The molar solubility of AgCl in 6.5 * 10^-3 M AgNO3 is 2.5 * 10^-8M. In deriving

Question

The molar solubility of AgCl in 6.5 * 10^-3 M AgNO3 is 2.5 * 10^-8M. In deriving Ksp from these data, which of the following assumptions is (are) reasonable?

A. Ksp is he same solubility.

B. Ksp of AgCl is the same in 2.5 * 10^-8M AgNO as in pure water.

C. Solubility of AgC; is independent of the concentration of AgNO3.

D. Ag+ does not change significantly upon addition of AgCl to 6.5 * 10*-3M AgNO3

E. Ag+ after the addition of AgCl to 6.5 *10^-3M AgNO3 is the same as it would be in pure water

Please explain why you chose your answer, Thanks!

Explanation / Answer

B is the correct answer.

It's important to remember that Ksp (equilibrium constant) is exactly that - a constant. Only a changing temperature can influence that number for a given compound.

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