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.
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).
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