Question 1

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( )

Accepted Answer

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Question 2

A solution containing 10.mmol of CO₃²⁻and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

Accepted Answer

To reach the first equivalence point, all CO₃²⁻ will be converted to HCO₃⁻. This requires 10 mmol of HCl. Using the concentration of HCl (1.1 M), the volume needed is 10 mmol / 1.1 M = 9.1 mL.

Question 3

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0072 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

Accepted Answer

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Question 4

The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is M.What is the solubility product constant for Fe(OH)₂?

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Question 5

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC₃H₅O₂,with strong base?

Accepted Answer

Propionic acid has a pKa of 4.87, which means that it will require a relatively strong base for neutralization. Thymol blue has a transition pH range of 8.0-9.6, which falls within the suitable range for titration of propionic acid, as it will be able to detect the pH change around the equivalence point. The other indicators have transition pH ranges that are too high or too low for this particular titration.

Question 6

What color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide?

Accepted Answer

Phenolphthalein changes from colorless to pink as the solution transitions from acidic to basic, which occurs when acetic acid is neutralized by sodium hydroxide.

Question 7

The K_sp of Ca(OH)₂ is 5.5 × 10^-5 at 25 °C.What is the concentration of OH^-(aq)in a saturated solution of Ca(OH)₂(aq)?

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Question 8

What is the molar solubility of silver(I)iodide at 25°C? The solubility product constant for silver(I)iodide is 8.3 × 10^-17 at 25°C.

Accepted Answer

The solubility product (Ksp) for silver(I) iodide (AgI) is given as 8.3 × 10^-17. The dissolution of AgI in water can be represented as AgI(s) ⇌ Ag+(aq) + I-(aq). Since each formula unit of AgI produces one Ag+ ion and one I- ion, if s is the molar solubility of AgI, then the concentrations of Ag+ and I- at equilibrium are both s. The Ksp expression is Ksp = [Ag+][I-] = s^2. Solving for s gives s = sqrt(Ksp) = sqrt(8.3 × 10^-17) = 9.1 × 10^-9 M.

Question 9

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

Accepted Answer

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Question 10

What is the pH of a saturated solution of Fe(OH)₂? (K_sp = 8.0 × 10^-16 and K_w = 1.01 × 10^-14)

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Question 11

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

Accepted Answer

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Question 12

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25 °C.What mass of BaSO₄ will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

Accepted Answer

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Question 13

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.

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Question 14

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

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Question 15

The solubility of manganese(II)carbonate is 5.4 × 10^-4 g/L.What is the solubility product constant for manganese(II)carbonate?

Accepted Answer

The solubility product constant (Ksp) for manganese(II) carbonate, MnCO3, can be calculated from its solubility. MnCO3 dissociates into Mn^2+ and CO3^2- ions in solution. Given the solubility is 5.4 × 10^-4 g/L, we first convert this to moles per liter (molarity, M) using the molar mass of MnCO3 (approximately 114.95 g/mol). This gives a solubility of about 4.7 × 10^-6 M. Since the dissociation produces one mole of Mn^2+ and one mole of CO3^2- for each mole of MnCO3 that dissolves, the concentrations of Mn^2+ and CO3^2- are each 4.7 × 10^-6 M in a saturated solution. The Ksp is the product of these concentrations: (4.7 × 10^-6)^2 = 2.2 × 10^-11.

Question 16

The solubility of strontium carbonate (SrCO₃)in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

Accepted Answer

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Question 17

A solution containing 10.mmol of CO₃²⁻ and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

Accepted Answer

The titration equation for CO₃²⁻ and HCO₃− is: CO₃²⁻ + HCl → CO₃− + H2O + Cl− In the first equivalence point, all of the HCO₃− will be neutralized to CO₃−, so the number of moles of HCl required is: mol of HCO₃− = 5.0 mmol mol of HCl = 5.0 mmol Since the concentration of the HCl is 1.1 M, the volume of HCl required is: V = mol of HCl / [HCl] = 5.0 mmol / 1.1 mol/L = 4.5 mL At the second equivalence point, all of the CO₃²⁻ will be neutralized to CO₃−, so the total number of moles of HCl required is: mol of HCO₃²⁻ + mol of HCO₃− = 10.0 mmol + 5.0 mmol = 15.0 mmol The volume of 1.1 M HCl required to reach the second equivalence point is: V = mol of HCl / [HCl] = 15.0 mmol / 1.1 mol/L = 13.6 mL Therefore, the best answer is D.

Question 18

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq).What is the pH after the addition of 32.0 mL of HCl(aq)? (K_b of C₆H₅CO₂^- = 1.6 × 10^-10)

Accepted Answer

1. Write the balanced equation for the reaction:
C6H5COO-Na+ (sodium benzoate) + HCl (hydrochloric acid)  →  C6H5COOH (benzoic acid) + NaCl (sodium chloride)

2. Write the equation for the dissociation of sodium benzoate:
C6H5COO-Na+ (sodium benzoate)  ↔  C6H5COO- (benzoate ion)  + Na+ (sodium ion)

3. Calculate the moles of sodium benzoate in the original solution:
moles of sodium benzoate = (0.10 M) x (25.0 mL/1000 mL) = 0.0025 mol

4. Since the initial solution of sodium benzoate is a salt and does not contain any significant amount of free H+ or OH- ions, we can assume that the initial pH of the solution is determined by the autoionization of water:
2H2O ↔ H3O+ + OH-
Kw = [H3O+][OH-] = 1.0 x 10^-14 mol^2/L^2
pKw = -logKw = 14.0
pH = 1/2(pKw - log[H3O+]) = 1/2(14.0 - 0) = 7.00

5. Calculate the moles of HCl added to the solution:
moles of HCl = (0.10 M) x (32.0 mL/1000 mL) = 0.0032 mol

6. Since the number of moles of HCl added is greater than the number of moles of sodium benzoate, the H+ ions from HCl will fully react with the benzoate ions to form benzoic acid:
moles of benzoate ion reacted = 0.0025 mol
moles of H+ added = 0.0032 mol
Since the reaction is 1:1, the excess moles of H+ will remain in the solution.

7. Calculate the final concentration of H+ ions in the solution:
moles of H+ remaining = 0.0032 mol - 0.0025 mol = 0.0007 mol
final volume of solution = 25.0 mL + 32.0 mL = 57.0 mL
final concentration of H+ ions = 0.0007 mol/0.057 L = 0.0123 M

8. Calculate the final pH of the solution:
pH = -log[H+] = -log(0.0123) = 1.91

Therefore, the correct answer is (C) 1.91.

Question 19

Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL of 0.1231 M NaOH to reach the endpoint.What is the molar mass of the acid?

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Question 20

An impure sample of sodium carbonate,Na₂CO₃,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq)+ Na₂CO₃(aq) CO₂(g)+ H₂O( )+ 2 NaCl(aq) What is the percent of Na₂CO₃ in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na₂CO₃ is 106.0 g/mol.

Accepted Answer

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Quiz 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

A solution containing 10.mmol of CO₃²⁻and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0072 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

The hydroxide ion concentration of a saturated solution of Fe(OH) ₂ is M.What is the solubility product constant for Fe(OH) ₂?

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC₃H₅O₂,with strong base?

What color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide?

The K_sp of Ca(OH) ₂ is 5.5 × 10^-5 at 25 °C.What is the concentration of OH^-(aq) in a saturated solution of Ca(OH) ₂(aq) ?

What is the molar solubility of silver(I) iodide at 25°C? The solubility product constant for silver(I) iodide is 8.3 × 10^-17 at 25°C.

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

What is the pH of a saturated solution of Fe(OH) ₂? (K_sp = 8.0 × 10^-16 and K_w = 1.01 × 10^-14)

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25 °C.What mass of BaSO₄ will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

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.

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

The solubility of manganese(II) carbonate is 5.4 × 10^-4 g/L.What is the solubility product constant for manganese(II) carbonate?

The solubility of strontium carbonate (SrCO₃) in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

A solution containing 10.mmol of CO₃²⁻ and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq) .What is the pH after the addition of 32.0 mL of HCl(aq) ? (K_b of C₆H₅CO₂^- = 1.6 × 10^-10)

Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL of 0.1231 M NaOH to reach the endpoint.What is the molar mass of the acid?

Quiz 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

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( )

A solution containing 10.mmol of CO32−and 5.0 mmol of HCO3−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0072 M Na2CO3? For Ag2CO3,Ksp = 8.6 × 10-12.

The hydroxide ion concentration of a saturated solution of Fe(OH) 2 is M.What is the solubility product constant for Fe(OH) 2?

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC3H5O2,with strong base?

What color change is exhibited by phenolphthalein during a titration of aqueous acetic acid with aqueous sodium hydroxide?

The Ksp of Ca(OH) 2 is 5.5 × 10-5 at 25 °C.What is the concentration of OH-(aq) in a saturated solution of Ca(OH) 2(aq) ?

What is the molar solubility of silver(I) iodide at 25°C? The solubility product constant for silver(I) iodide is 8.3 × 10-17 at 25°C.

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

What is the pH of a saturated solution of Fe(OH) 2? (Ksp = 8.0 × 10-16 and Kw = 1.01 × 10-14)

A 25.00-mL sample of propionic acid,HC3H5O2,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

The Ksp of BaSO4 is 1.1 × 10-10 at 25 °C.What mass of BaSO4 will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

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.

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

The solubility of manganese(II) carbonate is 5.4 × 10-4 g/L.What is the solubility product constant for manganese(II) carbonate?

The solubility of strontium carbonate (SrCO3) in water at 25°C is g/L.What is the Ksp of this sparingly soluble salt?

A solution containing 10.mmol of CO32− and 5.0 mmol of HCO3−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq) .What is the pH after the addition of 32.0 mL of HCl(aq) ? (Kb of C6H5CO2- = 1.6 × 10-10)

Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL of 0.1231 M NaOH to reach the endpoint.What is the molar mass of the acid?

An impure sample of sodium carbonate,Na2CO3,is titrated with 0.113 M HCl according to the reaction below. 2 HCl(aq) + Na2CO3(aq) CO2(g) + H2O( ) + 2 NaCl(aq) What is the percent of Na2CO3 in a 0.613 g sample if the titration requires 26.14 mL of HCl? The molar mass of Na2CO3 is 106.0 g/mol.

A solution containing 10.mmol of CO₃²⁻and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What volume of HCl must be added to reach the first equivalence point? (1 mmol = 0.001 mol)

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0072 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

The hydroxide ion concentration of a saturated solution of Fe(OH) ₂ is M.What is the solubility product constant for Fe(OH) ₂?

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC₃H₅O₂,with strong base?

The K_sp of Ca(OH) ₂ is 5.5 × 10^-5 at 25 °C.What is the concentration of OH^-(aq) in a saturated solution of Ca(OH) ₂(aq) ?

What is the molar solubility of silver(I) iodide at 25°C? The solubility product constant for silver(I) iodide is 8.3 × 10^-17 at 25°C.

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

What is the pH of a saturated solution of Fe(OH) ₂? (K_sp = 8.0 × 10^-16 and K_w = 1.01 × 10^-14)

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.145 M KOH.The equivalence point was reached when 43.02 mL of base had been added.What was the original concentration of the propionic acid?

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25 °C.What mass of BaSO₄ will dissolve in 1.0 L of water at 25 °C? (molar mass = 233.4 g/mol)

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.

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

The solubility of manganese(II) carbonate is 5.4 × 10^-4 g/L.What is the solubility product constant for manganese(II) carbonate?

The solubility of strontium carbonate (SrCO₃) in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

A solution containing 10.mmol of CO₃²⁻ and 5.0 mmol of HCO₃−is titrated with 1.1 M HCl.What total volume of HCl must be added to reach the second equivalence point? (1 mmol = 0.001 mol)

A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq) .What is the pH after the addition of 32.0 mL of HCl(aq) ? (K_b of C₆H₅CO₂^- = 1.6 × 10^-10)