What is the pH of a solution prepared by mixing 50.00 mL of 0.10 mol L-1 NH3 with 5.00 mL of 0.10 mol L-1 NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

A) 8.25 B) 9.28 C) 10.26 D) 11.13 A) 8.25 B) 9.28 C) 10.26 D) 11.13

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 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

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution.What is the pH before any base is added? Hydrofluoric acid is monoprotic.The $K _ { a }$ of hydrofluoric acid is 3.5 × 10-4.

A) 2.33 × 10-3 B) 2.63 C) 3.46 D) 7.07 × 10-3 E) 2.15 A) 2.33 × 10-3 B) 2.63 C) 3.46 D) 7.07 × 10-3 E) 2.15

What is the molar solubility of AgCl in 0.40 mol L-1 NH3? Ksp for AgCl is $1.8 \times 10 ^{- 10}$ and Kf for Ag(NH3)2+ is $1.7 \times 10^7$

A) 1.3 × 10-5 mol L-1 B) 2.0 × 10-5 mol L-1 C) 2.2 × 10-2 mol L-1 D) 5.5 × 10-2 mol L-1 A) 1.3 × 10-5 mol L-1 B) 2.0 × 10-5 mol L-1 C) 2.2 × 10-2 mol L-1 D) 5.5 × 10-2 mol L-1

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi.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 CH3COOH D) adding 0.050 moles of CH3COOLi E) adding 0.050 moles of NH4Cl. A) adding 0.050 moles of NaOH B) adding 0.050 moles of HCl C) adding 0.050 moles of CH3COOH D) adding 0.050 moles of CH3COOLi E) adding 0.050 moles of NH4Cl.

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 mol L-1 B) 1.62 × 10-17 mol L-1 C) 4.03 × 10-9 mol L-1 D) 3.65 × 10-6 mol L-1 E) 2.30 × 10-6 mol L-1 A) 2.44 × 10-17 mol L-1 B) 1.62 × 10-17 mol L-1 C) 4.03 × 10-9 mol L-1 D) 3.65 × 10-6 mol L-1 E) 2.30 × 10-6 mol L-1

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 100.0 mL of 0.20 mol L-1 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 A) 9.13 B) 9.25 C) 9.53 D) 4.74 E) 8.98

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

(Multiple Choice)

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Question 61

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 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 62

Identify the compound that is base-insoluble.

(Multiple Choice)

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Question 63

Calculate the pH of a buffer that is 0.158 mol L^-1 HClO and 0.099 mol L^-1 NaClO.The K_a for HClO is 2.9 × 10^-8.

(Multiple Choice)

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Question 64

A solution contains 0.036 mol L^-1 Cu²⁺ and 0.044 mol L^-1 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 65

A 25.0 mL sample of 0.150 mol L^-1 hydrofluoric acid is titrated with a 0.150 mol L^-¹ NaOH solution.What is the pH before any base is added? Hydrofluoric acid is monoprotic.The $K _ { a }$ of hydrofluoric acid is 3.5 × 10^-4.

(Multiple Choice)

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Question 66

What is the molar solubility of AgCl in 0.40 mol L^-1 NH₃? K_sp for AgCl is $1.8 \times 10 ^{- 10}$ and K_f for Ag(NH₃)₂⁺ is $1.7 \times 10^7$

(Multiple Choice)

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Question 67

A 1.0 L buffer solution is 0.050 mol L^-1 CH₃COOH and 0.250 mol L^-1 CH₃COOLi.Which of the following actions will destroy the buffer?

(Multiple Choice)

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Question 68

For a monoprotic weak acid titrated with a strong base,is the equivalence point acidic,basic,or neutral?

(Short Answer)

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Question 69

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

(Multiple Choice)

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Question 70

A 25.0 mL sample of 0.150 mol L^-1acetic acid is titrated with a 0.150 mol L^-1 NaOH solution.What is the pH after 26.0 mL of base is added? The $K _ { a }$ of acetic acid is 1.8 × 10^-5.

(Multiple Choice)

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Question 71

Determine the molar solubility of Fe(OH)₂in pure water.K_sp for Fe(OH)₂ = 4.87 × 10^-17.

(Multiple Choice)

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Question 72

How many millilitres of 0.0890 mol L^-1 NaOH are required to titrate 25.0 mL of 0.0680 $\operatorname { mol } \mathrm { L } ^ { - 1 } \mathrm { HBr }$ to the equivalence point?

(Multiple Choice)

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Question 73

Which of the following is the correct equation relating Q to K_sp for a supersaturated solution?

(Multiple Choice)

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Question 74

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

(Multiple Choice)

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Question 75

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 mol L^-1 NaOH? K_a = 6.76 × 10^-4 for HF.

(Multiple Choice)

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Question 76

Identify the pH of normal blood.

(Multiple Choice)

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Question 77

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH.Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

(Multiple Choice)

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Question 78

What is the maximum ratio of conjugate base to acid in an effective buffer?

(Multiple Choice)

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Question 79

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 NH₄Cl with 100.0 mL of 0.20 mol L^-1 NH₃.The K_b for NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 159

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 mol L-1 NH3 with 5.00 mL of 0.10 mol L-1 NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Identify the compound that is base-insoluble.

Calculate the pH of a buffer that is 0.158 mol L-1 HClO and 0.099 mol L-1 NaClO.The Ka for HClO is 2.9 × 10-8.

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution.What is the pH before any base is added? Hydrofluoric acid is monoprotic.The KaK _ { a }Ka​ of hydrofluoric acid is 3.5 × 10-4.

What is the molar solubility of AgCl in 0.40 mol L-1 NH3? Ksp for AgCl is 1.8×10−101.8 \times 10 ^{- 10}1.8×10−10 and Kf for Ag(NH3)2+ is 1.7×1071.7 \times 10^71.7×107

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi.Which of the following actions will destroy the buffer?

For a monoprotic weak acid titrated with a strong base,is the equivalence point acidic,basic,or neutral?

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 mol L-1 in calcium ion and 2.33 × 10-4 mol L-1 in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

A 25.0 mL sample of 0.150 mol L-1 acetic acid is titrated with a 0.150 mol L-1 NaOH solution.What is the pH after 26.0 mL of base is added? The KaK _ { a }Ka​ of acetic acid is 1.8 × 10-5.

Determine the molar solubility of Fe(OH)2 in pure water.Ksp for Fe(OH)2 = 4.87 × 10-17.

How many millilitres of 0.0890 mol L-1 NaOH are required to titrate 25.0 mL of 0.0680 mol⁡L−1HBr\operatorname { mol } \mathrm { L } ^ { - 1 } \mathrm { HBr }molL−1HBr to the equivalence point?

Which of the following is the correct equation relating Q to Ksp for a supersaturated solution?

Determine the molar solubility of AgI in pure water.Ksp (AgI)= 8.51 × 10-17.

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 mol L-1 NaOH? Ka = 6.76 × 10-4 for HF.

Identify the pH of normal blood.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

What is the maximum ratio of conjugate base to acid in an effective buffer?

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 100.0 mL of 0.20 mol L-1 NH3.The Kb for NH3 is 1.8 × 10-5.

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What is the pH of a solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the pH of a buffer that is 0.158 mol L^-1 HClO and 0.099 mol L^-1 NaClO.The K_a for HClO is 2.9 × 10^-8.

A 25.0 mL sample of 0.150 mol L^-1 hydrofluoric acid is titrated with a 0.150 mol L^-¹ NaOH solution.What is the pH before any base is added? Hydrofluoric acid is monoprotic.The $K _ { a }$ of hydrofluoric acid is 3.5 × 10^-4.

What is the molar solubility of AgCl in 0.40 mol L^-1 NH₃? K_sp for AgCl is $1.8 \times 10 ^{- 10}$ and K_f for Ag(NH₃)₂⁺ is $1.7 \times 10^7$

A 1.0 L buffer solution is 0.050 mol L^-1 CH₃COOH and 0.250 mol L^-1 CH₃COOLi.Which of the following actions will destroy the buffer?

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

A 25.0 mL sample of 0.150 mol L^-1acetic acid is titrated with a 0.150 mol L^-1 NaOH solution.What is the pH after 26.0 mL of base is added? The $K _ { a }$ of acetic acid is 1.8 × 10^-5.

Determine the molar solubility of Fe(OH)₂in pure water.K_sp for Fe(OH)₂ = 4.87 × 10^-17.

How many millilitres of 0.0890 mol L^-1 NaOH are required to titrate 25.0 mL of 0.0680 $\operatorname { mol } \mathrm { L } ^ { - 1 } \mathrm { HBr }$ to the equivalence point?

Which of the following is the correct equation relating Q to K_sp for a supersaturated solution?

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

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 mol L^-1 NaOH? K_a = 6.76 × 10^-4 for HF.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH.Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 NH₄Cl with 100.0 mL of 0.20 mol L^-1 NH₃.The K_b for NH₃ is 1.8 × 10^-5.