Solubility

We are given the solubility product of Cu(OH)₂, , and the concentration of Cu²⁺ in solution from CuCl₂, which is . The solubility of Cu(OH)₂ in this solution is determined by calculating the concentration of hydroxide ions from the given . For the reaction: At equilibrium, the concentration of Cu²⁺ is , and the concentration of OH⁻ is derived using . The correct solubility can be calculated by applying the relation: Solving for the concentration of OH⁻ gives us the correct answer. The result matches .

The elevation in boiling point is given by the formula: Where:

• is the van't Hoff factor. For KCl, (dissociates into K and Cl ).

Substitute the values: Boiling point of the solution:

To check for precipitation: Since both solutions are mixed 1:1, each ion's concentration is halved. For (iv), , Other options yield , hence no precipitation.

For a cubic close-packed (ccp/fcc) structure, the number of atoms per unit cell = 4.
Density formula: Given: Solving for : Convert to Å using :