Question

Be sure to answer all parts. Calculate K at 298 K for the

following reaction: SrSO₄(s) ? Sr₂+(aq) + SO₄₂?(aq) (Enter your
answer in scientific notation.) No other data is given in the
equation

Answer 1

The equilibrium constant (K) for the dissolution of strontium sulfate (SrSO4) at 298 K is the solubility product constant (Ksp), which is 2.8 × 10⁻⁷.

Step-by-step explanation:

To calculate the equilibrium constant (K) for the dissolution of strontium sulfate (SrSO4) at 298 K, we would use its solubility product constant (Ksp), which is a special type of equilibrium constant for substances dissolving in water. The dissolution reaction is given by:

SrSO4(s) ⇌ Sr2+(aq) + SO42−(aq)

The equilibrium expression for this reaction would be:

Ksp = [Sr2+][SO42−]

For this reaction, the Ksp value at 298 K is given as 2.8 × 10−7. Therefore, this is the value of K for the dissolution of SrSO4 in water at 298 K under standard conditions.