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
Step 1: Calculate the pK_a of acetic acid (CH_3CO_2H). The acid dissociation constant (K_a) for CH_3CO_2H is given as 1.76 × 10^-5. pK_a = -_10(K_a) pK_a = -_10(1.76 × 10^-5) pK_a ≈ 4.754 Step 2: Use the Henderson-Hasselbalch equation to calculate the pH. The Henderson-Hasselbalch equation is: pH = pK_a + _10([A^-][HA]) We are given: [HA] = [CH_3CO_2H] = 0.25 M [A^-] = [CH_3CO_2^-] = 0.45 M pK_a = 4.754 Substitute these values into the equation: pH = 4.754 + _10(0.45 M0.25 M) pH = 4.754 + _10(1.8) pH = 4.754 + 0.255 pH = 5.009 Rounding to a reasonable number of significant figures (e.g., two decimal places for pH), the pH is 5.01. If rounded to the nearest whole number as shown in the provided solution, it is 5. The final answer is 5.01. Got more? Send 'em!