Ionic Equilibrium
The solubility product (Ksp) of AgCl at 25°C is 1.8 × 10⁻¹⁰. The maximum concentration of Ag⁺ ions that can exist in a 0.01 M NaCl solution is:
Select the correct option:
🔒 Solution Hidden from View
Submit your answer to unlock the detailed step-by-step solution.
More equilibrium Practice Questions
The degree of dissociation of a 0.1 M weak monoprotic acid HA is 0.01. The dissociation constant Ka ...
The degree of dissociation of a 0.1 M weak monoprotic acid HA is 0.01. The dissociation constant Ka ...
The pH of a 0.01 M solution of HCl is:
The pH of a 0.01 M solution of HCl is:
At 700 K, 0.4 mol of H_2 and 0.4 mol of I_2 are placed in a 1 L flask. At equilibrium, the flask con...
At 700 K, 0.4 mol of H_2 and 0.4 mol of I_2 are placed in a 1 L flask. At equilibrium, the flask con...
For the reaction CO(g) + 3H_2(g) \rightleftharpoons CH_4(g) + H_2O(g), what will happen to the equil...
For the reaction CO(g) + 3H_2(g) \rightleftharpoons CH_4(g) + H_2O(g), what will happen to the equil...
At equilibrium, 20% of N_2O_4 is dissociated into NO_2 according to N_2O_4(g) \rightleftharpoons 2NO...
At equilibrium, 20% of N_2O_4 is dissociated into NO_2 according to N_2O_4(g) \rightleftharpoons 2NO...
At 25°C, the ionic product of water K_w = 1.0 \times 10^{-14}. What is the pOH of a solution whose [...
At 25°C, the ionic product of water K_w = 1.0 \times 10^{-14}. What is the pOH of a solution whose [...
For an endothermic reaction at 400 K, K_c = 2.0 \times 10^{-3}. When the temperature is raised to 60...
For an endothermic reaction at 400 K, K_c = 2.0 \times 10^{-3}. When the temperature is raised to 60...
The solubility of AgCl in 0.1 M NaCl solution is much lower than its solubility in pure water. If K_...
The solubility of AgCl in 0.1 M NaCl solution is much lower than its solubility in pure water. If K_...
In a closed vessel at 800 K, SO_3 partially dissociates: 2SO_3(g) \rightleftharpoons 2SO_2(g) + O_2(...
In a closed vessel at 800 K, SO_3 partially dissociates: 2SO_3(g) \rightleftharpoons 2SO_2(g) + O_2(...
According to the Lewis acid-base theory, which of the following species acts as a Lewis acid in the ...
According to the Lewis acid-base theory, which of the following species acts as a Lewis acid in the ...
Which of the following aqueous salt solutions will be basic (pH > 7) at 25°C due to hydrolysis of it...
Which of the following aqueous salt solutions will be basic (pH > 7) at 25°C due to hydrolysis of it...
In the reaction H_2O + NH_3 \rightleftharpoons OH^- + NH_4^+, which pair correctly identifies the co...
In the reaction H_2O + NH_3 \rightleftharpoons OH^- + NH_4^+, which pair correctly identifies the co...
About This Question
- Subject
- chemistry
- Chapter
- equilibrium
- Topic
- ionic equilibrium
- Difficulty
- Medium
- Year
- 2025
Solution
Correct Answer:
1.8 × 10⁻⁸ mol L⁻¹
For AgCl, Ksp = [Ag⁺][Cl⁻] = 1.8 × 10⁻¹⁰. In a 0.01 M NaCl solution, [Cl⁻] ≈ 0.01 M (since NaCl dissociates completely and the contribution from AgCl dissolution is negligible). Therefore, [Ag⁺] = Ksp/[Cl⁻] = 1.8 × 10⁻¹⁰ / 0.01 = 1.8 × 10⁻⁸ mol L⁻¹. This demonstrates the common ion effect: the presence of Cl⁻ from NaCl suppresses the dissolution of AgCl, drastically reducing the Ag⁺ concentration compared to dissolution in pure water where [Ag⁺] would be √(1.8 × 10⁻¹⁰) = 1.34 × 10⁻⁵ mol L⁻¹.
This medium difficulty chemistry question is from the chapter equilibrium, covering the topic of ionic equilibrium. It appeared in the 2025 exam.
Looking for more practice? Explore all chemistry questions or browse equilibrium questions on RankGuru.