid E)This is a buffer solution: the pH does not change upon addition of acid or base.

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.010 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H. A)2.87 B)3.74 C)4.75 D)5.74

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 5.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃. A)8.25 B)10.06 C)10.25 D)11.13

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine. A)10.17 B)10.57 C)10.97 D)11.78

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5 for NH₃. A)9.08 B)9.26 C)9.43 D)11.32

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 0.300 M NaOH? Assume that the volumes are additive. A)13.05 B)13.10 C)13.28 D)13.58

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 0.030 M NaCN? Assume that the volumes of the solutions are additive and that K_a = 4.9 × 10^-10 for HCN. A)1.5 × 10^-10 M B)4.9 × 10^-10 M C)1.6 × 10^-9 M D)7.0 × 10^-6 M

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5 for CH₃CO₂H. A)0.39:1 B)0.91:1 C)1.09:1 D)2.5:1

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 80.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point? A)10.0 mL B)40.0 mL C)80.0 mL D)160.mL

What is the pH of a solution made by mixing 25.00 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)0.64 B)1.64 C)12.36 D)13.36

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point? A)21.2 B)0.245 C)3.92 D)0.153 E)29.5

What is the pH of the resulting solution if 25.00 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.K_a = 1.8 × 10^-5 for CH₃CO₂H. A)9.43 B)9.08 C)4.92 D)4.57

What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5 for CH₃CO₂H. A)5.28 B)7.00 C)8.72 D)10.02

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5 for CH₃CO₂H. A)8.26 B)9.26 C)11.13 D)12.40

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 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl. A)0.30 B)3.18 C)3.76 D)4.03

What is the pH of the resulting solution if 45 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.K_a = 2.70 × 10^-11 for CH₃NH₃⁺. A)2.77 B)4.09 C)9.91 D)11.23

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The K_a of acetic acid is 4.50 × 10^-4. A)11.74 B)9.26 C)4.74 D)7.00 E)8.81

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5. A)2.83 B)1.5 × 10^-3 C)4.82 D)4.00 E)1.0 × 10⁴

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution.What is the pH after 26.0 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8. A)2.54 B)11.47 C)7.00 D)7.51 E)7.54

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5. A)4.90 B)50.0 C)41.6 D)60.1 E)4.65

A 25.0-mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution.What is the pH after 13.3 mL of base is added? The K_a of hydrazoic acid is 1.9 × 10^-5. A)4.45 B)1.34 C)3.03 D)4.78 E)4.66

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 0.3567 M NaOH? K_a = 1.8 × 10^-4 for formic acid. A)2.06 B)5.48 C)8.52 D)11.94

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? K_a = 6.76 × 10^-4 for HF. A)1.74 B)5.75 C)8.25 D)12.26

Formic acid (HCO₂H,K_a = 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

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

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the K_sp for CaF₂ is 1.5 × 10^-10. A)9.6 × 10^-4 g/L B)2.6 × 10^-2 g/L C)3.3 × 10^-2 g/L D)4.1 × 10^-2 g/L

Calculate the K_sp for silver sulfite if the solubility in pure water is 4.6 × 10^-3 g/L. A)3.8 × 10^-15 B)1.5 × 10^-14 C)2.4 × 10^-10 D)4.8 × 10^-10

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_sp 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

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.K_sp 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

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25°C. A)9.0 × 10^-11 B)3.6 × 10^-10 C)9.74 D)1.9 × 10^-5 E)1.3 × 10^-5

What is the molar solubility of barium fluoride (BaF₂)in water? The solubility-product constant for BaF₂ is 1.7 × 10^-6 at 25°C. A)6.5 × 10^-4 B)1.2 × 10^-2 C)1.8 × 10^-3 D)7.5 × 10^-3 E)5.7 × 10^-7

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

What is the molar solubility of AgCl in 0.30 M NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f 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

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is 1.0 × 10²¹. A)0.050 M B)0.10 M C)0.20 M D)0.40 M

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO₃ and 0.50 M Ba(NO₃)₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp 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)6.8 × 10^-2 M

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺.When the concentration of F^- exceeds ________ M,BaF₂ will precipitate.Neglect volume changes.For BaF₂,K_sp = 1.7 × 10^-6. A)5.9 × 10^-5 B)1.1 × 10^-2 C)2.4 × 10^-8 D)2.7 × 10^-3 E)1.2 × 10^-4

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 LiOH and 0.10 M HNO₃ D)a solution that is 0.10 M HNO₃ and 0.10 M LiNO₃ E)a solution that is 0.10 M HCN and 0.10 M KBr

Calculate the pH of a buffer that is 0.060 M HF and 0.030 M KF.The K_a for HF is 3.5 × 10^-4. A)2.06 B)4.86 C)3.16 D)3.56 E)3.76

Which metal hydroxide is most soluble in water? A)Fe(OH)₂;K_sp = 4.87 × 10^-17 B)Mg(OH)₂;K_sp = 2.06 × 10^-13 C)Ca(OH)₂;K_sp = 4.68 × 10^-6 D)Ba(OH)₂;K_sp = 5.0 × 10^-3

Which buffer controls the pH of blood? A)CH₃COOH and CH₃COO^- B)H₂CO₃ and HCO₃- C)NH₄⁺ and NH₃ D)H₃PO₄ and H₂PO₄^-

Copper(II)chloride is highly soluble in water.This compound has ________. A)high solubility product B)low solubility product C)high equilibrium constant D)high dissociation constant

An aqueous solution of 0.01 M NaCl and 0.01 M AgNO₃ are mixed.Which statement is true? (K_sp of AgCl = 1.8 × 10^-10) A)A precipitate of AgCl will form. B)No precipitate will form. C)The solution will not have any Ag+ and Cl^- ions after precipitation. D)None of the above

A buffer contains equal amounts of a weak acid and its conjugate base and has a pH of 5.25.Which would be a reasonable value of buffer pH after the addition of a small amount of base? A)4.15 B)5.35 C)5.15 D)6.35

Which solution is a buffer? A)a solution that is 0.200 M in H₃PO₄ and 0.200 M in HBr B)a solution that is 0.200 M in H₃PO₄ and 0.200 M in Na₂HPO₄ C)a solution that is 0.200 M in H₃PO₄ and 0.200 M in NaBr D)a solution that is 0.200 M in H₂SO₄ and 0.200 M in Na₂SO₄