Calculate the pH of a solution that is 2.00 M HF,1.00 M NaOH,and 0.546 M NaF.(K_a = 6.8 × 10^-4) A)3.36 B)2.98 C)3.17 D)2.60 E)none of these

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The solution contains HF, NaOH, and NaF. NaOH will react with HF to form NaF and water. The reaction is: HF + NaOH → NaF + H2O. Initially, there are 2.00 M HF and 1.00 M NaOH. After the reaction, 1.00 M HF will remain, and the concentration of NaF will be 1.546 M (0.546 M initial NaF + 1.00 M from the reaction). The pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where pKa = -log(Ka) = 3.17. Substituting the values, pH = 3.17 + log(1.546/1.00) = 3.36.

Calculate the PH of a Solution That Is 2