A aqueous mixture is prepared by dissolving the following solutes at : • sodium…

CHEMISTRY · Multi-part · AP · Chemistry · Acids and Bases · Acids and Bases

Problem

A 1.00 L1.00\,\text{L} aqueous mixture is prepared by dissolving the following solutes at 25 ∘C25\,^{\circ}\text{C}: • 0.050 mol0.050\,\text{mol} sodium chloride, NaCl (strong electrolyte) • 0.050 mol0.050\,\text{mol} acetic acid, CH3_3COOH (weak electrolyte; Ka=1.8×10−5K_a = 1.8 \times 10^{-5}) • 0.050 mol0.050\,\text{mol} sucrose, C12_{12}H22_{22}O11_{11} (nonelectrolyte) No volume change occurs upon mixing. (a) Using principles of chemical equilibrium, determine the equilibrium molar concentration of hydronium ions produced by the ionization of acetic acid in the mixture. Clearly outline the setup and solution of the equilibrium expression. (b) Calculate the total molar concentration of mobile ions present in the mixture, accounting for contributions from all three solutes and the ionization of acetic acid. (c) Predict qualitatively how the electrical conductivity of this mixture compares with that of a 0.100 mol L−10.100\,\text{mol\,L}^{-1} NaCl solution. Justify your prediction using your result from part (b). (d) Sketch a labeled particulate diagram of a small representative region of the mixture. Include and distinguish among Na+^+, Cl−^-, CH3_3COO−^-, CH3_3COOH molecules, sucrose molecules, and water, showing appropriate orientations of water molecules around ions.

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