Question 1

The solubility of all except which the following compounds increases as the pH of the solution decreases?

Accepted Answer

The solubility of KClO₄ is not affected by pH because it does not involve any acidic or basic ions that would react with H⁺ or OH^- ions in solution.

Question 2

The solubility of silver bromide is greater in 0.10 M NaBr than in pure water.

Accepted Answer

The solubility of silver bromide decreases in 0.10 M NaBr solution compared to pure water due to the common ion effect, where the presence of bromide ions from NaBr reduces the solubility of AgBr.

Question 3

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq)and 0.155 M NaHClO(aq),the final concentrations of HClO(aq)and ClO^-(aq),respectively,are

Accepted Answer

The addition of NaOH will react with HClO, decreasing its concentration and increasing the concentration of ClO⁻. The reaction is: HClO + OH⁻ → ClO⁻ + H₂O. The initial moles of HClO are 0.200 mol/L * 1.00 L = 0.200 mol, and NaOH added is 0.010 mol. After the reaction, HClO will be 0.200 mol - 0.010 mol = 0.190 mol, and ClO⁻ will be 0.155 mol + 0.010 mol = 0.165 mol. Dividing by 1.00 L gives concentrations of 0.190 M HClO and 0.165 M ClO⁻.

Question 4

If 50.0 mL of 0.22 M NaCl(aq)is mixed with 50.0 mL of 0.0050 M AgNO₃(aq),will AgCl(s)precipitate? K_sp(AgCl)= 1.6 × 10^-¹⁰.

Accepted Answer

The answer of If 50.0 mL of 0.22 M NaCl(aq)is...

Question 5

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

Accepted Answer

The answer of Assuming no volume change on mixing,what mass...

Question 6

The weak base,B,has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

Accepted Answer

The answer of The weak base,B,has K_b = 3.1 ×...

Question 7

You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,phenol (pK_a = 9.89),aniline (pK_b = 9.37),HNO₂ (pK_a = 3.37),CH₃NH₂ (pK_b = 3.44).Which two reagents would you use to make a buffer with a pH of 10.5?

Accepted Answer

CH₃NH₂ is a weak base with a pKₐ of 10.56 (calculated from pK_b = 3.44), close to the desired pH of 10.5. Adding HCl will partially protonate CH₃NH₂, forming a buffer system.

Question 8

The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

Accepted Answer

The formation of the coordination complex Ag(NH₃)₂⁺(aq) increases the solubility of silver chloride in 0.01 M NH₃(aq). This is because the complex can surround and stabilize the Ag+ ions, preventing them from precipitating out with the Cl- ions.

Question 9

How many moles of KOH(s)must be added to 1.00 L of 0.782 M HF(aq)to produce a buffer with a pH = 4.00?

Accepted Answer

The answer of How many moles of KOH(s)must be added...

Question 10

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

Accepted Answer

In the coordination complex, the thiosulfate ion acts as a Lewis base because it donates a pair of electrons to the silver ion, which is the Lewis acid.

Question 11

What is the equilibrium constant for the reaction HCN(aq)+ OH^-(aq) →CN^-(aq)+ H₂O(l)

Accepted Answer

The equilibrium constant for the reaction HCN(aq)+ OH^-(aq) →CN^-(aq)+ H₂O(l) is K_a/K_w. This is because the reaction is the conjugate acid-base reaction of the weak acid HCN and the weak base CN^-. The equilibrium constant for a conjugate acid-base reaction is equal to the ratio of the acid dissociation constant (K_a) of the acid to the water dissociation constant (K_w).

Question 12

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Accepted Answer

The answer of In the titration of 0.300 M CH₃NH₂(aq)with...

Question 13

In the titration of 0.300 M H₃PO₄(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

Accepted Answer

The answer of In the titration of 0.300 M H₃PO₄(aq)with...

Question 14

The K_spfor mercury(I)iodide is 1.2 * 10^-²⁸.What is the solubility of mercury(I)iodide?

Accepted Answer

The answer of The K_spfor mercury(I)iodide is 1.2 *...

Quiz 13: Aqueous Equilibria

The solubility of all except which the following compounds increases as the pH of the solution decreases?

The solubility of silver bromide is greater in 0.10 M NaBr than in pure water.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq) ,the final concentrations of HClO(aq) and ClO^-(aq) ,respectively,are

If 50.0 mL of 0.22 M NaCl(aq)is mixed with 50.0 mL of 0.0050 M AgNO₃(aq),will AgCl(s)precipitate? K_sp(AgCl)= 1.6 × 10^-¹⁰.

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The weak base,B,has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,phenol (pK_a = 9.89) ,aniline (pK_b = 9.37) ,HNO₂ (pK_a = 3.37) ,CH₃NH₂ (pK_b = 3.44) .Which two reagents would you use to make a buffer with a pH of 10.5?

The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

How many moles of KOH(s)must be added to 1.00 L of 0.782 M HF(aq)to produce a buffer with a pH = 4.00?

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

What is the equilibrium constant for the reaction HCN(aq) + OH^-(aq) →CN^-(aq) + H₂O(l)

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

In the titration of 0.300 M H₃PO₄(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

The K_spfor mercury(I) iodide is 1.2 * 10^-²⁸.What is the solubility of mercury(I) iodide?

Quiz 13: Aqueous Equilibria

The solubility of all except which the following compounds increases as the pH of the solution decreases?

The solubility of silver bromide is greater in 0.10 M NaBr than in pure water.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq) ,the final concentrations of HClO(aq) and ClO-(aq) ,respectively,are

If 50.0 mL of 0.22 M NaCl(aq)is mixed with 50.0 mL of 0.0050 M AgNO3(aq),will AgCl(s)precipitate? Ksp(AgCl)= 1.6 × 10-10.

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH3(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The weak base,B,has Kb = 3.1 × 10-4.The pH of a solution in which [B] = [BH+] is

You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,phenol (pKa = 9.89) ,aniline (pKb = 9.37) ,HNO2 (pKa = 3.37) ,CH3NH2 (pKb = 3.44) .Which two reagents would you use to make a buffer with a pH of 10.5?

The solubility of silver chloride is greater in 0.01 M NH3(aq)because of formation of the coordination complex Ag(NH3)2+(aq).

How many moles of KOH(s)must be added to 1.00 L of 0.782 M HF(aq)to produce a buffer with a pH = 4.00?

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

What is the equilibrium constant for the reaction HCN(aq) + OH-(aq) →CN-(aq) + H2O(l)

In the titration of 0.300 M CH3NH2(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

In the titration of 0.300 M H3PO4(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

The Ksp for mercury(I) iodide is 1.2 * 10-28.What is the solubility of mercury(I) iodide?

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq) ,the final concentrations of HClO(aq) and ClO^-(aq) ,respectively,are

If 50.0 mL of 0.22 M NaCl(aq)is mixed with 50.0 mL of 0.0050 M AgNO₃(aq),will AgCl(s)precipitate? K_sp(AgCl)= 1.6 × 10^-¹⁰.

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The weak base,B,has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,phenol (pK_a = 9.89) ,aniline (pK_b = 9.37) ,HNO₂ (pK_a = 3.37) ,CH₃NH₂ (pK_b = 3.44) .Which two reagents would you use to make a buffer with a pH of 10.5?

The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

What is the equilibrium constant for the reaction HCN(aq) + OH^-(aq) →CN^-(aq) + H₂O(l)

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

In the titration of 0.300 M H₃PO₄(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

The K_spfor mercury(I) iodide is 1.2 * 10^-²⁸.What is the solubility of mercury(I) iodide?