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Solubility product of AgCl is 2.8 × 10-10 at 25ºC. Calculate solubility of the salt in 0.1 M AgNO3 solution -
- a)2.8 × 10-9 mole/litre
- b)2.8 × 10-10 mole/litre
- c)3.2 × 10-9 mole/litre
- d)3.2 × 10-12 mole/litre
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Solubility product of AgCl is 2.8 × 10-10at 25ºC. Calculate ...
Ksp(AgCl) = 2.8 × 10–10
2.8 × 10–10 = (s + 0.1)s
s = 2.8 × 10–9
2.8 × 10–10 = (s + 0.1)s
s = 2.8 × 10–9
Most Upvoted Answer
Solubility product of AgCl is 2.8 × 10-10at 25ºC. Calculate ...
Solubility Product of AgCl
The solubility product (Ksp) is a measure of the extent to which a sparingly soluble salt dissolves in water. It is defined as the product of the concentrations of the ions in a saturated solution of the salt.
The solubility product of AgCl can be represented by the equation:
AgCl(s) ⇌ Ag+(aq) + Cl-(aq)
The equilibrium expression for this reaction is:
Ksp = [Ag+][Cl-]
Given that the solubility product of AgCl is 2.8 × 10^-10 at 25°C, we can write the equation as:
2.8 × 10^-10 = [Ag+][Cl-]
Solubility of AgCl in 0.1 M AgNO3 Solution
When AgCl is dissolved in AgNO3 solution, the Ag+ ions from AgNO3 will combine with the Cl- ions from AgCl to form AgCl(s). This will result in a decrease in the concentration of Cl- ions in the solution.
To calculate the solubility of AgCl in 0.1 M AgNO3 solution, we need to consider the common ion effect. The presence of Ag+ ions from AgNO3 will shift the equilibrium of the AgCl dissociation reaction to the left, reducing the solubility of AgCl.
To find the solubility of AgCl, we can assume that x moles of AgCl dissolve, resulting in x moles of Ag+ and x moles of Cl- ions in the solution. Since AgNO3 is a strong electrolyte, it completely dissociates into Ag+ and NO3- ions.
Therefore, the concentration of Ag+ ions in the solution will be 0.1 M, and the concentration of Cl- ions will be x M.
Using the equilibrium expression for AgCl:
Ksp = [Ag+][Cl-]
Substituting the known values:
2.8 × 10^-10 = (0.1)(x)
Solving for x:
x = (2.8 × 10^-10) / 0.1
x ≈ 2.8 × 10^-9 mole/litre
Thus, the solubility of AgCl in 0.1 M AgNO3 solution is approximately 2.8 × 10^-9 mole/litre.
Therefore, the correct answer is option 'A'.
The solubility product (Ksp) is a measure of the extent to which a sparingly soluble salt dissolves in water. It is defined as the product of the concentrations of the ions in a saturated solution of the salt.
The solubility product of AgCl can be represented by the equation:
AgCl(s) ⇌ Ag+(aq) + Cl-(aq)
The equilibrium expression for this reaction is:
Ksp = [Ag+][Cl-]
Given that the solubility product of AgCl is 2.8 × 10^-10 at 25°C, we can write the equation as:
2.8 × 10^-10 = [Ag+][Cl-]
Solubility of AgCl in 0.1 M AgNO3 Solution
When AgCl is dissolved in AgNO3 solution, the Ag+ ions from AgNO3 will combine with the Cl- ions from AgCl to form AgCl(s). This will result in a decrease in the concentration of Cl- ions in the solution.
To calculate the solubility of AgCl in 0.1 M AgNO3 solution, we need to consider the common ion effect. The presence of Ag+ ions from AgNO3 will shift the equilibrium of the AgCl dissociation reaction to the left, reducing the solubility of AgCl.
To find the solubility of AgCl, we can assume that x moles of AgCl dissolve, resulting in x moles of Ag+ and x moles of Cl- ions in the solution. Since AgNO3 is a strong electrolyte, it completely dissociates into Ag+ and NO3- ions.
Therefore, the concentration of Ag+ ions in the solution will be 0.1 M, and the concentration of Cl- ions will be x M.
Using the equilibrium expression for AgCl:
Ksp = [Ag+][Cl-]
Substituting the known values:
2.8 × 10^-10 = (0.1)(x)
Solving for x:
x = (2.8 × 10^-10) / 0.1
x ≈ 2.8 × 10^-9 mole/litre
Thus, the solubility of AgCl in 0.1 M AgNO3 solution is approximately 2.8 × 10^-9 mole/litre.
Therefore, the correct answer is option 'A'.
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Solubility product of AgCl is 2.8 × 10-10at 25ºC. Calculate solubility of the salt in 0.1 M AgNO3solution -a)2.8 × 10-9mole/litreb)2.8 × 10-10mole/litrec)3.2 × 10-9mole/litred)3.2 × 10-12mole/litreCorrect answer is option 'A'. Can you explain this answer?
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