The hydroxide ion concentration of a saturated solution of Fe(OH)2 is $1.16 \times 10 ^ { - 5 }$ M. What is the solubility product constant for Fe(OH)2?

A) $7.9 \times 10 ^ { - 16 }$ B) $6.32 \times 10 ^ { - 15 }$ C) $1.58 \times 10 ^ { - 15 }$ D) $3.41 \times 10 ^ { - 3 }$ E) $2.27 \times 10 ^ { - 2 }$ A) $7.9 \times 10 ^ { - 16 }$ B) $6.32 \times 10 ^ { - 15 }$ C) $1.58 \times 10 ^ { - 15 }$ D) $3.41 \times 10 ^ { - 3 }$ E) $2.27 \times 10 ^ { - 2 }$

How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq) to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol A) 0.36 mol B) 0.44 mol C) 0.56 mol D) 0.64 mol E) 1.8 mol

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2) is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H) and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 × 10-5)

A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74 A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74

Given the following reactions, AgBr(s) $\leftrightharpoons$ Ag+(aq) + Br-(aq) Ksp = 5.4 × 10-13 Ag+(aq) + 2 CN-(aq) $\leftrightharpoons$ Ag(CN)2-(aq) Kf = 1.2 × 1021 Determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN-(aq) $\leftrightharpoons$ Ag(CN)2-(aq) + Br-(aq)

A) 4.5 × 10-34 B) 1.5 × 10-9 C) 6.5 × 108 D) 1.2 × 1021 E) 2.2 × 1033 A) 4.5 × 10-34 B) 1.5 × 10-9 C) 6.5 × 108 D) 1.2 × 1021 E) 2.2 × 1033

Suppose 50.00 mL of 2.0 × 10-5 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-4 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10-14.

A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp. A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp.

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2, Ksp = 1.8 × 10-11.

A) 4.2 × 10-6 B) 1.7 × 10-4 C) 1.2 × 10-8 D) 9.5 × 10-9 E) 3.1 × 10-5 A) 4.2 × 10-6 B) 1.7 × 10-4 C) 1.2 × 10-8 D) 9.5 × 10-9 E) 3.1 × 10-5

What is the molar solubility of solid iron(III) hydroxide, Fe(OH)3, in a solution that is buffered to a pH of 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25 °C.

A) 6.9 × 10-28 mol/L B) 2.0 × 10-26 mol/L C) 1.3 × 10-13 mol/L D) 2.0 × 10-3 mol/L E) 5.0 × 102 mol/L A) 6.9 × 10-28 mol/L B) 2.0 × 10-26 mol/L C) 1.3 × 10-13 mol/L D) 2.0 × 10-3 mol/L E) 5.0 × 102 mol/L

Consider the reaction Cu2+(aq) + 4 NH3(aq) $\leftrightharpoons$ Cu(NH3)42+(aq) Kf = 2.1 × 1013 If the Ksp for Cu(OH)2 is 2.2 × 10-20, what is the value of the equilibrium constant, K, for the reaction below? Cu(NH3)42+(aq) + 2 OH-(aq) $\leftrightharpoons$ Cu(OH)2(s) + 4 NH3(aq)

A) 1.0 × 10-33 B) 4.6 × 10-7 C) 2.1 × 1013 D) 2.2 × 106 E) 9.5 × 1032 A) 1.0 × 10-33 B) 4.6 × 10-7 C) 2.1 × 1013 D) 2.2 × 106 E) 9.5 × 1032

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 × 10-5)

A) 9.98 B) 4.02 C) 8.53 D) 9.26 E) none of these A) 9.98 B) 4.02 C) 8.53 D) 9.26 E) none of these

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO2H) is titrated with 0.100 M aqueous potassium hydroxide? (Ka of HCO2H = 1.8 × 10-4)

A) 5.71 B) 7.00 C) 8.28 D) 8.52 E) 10.26 A) 5.71 B) 7.00 C) 8.28 D) 8.52 E) 10.26

Exam 18: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

(Multiple Choice)

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Question 41

The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is $1.16 \times 10 ^ { - 5 }$ M. What is the solubility product constant for Fe(OH)₂?

(Multiple Choice)

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Question 42

Given the two equilibria below, Ag(NH₃)₂⁺(aq) $\rightleftharpoons$ $\leftrightharpoons$ Ag⁺(aq) + 2NH₃(aq); K_d = 5.9 × 10^-8 AgCN(s) $\rightleftharpoons$ Ag⁺(aq) + CN?(aq); K_sp = $2.2 \times 10 ^ { - 16 }$ what is K for the following equilibrium? AgCN(s) + 2NH₃(aq) $\rightleftharpoons$ Ag(NH₃)₂⁺(aq) + CN^-(aq)

(Multiple Choice)

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Question 43

How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq) to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

(Multiple Choice)

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Question 44

What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂) is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H) and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 × 10^-5)

(Multiple Choice)

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Question 45

Given the following reactions, AgBr(s) $\leftrightharpoons$ Ag⁺(aq) + Br^-(aq) K_sp = 5.4 × 10^-13 Ag⁺(aq) + 2 CN^-(aq) $\leftrightharpoons$ Ag(CN)₂^-(aq) K_f = 1.2 × 10²¹ Determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN^-(aq) $\leftrightharpoons$ Ag(CN)₂^-(aq) + Br^-(aq)

(Multiple Choice)

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Question 46

Suppose 50.00 mL of 2.0 × 10^-5 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃. Which of the following statements is true? For Fe(IO₃)₃, K_sp = 1.0 × 10^-14.

(Multiple Choice)

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Question 47

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂, K_sp = 1.8 × 10^-11.

(Multiple Choice)

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Question 48

What is the molar solubility of solid iron(III) hydroxide, Fe(OH)₃, in a solution that is buffered to a pH of 2.50 at 25 °C? The K_sp of Fe(OH)₃ is 6.3 × 10^-38 at 25 °C.

(Multiple Choice)

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Question 49

Potassium hydrogen phthalate (KHP) is used to standardize sodium hydroxide. If 35.39 mL of NaOH(aq) is required to titrate 0.8246 g KHP to the equivalence point, what is the concentration of the NaOH(aq)? (The molar mass of KHP = 204.2 g/mol) HC₈H₄O₄^-(aq) + OH^-(aq) $\leftrightharpoons$ C₈H₄O₄^2-(aq) + H₂O( $\ell$ )

(Multiple Choice)

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Question 50

What is the solubility product expression for La(OH)₃?

(Multiple Choice)

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Question 51

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 3.6 × 10^-13)

(Multiple Choice)

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Question 52

Consider the reaction Cu²⁺(aq) + 4 NH₃(aq) $\leftrightharpoons$ Cu(NH₃)₄²⁺(aq) K_f = 2.1 × 10¹³ If the K_sp for Cu(OH)₂ is 2.2 × 10^-20, what is the value of the equilibrium constant, K, for the reaction below? Cu(NH₃)₄²⁺(aq) + 2 OH^-(aq) $\leftrightharpoons$ Cu(OH)₂(s) + 4 NH₃(aq)

(Multiple Choice)

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Question 53

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH₃ with 100.0 mL of 0.100 M HCl. (K_b for NH₃ = 1.8 × 10^-5)

(Multiple Choice)

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Question 54

A 50.00-mL solution of 0.0426 M trimethylamine (K_b = 6.5 × 10^-5) is titrated with a 0.0257 M solution of hydrochloric acid as the titrant. What is the pH of the base solution after 22.31 mL of titrant have been added? (K_w = 1.00 × 10^-14)

(Multiple Choice)

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Question 55

If 25 mL of 0.750 M HCl are added to 100. mL of 0.302 M NaOH, what is the final pH?

(Multiple Choice)

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Question 56

For a monoprotic acid titration, the _____ in a titration is the point where number of moles of a strong base added equals the number of moles of an acid initially present.

(Short Answer)

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Question 57

What will be the pH of the solution when 0.10 mol of H⁺ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia, NH3, and 0.26 M ammonium fluoride, NH₄F? (K_b for ammonia = 1.8 × 10^-5)

(Multiple Choice)

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Question 58

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO₂H) is titrated with 0.100 M aqueous potassium hydroxide? (K_a of HCO₂H = 1.8 × 10^-4)

(Multiple Choice)

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Question 59

You have 75.0 mL of 0.17 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the K_a value of HA?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 87

Exam 18: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Which acid-base combination is depicted by this titration curve? The dot on the curve is located at the titrant volume where the titration solution pH equals 7.

The hydroxide ion concentration of a saturated solution of Fe(OH)2 is 1.16×10−51.16 \times 10 ^ { - 5 }1.16×10−5 M. What is the solubility product constant for Fe(OH)2?

How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq) to make a buffer with a pH of 9.00? (pKa of NH4+ = 9.25)

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2) is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H) and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 × 10-5)

Suppose 50.00 mL of 2.0 × 10-5 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-4 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10-14.

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2, Ksp = 1.8 × 10-11.

What is the molar solubility of solid iron(III) hydroxide, Fe(OH)3, in a solution that is buffered to a pH of 2.50 at 25 °C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25 °C.

What is the solubility product expression for La(OH)3?

What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 3.6 × 10-13)

Consider the reaction Cu2+(aq) + 4 NH3(aq) ⇋\leftrightharpoons⇋ Cu(NH3)42+(aq) Kf = 2.1 × 1013 If the Ksp for Cu(OH)2 is 2.2 × 10-20, what is the value of the equilibrium constant, K, for the reaction below? Cu(NH3)42+(aq) + 2 OH-(aq) ⇋\leftrightharpoons⇋ Cu(OH)2(s) + 4 NH3(aq)

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 × 10-5)

A 50.00-mL solution of 0.0426 M trimethylamine (Kb = 6.5 × 10-5) is titrated with a 0.0257 M solution of hydrochloric acid as the titrant. What is the pH of the base solution after 22.31 mL of titrant have been added? (Kw = 1.00 × 10-14)

If 25 mL of 0.750 M HCl are added to 100. mL of 0.302 M NaOH, what is the final pH?

For a monoprotic acid titration, the _____ in a titration is the point where number of moles of a strong base added equals the number of moles of an acid initially present.

What will be the pH of the solution when 0.10 mol of H+ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia, NH3, and 0.26 M ammonium fluoride, NH4F? (Kb for ammonia = 1.8 × 10-5)

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO2H) is titrated with 0.100 M aqueous potassium hydroxide? (Ka of HCO2H = 1.8 × 10-4)

You have 75.0 mL of 0.17 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka value of HA?

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The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is $1.16 \times 10 ^ { - 5 }$ M. What is the solubility product constant for Fe(OH)₂?

How many moles of HCl must be added to 1.0 L of 1.0 M NH₃(aq) to make a buffer with a pH of 9.00? (pK_a of NH₄⁺ = 9.25)

What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂) is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H) and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 × 10^-5)

Suppose 50.00 mL of 2.0 × 10^-5 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃. Which of the following statements is true? For Fe(IO₃)₃, K_sp = 1.0 × 10^-14.

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂, K_sp = 1.8 × 10^-11.

What is the molar solubility of solid iron(III) hydroxide, Fe(OH)₃, in a solution that is buffered to a pH of 2.50 at 25 °C? The K_sp of Fe(OH)₃ is 6.3 × 10^-38 at 25 °C.

What is the solubility product expression for La(OH)₃?

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.25 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 3.6 × 10^-13)

Calculate the pH of a solution made by mixing 100.0 mL of 0.627 M NH₃ with 100.0 mL of 0.100 M HCl. (K_b for NH₃ = 1.8 × 10^-5)

A 50.00-mL solution of 0.0426 M trimethylamine (K_b = 6.5 × 10^-5) is titrated with a 0.0257 M solution of hydrochloric acid as the titrant. What is the pH of the base solution after 22.31 mL of titrant have been added? (K_w = 1.00 × 10^-14)

What will be the pH of the solution when 0.10 mol of H⁺ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia, NH3, and 0.26 M ammonium fluoride, NH₄F? (K_b for ammonia = 1.8 × 10^-5)

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO₂H) is titrated with 0.100 M aqueous potassium hydroxide? (K_a of HCO₂H = 1.8 × 10^-4)

You have 75.0 mL of 0.17 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the K_a value of HA?