A saturated solution of magnesium hydroxide, Mg(OH)₂, in pure water has a pH of 10.50 at 298 K. All the hydroxide ions come from the dissolved solid. What is the solubility product of magnesium hydroxide at 298 K? Take Kw = 1.0 × 10⁻¹⁴ and 10^(0.5) = 3.16.

ChemistryMediumHigh School (11–12)Acids, Bases and Salts › Salts and Their Uses JEE Main

A saturated solution of magnesium hydroxide, $\text{Mg(OH)}_2$ , in pure water has a pH of $10.50$ at $298\ \text{K}$ . All the hydroxide ions come from the dissolved solid. What is the solubility product of magnesium hydroxide at $298\ \text{K}$ ? Take $K_w = 1.0 \times 10^{-14}$ and $10^{0.5} = 3.16$ .

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← A student has 40.0 mL of 0.0250 mol L⁻¹ sulfuric acid, which gives both of its protons fully in water. What volume of 0.0500 mol L⁻¹ sodium hydroxide must be added to make the pH of the mixture exactly 12.00 at 298 K, in mL? Assume that the volumes add, and take Kw = 1.0 × 10⁻¹⁴.For N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), Kc = 0.50 L² mol⁻² at a certain temperature. A 2.00 L vessel at that temperature holds 1.00 mol of N₂, 2.00 mol of H₂ and 0.400 mol of NH₃. Which statement about this mixture is correct? →

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