This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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To solve pH and pOH questions without a log table, we typically work with concentrations that are exact powers of 10. This simplifies the logarithm calculation. The key formulas are: • pH = -[H^+] • pOH = -[OH^-] • pH + pOH = 14 (at 25^) • [H^+][OH^-] = 1.0 × 10^-14 (at 25^) When the concentration of H^+ or OH^- ions is in the form 1.0 × 10^-x M, then (1.0 × 10^-x) = -x. Example 1: Calculating pH from [H^+] What is the pH of a solution where the hydrogen ion concentration, [H^+], is 1.0 × 10^-4 M? Step 1: Use the pH formula. pH = -[H^+] Step 2: Substitute the given concentration. pH = -(1.0 × 10^-4) Step 3: Simplify the logarithm. Since (10^-4) = -4. pH = -(-4) pH = 4 The pH of the solution is 4. Example 2: Calculating pOH from [OH^-] What is the pOH of a solution where the hydroxide ion concentration, [OH^-], is 1.0 × 10^-2 M? Step 1: Use the pOH formula. pOH = -[OH^-] Step 2: Substitute the given concentration. pOH = -(1.0 × 10^-2) Step 3: Simplify the logarithm. Since (10^-2) = -2. pOH = -(-2) pOH = 2 The pOH of the solution is 2. Example 3: Calculating pH from pOH (or vice versa) If the pOH of a solution is 3, what is its pH? Step 1: Use the relationship between pH and pOH. pH + pOH = 14 Step 2: Substitute the given pOH value. pH + 3 = 14 Step 3: Solve for pH. pH = 14 - 3 pH = 11 The pH of the solution is 11.