Calculate the molar solubility of MX (Ksp = 1.27 × 10^-36) in pure water.

Verified step by step guidance

1. Identify the dissociation equation for the salt MX: MX(s) \rightleftharpoons M^+(aq) + X^-(aq).
2. Write the expression for the solubility product constant (K_{sp}): K_{sp} = [M^+][X^-].
3. Assume the molar solubility of MX is 's'. Therefore, [M^+] = s and [X^-] = s.
4. Substitute the concentrations into the K_{sp} expression: K_{sp} = s \times s = s^2.
5. Solve for 's' by taking the square root of both sides: s = \sqrt{K_{sp}}.