Calculate The Solubility of Agcl in 0.10 M Nacl
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When silver chloride (AgCl) is added to a solution containing sodium chloride (NaCl), the solubility of AgCl decreases due to the common ion effect. This calculator helps determine the new solubility of AgCl in a 0.10 M NaCl solution.
Introduction
Silver chloride (AgCl) is a sparingly soluble salt with a solubility product constant (Ksp) of 1.8 × 10−10 at 25°C. When NaCl is added to a solution containing AgCl, the chloride ions (Cl−) from NaCl combine with the silver ions (Ag+) from AgCl, reducing the concentration of Ag+ and thus decreasing the solubility of AgCl.
The common ion effect occurs when a common ion is added to a solution of a sparingly soluble salt. This reduces the solubility of the salt because the ion product exceeds the solubility product.
The Common Ion Effect
The common ion effect is a fundamental concept in chemistry that explains how the solubility of a sparingly soluble salt is reduced when a common ion is added to the solution. In the case of AgCl and NaCl:
- AgCl dissociates in water: AgCl(s) ⇌ Ag+(aq) + Cl−(aq)
- NaCl dissociates in water: NaCl(s) ⇌ Na+(aq) + Cl−(aq)
The added Cl− ions from NaCl combine with Ag+ ions, reducing the concentration of Ag+ and thus decreasing the solubility of AgCl.
Calculation Method
The solubility of AgCl in the presence of NaCl can be calculated using the following steps:
- Determine the initial solubility of AgCl in pure water (S0):
S0 = √(Ksp) = √(1.8 × 10−10) ≈ 1.34 × 10−5 M
- Calculate the new solubility (S) in the presence of NaCl:
S = S0 / √(1 + [Cl−]initial / S0)
Where [Cl−]initial is the initial concentration of Cl− from NaCl.
Example Calculation
Let's calculate the solubility of AgCl in a 0.10 M NaCl solution:
- Initial solubility of AgCl: S0 ≈ 1.34 × 10−5 M
- Initial Cl− concentration from NaCl: [Cl−]initial = 0.10 M
- Calculate the new solubility:
S = (1.34 × 10−5) / √(1 + 0.10 / 1.34 × 10−5) ≈ 1.34 × 10−5 / √(1 + 74538) ≈ 1.34 × 10−5 / 273 ≈ 4.91 × 10−8 M
The solubility of AgCl decreases from approximately 1.34 × 10−5 M in pure water to about 4.91 × 10−8 M in a 0.10 M NaCl solution.
Practical Applications
Understanding the common ion effect is important in various practical applications, including:
- Water treatment: Controlling the precipitation of metal hydroxides
- Analytical chemistry: Selective precipitation techniques
- Environmental science: Assessing the impact of dissolved salts on mineral solubility
The common ion effect is also crucial in understanding the behavior of biological systems where ions play a significant role.
Frequently Asked Questions
What is the common ion effect?
The common ion effect is the decrease in solubility of a sparingly soluble salt when a common ion is added to the solution. This occurs because the ion product exceeds the solubility product.
How does NaCl affect the solubility of AgCl?
NaCl provides additional Cl− ions to the solution, which combine with Ag+ ions from AgCl, reducing the concentration of Ag+ and thus decreasing the solubility of AgCl.
What is the Ksp of AgCl?
The solubility product constant (Ksp) of AgCl is 1.8 × 10−10 at 25°C.
How is the solubility of AgCl calculated in the presence of NaCl?
The solubility is calculated using the formula: S = S0 / √(1 + [Cl−]initial / S0), where S0 is the initial solubility of AgCl in pure water.