## Chemistry 10th Edition

(a) $[H^+] = [Br^-] = 0.45M$ (b) $[K^+] = [OH^-] = 0.045M$ (c) $[Ca^{2+}] = 0.0112M$, and $[Cl^-] = 0.0224M$
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. For $CaCl_2$, since there is 2 $Cl^-:$ - $CaCl_2 (aq) -- \gt Ca^{2+}(aq) + 2Cl^-(aq)$ The "$Cl^-$" concentration will be the double of the salt concentration. 2 * 0.0112 = 0.0224