For this problem, we’re being asked to calculate the solubility in mole/liter for copper(II) sulfide at 25 °C given a Ksp value of 1.3 x 10-36
Since the copper(II) sulfide (CuS) is an ionic compound, it forms ions when dissociating in water. The dissociation of CuS in water is as follows:
The hydroxide ion, OH–, has a charge of –1. Nickel then has a charge of +2:
CuS(s) ⇌ Cu2+(aq) + S2-(aq)
We can construct an ICE table for the dissociation of CuS.
Remember that solids are ignored in the ICE table and Ksp expression.
What is the solubility in mole/liter for copper(II) sulfide at 25 °C given a Ksp value of 1.3 x 10-36. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!)
Frequently Asked Questions