Using concentrations, the solubility of [Ag+] in a solution of 0.01 M KCl is 1.8

Question

Using concentrations, the solubility of [Ag+] in a solution of 0.01 M KCl is 1.8 * 10-8. Calculate the percent relative error when using concentrations for the solubility of [Ag+] compared to activities.

Explanation / Answer

Suppose Ag2C2O4 is soluble so, Ag2C2O4 (s) ------> 2Ag+(aq) + C2O42-(aq) Then Ksp = [Ag+]2*[C2O42-(aq)] where [Ag2C2O4] and is given activity of 1. Technically speaking, we shouldn't be using concentration, activity is an effective concentration, ie activity = constant x molarity(also known as concentration) So activity of pure components is always 1, that is why we omit the [original solid] So, you can hopefully see that the ratio of the Ag+ : ethane-dioate is 2:1, so as they are in the same volume, the no of mol must be in that same ratio, and so the activity(concentration) should be the same ratio too. So, knowing one of the activity(or effective concentration), you can determine the other ones and from there you can get Ksp.

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