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 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) 6.8 × 10-2 M A) 6.5 × 10-5 M B) 1.3 × 10-4 M C) 3.2 × 10-4 M D) 6.8 × 10-2 M

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 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

Calculate the pH of a buffer that is 0.105 M HC2H3O2 and 0.146 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 A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2)and 0.205 M in formic acid (HCO2H).The Ka of formic acid is 1.77 × 10-4.

A) 3.910 B) 3.587 C) 13.84 D) 10.10 E) 4.963 A) 3.910 B) 3.587 C) 13.84 D) 10.10 E) 4.963

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) 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.

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 A) 13.05 B) 13.10 C) 13.28 D) 13.58

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? Kb = 1.80 × 10-5 for NH3.

A) 9.08 B) 9.26 C) 9.43 D) 11.32 A) 9.08 B) 9.26 C) 9.43 D) 11.32

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 Ka = 1.8 × 10-5 for CH3CO2H.

A) 2.87 B) 3.74 C) 4.75 D) 5.74 A) 2.87 B) 3.74 C) 4.75 D) 5.74

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 A) 4.19 B) 9.69 C) 4.49 D) 4.31 E) 10.51

Exam 16: Aqueous Ionic Equilibrium

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.

(Multiple Choice)

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Question 21

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.

(Multiple Choice)

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Question 22

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.

(Multiple Choice)

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Question 23

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄)= 1.82 × 10^-8.

(Multiple Choice)

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Question 24

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.K_sp for TlCl is 1.7 × 10^-⁴.

(Multiple Choice)

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Question 25

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.

(Multiple Choice)

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Question 26

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.

(Multiple Choice)

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Question 27

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10?

(Multiple Choice)

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Question 28

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.

(Multiple Choice)

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Question 29

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.

(Multiple Choice)

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Question 30

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?

(Multiple Choice)

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Question 31

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.

(Multiple Choice)

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Question 32

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.

(Multiple Choice)

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Question 33

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?

(Multiple Choice)

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Question 34

Give the equation for a supersaturated solution in comparing Q with K_sp.

(Multiple Choice)

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Question 35

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.

(Multiple Choice)

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Question 36

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^-5for NH₃.

(Multiple Choice)

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Question 37

Give the equation for an unsaturated solution in comparing Q with K_sp.

(Multiple Choice)

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Question 38

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.

(Multiple Choice)

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Question 39

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.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 148

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 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 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.

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄)= 1.82 × 10^-8.

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 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.

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.

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10?

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.

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

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 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 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?

Give the equation for a supersaturated solution in comparing Q with K_sp.

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^-5for NH₃.

Give the equation for an unsaturated solution in comparing Q with K_sp.

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.

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.

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Exam 16: Aqueous Ionic Equilibrium

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 Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

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 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.

Determine the molar solubility of PbSO4 in pure water.Ksp (PbSO4)= 1.82 × 10-8.

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

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.

Calculate the pH of a buffer that is 0.105 M HC2H3O2 and 0.146 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

Which of the following acids (listed with pKa values)and their conjugate base would form a buffer with a pH of 8.10?

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2)and 0.205 M in formic acid (HCO2H).The Ka of formic acid is 1.77 × 10-4.

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?

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 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 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?

Give the equation for a supersaturated solution in comparing Q with Ksp.

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? Kb = 1.80 × 10-5 for NH3.

Give the equation for an unsaturated solution in comparing Q with Ksp.

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 Ka = 1.8 × 10-5 for CH3CO2H.

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.

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Thermochemistry

The Quantum-Mechanical Model of the Atom

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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 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 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.

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄)= 1.82 × 10^-8.

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 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.

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.

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10?

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.

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

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 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.

Give the equation for a supersaturated solution in comparing Q with K_sp.

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^-5for NH₃.

Give the equation for an unsaturated solution in comparing Q with K_sp.

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.

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.