Chemistry 10th Edition

(a) $[Sr^{2+}] = 0.0105M, [OH^-] = 0.0210M$ (b) $[H^+] = [ClO^{3-}] = 0.0105M$ (c) $[K^+] = 0.0210M, [S{O_4}^{2-}] = 0.0105M$
Strong electrolytes, like strong acids and bases, and salts, are capable of ionizating completely in water, therefore: - $[AB] = [A^+] = [B^-]$ Because the reaction: - $AB (aq) -- \gt A^+(aq) + B^-(aq)$ Occurs for all the compound molecules. For $Sr(OH)_2$, since there is 2 $OH^-:$ - $Sr(OH)_2(aq) -- \gt Sr^{2+}(aq) + 2OH^-(aq)$ The "$OH^-$" concentration will be the double of the base concentration. 2 * 0.0105 = 0.0210M The same thing for $K_2SO_4$ 2 * 0.0105 = 0.0210