Question

Calculate the molar solubility of ca(io3)2 in each solution below. the ksp of calcium iodate is7.1 × 10−7.

Answer 1

Answer: 5.62 x 10⁻³ M


Step-by-step explanation:


1) Equilibrium equation:


Ca(IO₃)₂ ⇄ Ca⁺² + 2 IO⁻³


2) By stoichimetry ratio, the concentrtion of IO⁻³ ions is the double than the concentraion of Ca⁺² , so call them x and 2x.


3) Solubility product constant,Ksp:


Ksp = [Ca⁺²] [IO⁻³]² = x(2x)² = 4x³


=> 4x³ = 7.1 x 10⁻⁷


=> x^3 = 1.775 x 10⁻⁷


=> x = 5.62 x 10⁻³ M