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Exam 17: Aqueous Ionic Equilibrium

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Question 51

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A 25.0-mL sample of 0.150 M butanoic 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 butanoic acid is 1.5 × 10^-5.

A) 4.55
B) 1.34
C) 3.08
D) 4.88
E) 4.77

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Question 52

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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.

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Question 53

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The largest change in pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

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 1.50 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 K_a for HF is 3.5 × 10^-4.

What is the molar solubility of calcium fluoride (CaF₂) in water? The solubility-product constant for CaF₂ is 3.9 × 10^-11 at 25°C.

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.

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have

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.

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.

Give the expression for K_f for Co(SCN) ₄^2-.

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 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 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 nitrous acid is 1.36 × 10^-3.

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M NaF.The K_a for HF is 3.5 × 10^-4.

Determine the molar solubility of CaSO₄ in a solution containing 0.12 M K₂SO₄. K_sp (CaSO₄) = 2.4 × 10^-5.

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.

Calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF.The K_a for HF is 3.5 × 10^-4.

A complex ion contains

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.

Which one of the following statements is TRUE?