Acid and Base Equilibria
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.110 M solution of a weak acid has a pH of 2.84. What is the value of Ka for the acid?
1.8 × 10⁻⁵
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.250 M solution of a weak acid has a pH of 2.67. What is the value of Ka for the acid?
1.8 × 10⁻⁵
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.110 M solution of HBrO? Ka of HBrO = 2.8 × 10⁻⁹
4.74
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.250 M solution of HCN? Ka of HCN = 4.9 × 10⁻¹⁰
4.96
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 6.00 M H₃PO₄ solution? For H₃PO₄, Ka₁ = 7.5 × 10⁻³, Ka₂ = 6.2 × 10⁻⁸, and Ka₃ = 4.2 × 10⁻¹³.
0.68
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a solution that has 0.300 M HNO₂ and 0.300 M HCN? Ka of HNO₂ = 4.6 × 10⁻⁴ and Ka of HCN = 4.9 × 10⁻¹⁰
1.92
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.375 M solution of HF? Ka of HF = 3.5 × 10⁻⁴
1.96
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.135 M NaCN solution? Ka of HCN = 4.9 × 10⁻¹⁰
11.20
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.150 M solution of NH₃? Kb of NH₃ = 1.76 × 10⁻⁵
11.210
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.145 M solution of (CH₃)₃N? Kb of (CH₃)₃N = 6.4 × 10⁻⁵
11.48
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.300 M solution of CH₃NH₂? Kb of CH₃NH₂ = 4.4 × 10⁻⁴
12.04
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.280 M solution of (CH₃)₂NH? Kb of (CH₃)₂NH = 5.4 × 10⁻⁴
12.08
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a solution that has 0.250 M HF and 0.250 M HClO? Ka of HF = 3.5 × 10⁻⁴ and Ka of HClO = 2.9 × 10⁻⁸
2.03
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a solution that has 0.200 M HF and 0.200 M HCN? Ka of HF = 3.5 × 10⁻⁴ and Ka of HCN = 4.9 × 10⁻¹⁰
2.08
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.145 M solution of a weak acid has a pH of 2.75. What is the value of Ka for the acid?
2.2 × 10⁻⁵
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.200 M solution of HCOOH? Ka of HCOOH = 1.8 × 10⁻⁴
2.22
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.200 M solution of a weak acid has a pH of 3.15. What is the value of Ka for the acid?
2.5 × 10⁻⁶
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.150 M solution of CH₃COOH? Ka of CH₃COOH = 1.8 × 10⁻⁵
2.78
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a solution that has 0.125 M CH₃COOH and 0.125 M H₃BO₃? Ka of CH₃COOH = 1.8 × 10⁻⁵ and Ka of H₃BO₃ = 5.4 × 10⁻¹⁰
2.82
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.200 M H2S solution? Ka₁ of H₂S = 8.9 × 10⁻⁸ and Ka₂ = 1 × 10⁻¹⁹
3.89
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.150 M NH₄Cl solution? Kb of NH₃ = 1.76 × 10⁻⁵
5.035
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.200 M solution of a weak acid has a pH of 2.50. What is the value of Ka for the acid?
5.1 × 10⁻⁵
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. A 0.165 M solution of a weak acid has a pH of 3.02. What is the value of Ka for the acid?
5.5 × 10⁻⁶
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.200 M CH₃NH₃Br solution? Kb of CH₃NH₂ = 4.4 × 10⁻⁴
5.68
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.225 M (CH₃₂NH₂Br solution? Kb of (CH₃)₂NH = 5.4 × 10⁻⁴
5.68
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.100 M NaClO₂ solution? Ka of HClO₂ = 1.1 × 10⁻²
7.48
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is a weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.225 M KNO₂ solution? Ka of HNO₂ = 4.6 × 10⁻⁴
8.34
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.350 M MgF₂ solution? Ka of HF = 3.5 × 10⁻⁴
8.65
A salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, the solution will be either acidic or basic. The pH of the solution can be determined using an ICE table with the equilibrium reaction for the reaction between the ion and water. What is the pH of a 0.200 M KC₇H₅O₂ solution? Ka of HC₇H₅O₂ = 6.5 × 10⁻⁵
8.74
Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. Ka is the equilibrium constant for the dissociation of a weak acid and Kb is the equilibrium constant for the dissociation of a weak base. What is the pH of a 0.175 M solution of C₅H₅N? Kb of C₅H₅N = 1.7 × 10⁻⁹
9.23
