Question

determine the value of ksp for cu(io₃)₂ by constructing an ice table, writing the solubility constant expression, and solving the expression. the molar solubility of cu(io₃)₂ is 2.7×10⁻³ m at this temperature. complete parts 1 - 2 before submitting your answer. using the values from the ice table, construct the expression for the solubility constant. each reaction participant must be represented by one tile. do not combine terms once the expression is constructed, solve for ksp. ksp = =

Explanation:

Step1: Write the dissolution equation

$$\ce{Cu(IO3)2(s) <=> Cu^{2 + }(aq) + 2IO3^{-}(aq)}$$
Let the molar solubility of $\ce{Cu(IO3)2}$ be $s$. Then $[\ce{Cu^{2+}}]=s$ and $[\ce{IO3^{-}}]=2s$.

Step2: Construct the solubility - constant expression

The solubility - constant expression $K_{sp}=[\ce{Cu^{2+}}][\ce{IO3^{-}}]^2$. Substituting $[\ce{Cu^{2+}}]=s = 2.7\times10^{-3}\ M$ and $[\ce{IO3^{-}}]=2s$ into the expression:
$$K_{sp}=(s)\times(2s)^2$$
$$K_{sp}=4s^{3}$$

Step3: Calculate the value of $K_{sp}$

Substitute $s = 2.7\times10^{-3}\ M$ into the $K_{sp}$ formula:
$$K_{sp}=4\times(2.7\times 10^{-3})^{3}$$
First, calculate $(2.7\times 10^{-3})^{3}=2.7^{3}\times10^{-9}=19.683\times10^{-9}$
Then, $K_{sp}=4\times19.683\times10^{-9}=7.8732\times10^{-8}\approx7.9\times10^{-8}$

Answer:

$K_{sp}=\frac{[2.7\times 10^{-3}][5.4\times 10^{-3}]^{2}}{[0]} = 7.9\times 10^{-8}$