Calculate solubility products (Ksp) and the concentrations of ions in aqueous solutions. (Formula: 𝐾sp = [C]c[D]d for the reaction aA(s) ⇋ cC(aq) + dD(aq))

Silver bromide, $AgBr$, dissolves in water according to the equilibrium: $$AgBr(s) \rightleftharpoons Ag^{+}(aq) + Br^{-}(aq)$$ The solubility of silver bromide in water at $298 \text{ K}$ is $7.3 \times 10^{-7} \text{ mol/L}$. Which of the following is the solubility product constant, $K_{sp}$, for silver bromide?

A saturated aqueous solution of barium sulfate, $\ce{BaSO4}(s)$, is prepared at 25 °C. The concentration of sulfate ions, $[\ce{SO4^{2-}}]$, at equilibrium is $1.05 \times 10^{-5}$ mol L$^{-1}$. Calculate the solubility product constant, $K_{sp}$, for barium sulfate. Show your working.

Silver bromide, AgBr, is a sparingly soluble salt. At 298 K, the solubility product constant for AgBr is $K_{sp} = 5.0 \times 10^{-13}$. Calculate the concentration of bromide ions, $[\text{Br}^{-}]$, in a saturated solution of silver bromide. Show your working.