Ksp of AgCl is 1 × 10–10. Its solubility in 0.1 M KNO3 will be :-10–5 moles/litre> 10–5 moles/litre< 10–5 moles/litreNone of these
Question
Ksp of AgCl is 1 × 10–10. Its solubility in 0.1 M KNO3 will be :-10–5 moles/litre> 10–5 moles/litre< 10–5 moles/litreNone of these
Solution
The solubility of AgCl in a solution of KNO3 is not affected by the presence of KNO3. This is because KNO3 is a salt of a strong acid (HNO3) and a strong base (KOH), and it does not react with AgCl.
The solubility product constant (Ksp) of AgCl is given as 1 × 10^-10. The dissolution of AgCl can be represented by the following equation:
AgCl(s) ⇌ Ag+(aq) + Cl-(aq)
Since AgCl is a sparingly soluble salt, we can assume that its solubility is 's'. Therefore, the concentrations of Ag+ and Cl- ions in the solution are both 's'.
According to the definition of Ksp, we have:
Ksp = [Ag+][Cl-] = s^2
Substituting the given value of Ksp into this equation, we get:
1 × 10^-10 = s^2
Solving for 's', we get:
s = sqrt(1 × 10^-10) = 1 × 10^-5 moles/litre
Therefore, the solubility of AgCl in 0.1 M KNO3 is 1 × 10^-5 moles/litre. So, the answer is "= 10^-5 moles/litre".
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