In this lesson you will learn about how slightly soluble ionic compounds establish equilibrium as well as how to predict the formation of a precipitate when a slightly soluble salt is added to water or to a solution with a common ion.
By the end of this lesson, students should be able to:
- define ion product quotient, Qsp, and solubility product constant, Ksp.
- write balanced equation for the solubility equilibria of slightly soluble salts
- write both Qsp and Ksp expressions and calculate their values using molar solubility data.
- calculate molar solubility (in mol/L) of slightly soluble salts using their Ksp value and ICE tables (systematic problem solving approach)
- identify and rank slight soluble salts that produce the same number of ions or different number of ions.
- predict if a precipitate of a soluble salt forms by comparing Qsp and Ksp values.
- explain the common ion effect using your own words.
- solve solubility equilibria problems that involve the presence of a common ion using a systematic problem solving approach – stepwise.
Let’s start by examining the equilibrium process of slightly soluble salts. Please watch video lesson below and take notes.
Next, let’s examine how the presence of a common ion between a slight soluble salt solid and an aqueous solutions can affect the solubility of a slightly soluble salt. For the video lesson below, you should take clear notes and focus on the problem solving strategy shown in the lesson below.
To help you sharpen your problem solving skills, below is a worksheet on solubility equilibria. Please answer all problems on a separate sheet of paper and compare your answers against the answer key included at the end of the document.