What is the pH of a solution made by combining 134 mL of 0.26 M NaC₂H₃O₂ with 211 mL of 0.31 M HC₂H₃O₂? The K_a of acetic acid is 1.75 × 10^-5. A) 4.47 B) 5.04 C) 5.52 D) 4.42 E) 4.97

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Quizplus · Accepted Answer

The correct answer is A because the pH of the solution is 4.47. The reaction between NaC2H3O2 and HC2H3O2 is a neutralization reaction, which produces NaCl and HC2H3O2. The concentration of HC2H3O2 in the final solution can be calculated using the following equation:[HC2H3O2] = (0.26 M * 134 mL + 0.31 M * 211 mL) / (134 mL + 211 mL) = 0.28 MThe pH of the solution can then be calculated using the following equation:pH = -log[H+]= -log(Ka * [HC2H3O2] / [C2H3O2-])pH = -log(1.75 * 10^-5 * 0.28 / 0.26) = 4.47

What Is the PH of a Solution Made by Combining