This question is about the properties and reactions of butanoic acid, C3H7COOHC_3H_7COOHC3H7COOH. Butanoic acid is a weak acid with an acid dissociation constant, KaK_aKa, of 1.52×10−5 mol dm−31.52 \times 10^{-5} \text{ mol dm}^{-3}1.52×10−5 mol dm−3 at 25∘C25^\circ\text{C}25∘C.
A student uses a pH meter to measure the pH of a solution of C3H7COOHC_3H_7COOHC3H7COOH at 25∘C25^\circ\text{C}25∘C. The measured pH is 2.7102.7102.710. Calculate the concentration of butanoic acid in the solution. Give your answer to three significant figures.
Butanoic acid is added to another weak acid, hydrofluoric acid, HFHFHF (Ka=6.80×10−4 mol dm−3K_a = 6.80 \times 10^{-4} \text{ mol dm}^{-3}Ka=6.80×10−4 mol dm−3). An equilibrium is set up containing two acid-base pairs. Write the equilibrium equation and identify the conjugate acid-base pairs as A1, B1 and A2, B2.
The student plans to prepare a buffer solution that has a pH of 4.704.704.70. The buffer solution will contain butanoic acid, C3H7COOHC_3H_7COOHC3H7COOH, and sodium butanoate, C3H7COONaC_3H_7COONaC3H7COONa. The student plans to add 8.38 g8.38\text{ g}8.38 g C3H7COONaC_3H_7COONaC3H7COONa to 250 cm3250\text{ cm}^3250 cm3 of 0.400 mol dm−30.400\text{ mol dm}^{-3}0.400 mol dm−3 C3H7COOHC_3H_7COOHC3H7COOH. The student assumes that the volume of the solution does not change.
Show by calculation whether, or not, the student's experimental method would produce the required pH of 4.704.704.70. Show all your working.
When the student prepares the buffer solution, the volume of solution increases slightly. Suggest whether the pH of the buffer solution would be the same, greater than, or less than your calculated value. Explain your reasoning.
