For this problem, we’re being asked to calculate the molar solubility of Ag2CrO4 .
Since the Ni(OH)2 is an ionic compound, it forms ions when dissociating in water. The dissociation of Ni(OH)2 in water is as follows:
The hydroxide ion, OH–, has a charge of –1. Nickel then has a charge of +2:
Ag2CrO4 (s) ⇌ 2 Ag+(aq) + CrO42-(aq) Ksp = 1.12×10−12
We can construct an ICE table for the dissociation of Ag2CrO4.
Remember that solids are ignored in the ICE table and Ksp expression.
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.
Ag2CrO4 Ksp = 1.12×10−12)
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