Two clear, colorless solutions are mixed in a beaker at . • Solution A: of • Solution…

CHEMISTRY · Multi-part · AP · Chemistry · Equilibrium · Equilibrium

Problem

Two clear, colorless solutions are mixed in a beaker at

25\,\circ\text{C}

. • Solution A:

50.0\,\text{mL}

0.010\,\text{M}

\mathrm{Ba(NO_3)_2}

• Solution B:

25.0\,\text{mL}

0.040\,\text{M}

\mathrm{Na_2SO_4}

The solubility-product constant for barium sulfate at

25\,\circ\text{C}

K_{sp}[\mathrm{BaSO_4}] = 1.1 \times 10^{-10}

. Assume volumes are additive. (1) Part 1: (a) Calculate the molar concentrations of

\mathrm{Ba^{2+}}

and

\mathrm{SO_4^{2-}}

ions in the mixture immediately after the two solutions are combined but before any precipitation occurs. (2) Part 2: (b) Determine the numerical value of the reaction quotient,

Q

, for the possible formation of

\mathrm{BaSO_4}

at the instant of mixing. (3) Part 3: (c) Using a comparison of

Q

and

K_{sp}

, state whether a precipitate of

\mathrm{BaSO_4}

will form. Justify your answer with reference to your calculated values. (4) Part 4: (d) If a precipitate does form, calculate the concentration of the ion present in excess once equilibrium is re-established. If no precipitate forms, explain why the initial ion concentrations remain unchanged.

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