# Problem: The Ksp of AgCl is 1.6 x 10-10. What is the solubility of AgCl in 0.0010 M MgCl2? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).

###### FREE Expert Solution

For this problem, we’re being asked to calculate the solubility (in g/L) of AgCl(s) in 0.0010 M MgCl2(aq). Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of AgCl and MgCl2 in water are as follows:

The chloride ion, Cl, has a charge of –1. Ag has a charge is +1:

AgCl(s)  Ag+(aq) + Cl(aq)

The chloride ion, Cl, has a charge of –1. Mg has a charge is +2:

MgCl2(s)  Mg2+(aq) + 2 Cl(aq)

Calculate the molarity of Cl-:

= 0.0020 M Cl-

Notice that there is a common ion present, Cl. The common ion effect states that the solubility of a salt is lower in the presence of a common ion. ###### Problem Details

The Ksp of AgCl is 1.6 x 10-10. What is the solubility of AgCl in 0.0010 M MgCl2? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).