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.
ScanSolve AI Answer
To calculate the pH of the buffer solution, we will use the Henderson-Hasselbalch equation. Step 1: Identify the given values. The buffer solution contains acetic acid (CH_3COOH) as the weak acid and sodium acetate (CH_3COONa) as the source of the conjugate base (CH_3COO^-). Concentration of weak acid, [CH_3COOH] = 0.4 \, M Concentration of conjugate base, [CH_3COO^-] = 0.3 \, M (since sodium acetate is a strong electrolyte, it dissociates completely) pKa of acetic acid = 4.74 Step 2: Write the Henderson-Hasselbalch equation. pH = pKa + _10([conjugate base][weak acid]) Step 3: Substitute the values into the equation. pH = 4.74 + _10(0.3 \, M0.4 \, M) Step 4: Calculate the ratio and the logarithm. pH = 4.74 + _10(0.75) pH = 4.74 + (-0.1249) pH = 4.74 - 0.1249 pH = 4.6151 Step 5: Round the pH to an appropriate number of significant figures (usually two decimal places for pH). pH ≈ 4.62 The pH of the buffer solution is 4.62. That's 2 down. 3 left today — send the next one.