What is the molar solubility of Fe(OH)3(s)in a solution that is buffered at pH 2.50 at 25 S1U1P1$\circ$S1S1P0C? The Ksp of Fe(OH)3 is 6.3 $\times$ 10-38 at 25 S1U1P1$\circ$S1S1P0C.

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

In which of the following solutions would silver(I)phosphate,Ag3PO4,be least soluble?

A) 0.10 M Na3PO4 B) 0.10 M AgNO3 C) 0.10 M Na2HPO4 D) 0.10 M HNO3 E) 0.10 M NaH2PO4 A) 0.10 M Na3PO4 B) 0.10 M AgNO3 C) 0.10 M Na2HPO4 D) 0.10 M HNO3 E) 0.10 M NaH2PO4

If 30 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 $\times$ 10-5 at 25°C.

A) 10.4 B) 4.3 C) 5.0 D) 2.7 E) 4.5 A) 10.4 B) 4.3 C) 5.0 D) 2.7 E) 4.5

What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 $\times$ 10-10)

A) 4.80 B) 8.75 C) 9.20 D) 9.25 E) 9.76 A) 4.80 B) 8.75 C) 9.20 D) 9.25 E) 9.76

What is the pH of the buffer that results when 12.0 g of NaH2PO4 and 8.00 g of Na2HPO4 are diluted with water to a volume of 0.50 L? (Ka of H2PO4- = 6.2 $\times$ 10-8,the molar masses of NaH2PO4 and Na2HPO4 are 120.0 g/mol and 142.0 mol,respectively)

A) 4.10 B) 6.96 C) 7.21 D) 7.46 E) 9.90 A) 4.10 B) 6.96 C) 7.21 D) 7.46 E) 9.90

What is the maximum hydroxide-ion concentration that a 0.027 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2,Ksp = 1.8 $\times$ 10-11.

A) 4.2 $\times$ 10-6 B) 1.7 $\times$ 10-4 C) 1.2 $\times$ 10-8 D) 6.7 $\times$ 10-9 E) 2.6 $\times$ 10-5 A) 4.2 $\times$ 10-6 B) 1.7 $\times$ 10-4 C) 1.2 $\times$ 10-8 D) 6.7 $\times$ 10-9 E) 2.6 $\times$ 10-5

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

What mass of sodium hydroxide must be added to 40.0 mL of 0.607 M acetic acid in order to create a buffer with a pH of 4.66? K_a for acetic acid is 1.8 $\times$ 10^-5.

(Multiple Choice)

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Question 41

Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid? 1)The moles of acid added from the buret equals the initial moles of weak base. 2)The volume of acid added from the buret must equal the volume of base titrated. 3)The pH of the solution is less than 7.00.

(Multiple Choice)

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Question 42

If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.

(Short Answer)

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Question 43

A 50.00-mL solution of 0.0797 M ammonia (K_b = 1.8 $\times$ 10^-5)is titrated with a 0.0315 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 23.88 mL of titrant have been added? (K_w = 1.00 $\times$ 10^-14)

(Multiple Choice)

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Question 44

What is the molar solubility of Fe(OH)₃(s)in a solution that is buffered at pH 2.50 at 25 ^$\circ$C? The K_sp of Fe(OH)₃ is 6.3 $\times$ 10^-38 at 25 ^$\circ$C.

(Multiple Choice)

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Question 45

In which of the following solutions would silver(I)phosphate,Ag₃PO₄,be least soluble?

(Multiple Choice)

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Question 46

If 25 mL of 0.750 M HCl are added to 100.mL of 0.392 M NaOH,what is the final pH?

(Multiple Choice)

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Question 47

A 50.00-mL solution of 0.0350 M quinoline (K_b = 8.0 $\times$ 10^-10)is titrated with a 0.0137 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (K_w = 1.0 $\times$ 10^-14)

(Multiple Choice)

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Question 48

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) C₈H₄O₄^2-(aq)+ H₂O( )

(Multiple Choice)

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Question 49

If 500 mL of 1.2 $\times$ 10^-6 M AgNO₃ is mixed with 500 mL of 1.2 $\times$ 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 $\times$ 10^-13.

(Multiple Choice)

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Question 50

The concentration of magnesium carbonate in a saturated aqueous solution at 25°C is M.What is the K_sp of this sparingly soluble salt?

(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 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 $\times$ 10^-3,K_a2 = 6.2 $\times$ 10^-8,and K_a3 = 3.6 $\times$ 10^-13)

(Multiple Choice)

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Question 52

You have 75.0 mL of 0.11 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 53

If 30 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 $\times$ 10^-5 at 25°C.

(Multiple Choice)

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Question 54

What is the pH of an aqueous solution composed of 0.64 M NH₄⁺ and 0.20 M NH₃? (K_a of NH₄⁺ = 5.6 $\times$ 10^-10)

(Multiple Choice)

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Question 55

What is the pH of the buffer that results when 12.0 g of NaH₂PO₄ and 8.00 g of Na₂HPO₄ are diluted with water to a volume of 0.50 L? (K_a of H₂PO₄^- = 6.2 $\times$ 10^-8,the molar masses of NaH₂PO₄ and Na₂HPO₄ are 120.0 g/mol and 142.0 mol,respectively)

(Multiple Choice)

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Question 56

A certain weak base B has a base-ionization constant K_b of 7.3 $\times$ 10^-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH⁺]?

(Multiple Choice)

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Question 57

Which of the following mathematical expressions is the Henderson-Hasselbalch equation?

(Multiple Choice)

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Question 58

What is the maximum hydroxide-ion concentration that a 0.027 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 $\times$ 10^-11.

(Multiple Choice)

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Question 59

Two important biological buffer systems control pH in the range between 6.9 and 7.4.These buffer systems are H₂CO₃/HCO₃^- and ________.

(Essay)

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Question 60

Showing 41 - 60 of 88

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

What mass of sodium hydroxide must be added to 40.0 mL of 0.607 M acetic acid in order to create a buffer with a pH of 4.66? Ka for acetic acid is 1.8 ×\times× 10-5.

If the ratio of acid to base in a buffer is increased by a factor of 10,the buffer pH decreases by ________.

A 50.00-mL solution of 0.0797 M ammonia (Kb = 1.8 ×\times× 10-5)is titrated with a 0.0315 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 23.88 mL of titrant have been added? (Kw = 1.00 ×\times× 10-14)

What is the molar solubility of Fe(OH)3(s)in a solution that is buffered at pH 2.50 at 25 ∘\circ∘ C? The Ksp of Fe(OH)3 is 6.3 ×\times× 10-38 at 25 ∘\circ∘ C.

In which of the following solutions would silver(I)phosphate,Ag3PO4,be least soluble?

If 25 mL of 0.750 M HCl are added to 100.mL of 0.392 M NaOH,what is the final pH?

A 50.00-mL solution of 0.0350 M quinoline (Kb = 8.0 ×\times× 10-10)is titrated with a 0.0137 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (Kw = 1.0 ×\times× 10-14)

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) C8H4O42-(aq)+ H2O( )

If 500 mL of 1.2 ×\times× 10-6 M AgNO3 is mixed with 500 mL of 1.2 ×\times× 10-6 M NaBr,what will occur? For AgBr,Ksp = 5 ×\times× 10-13.

The concentration of magnesium carbonate in a saturated aqueous solution at 25°C is M.What is the Ksp of this sparingly soluble salt?

What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 ×\times× 10-3,Ka2 = 6.2 ×\times× 10-8,and Ka3 = 3.6 ×\times× 10-13)

You have 75.0 mL of 0.11 M HA.After adding 30.0 mL of 0.10 M NaOH,the pH is 5.50.What is the Ka value of HA?

If 30 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 ×\times× 10-5 at 25°C.

What is the pH of an aqueous solution composed of 0.64 M NH4+ and 0.20 M NH3? (Ka of NH4+ = 5.6 ×\times× 10-10)

What is the pH of the buffer that results when 12.0 g of NaH2PO4 and 8.00 g of Na2HPO4 are diluted with water to a volume of 0.50 L? (Ka of H2PO4- = 6.2 ×\times× 10-8,the molar masses of NaH2PO4 and Na2HPO4 are 120.0 g/mol and 142.0 mol,respectively)

A certain weak base B has a base-ionization constant Kb of 7.3 ×\times× 10-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH+]?

Which of the following mathematical expressions is the Henderson-Hasselbalch equation?

What is the maximum hydroxide-ion concentration that a 0.027 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2,Ksp = 1.8 ×\times× 10-11.

Two important biological buffer systems control pH in the range between 6.9 and 7.4.These buffer systems are H2CO3/HCO3- and ________.

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What mass of sodium hydroxide must be added to 40.0 mL of 0.607 M acetic acid in order to create a buffer with a pH of 4.66? K_a for acetic acid is 1.8 $\times$ 10^-5.

A 50.00-mL solution of 0.0797 M ammonia (K_b = 1.8 $\times$ 10^-5)is titrated with a 0.0315 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 23.88 mL of titrant have been added? (K_w = 1.00 $\times$ 10^-14)

What is the molar solubility of Fe(OH)₃(s)in a solution that is buffered at pH 2.50 at 25 ^$\circ$C? The K_sp of Fe(OH)₃ is 6.3 $\times$ 10^-38 at 25 ^$\circ$C.

In which of the following solutions would silver(I)phosphate,Ag₃PO₄,be least soluble?

A 50.00-mL solution of 0.0350 M quinoline (K_b = 8.0 $\times$ 10^-10)is titrated with a 0.0137 M solution of hydrochloric acid as the titrant.What is the pH at the equivalence point? (K_w = 1.0 $\times$ 10^-14)

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) C₈H₄O₄^2-(aq)+ H₂O( )

If 500 mL of 1.2 $\times$ 10^-6 M AgNO₃ is mixed with 500 mL of 1.2 $\times$ 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 $\times$ 10^-13.

The concentration of magnesium carbonate in a saturated aqueous solution at 25°C is M.What is the K_sp of this sparingly soluble salt?

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 $\times$ 10^-3,K_a2 = 6.2 $\times$ 10^-8,and K_a3 = 3.6 $\times$ 10^-13)

You have 75.0 mL of 0.11 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?

If 30 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 $\times$ 10^-5 at 25°C.

What is the pH of an aqueous solution composed of 0.64 M NH₄⁺ and 0.20 M NH₃? (K_a of NH₄⁺ = 5.6 $\times$ 10^-10)

What is the pH of the buffer that results when 12.0 g of NaH₂PO₄ and 8.00 g of Na₂HPO₄ are diluted with water to a volume of 0.50 L? (K_a of H₂PO₄^- = 6.2 $\times$ 10^-8,the molar masses of NaH₂PO₄ and Na₂HPO₄ are 120.0 g/mol and 142.0 mol,respectively)

A certain weak base B has a base-ionization constant K_b of 7.3 $\times$ 10^-4 at 25°C.If strong acid is added to a solution of B,at what pH will [B] = [BH⁺]?

What is the maximum hydroxide-ion concentration that a 0.027 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 $\times$ 10^-11.

Two important biological buffer systems control pH in the range between 6.9 and 7.4.These buffer systems are H₂CO₃/HCO₃^- and ________.