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Chapter 15: Q40 E (page 873)

A volume of 0.800 L of a 2×10-4-MBa(NO3)2 solution is added to 5×10-4 MLi2 SO4. Does BaSO4 precipitate? Explain your answer.

Short Answer

Expert verified

Ki is smaller than Ksp for BaSO4, no precipitation of BaSO4 will occur

Step by step solution

01

Define Precipitate

Precipitation occurs when ionic product is greater than a solubility product of a substance.

02

Calculating the concentration of barium ions

Substituting the formula in c2

\({c_2}=\frac{{{c_1}{V_1}}}{{{V_2}}}=\frac{{2 \times 1{0^{-4}}\times 0.8L}}{{1L}}=1.6\times1{0^{-4}}\)

\(\left( {B{a^{2+}}}\right)=1.6\times1{0^{-4}}\)

\({c_2}=\frac{{{c_1}{V_1}}}{{{V_2}}}=\frac{{5\times1{0^{-4}}\times0.2L}}{{1L}}=1\times1{0^{-4}}\)

\(\left({SO_4^{2-}}\right)=1\times1{0^{-4}}\)

03

Determining ionic product

\({K_i}=\left({B{a^{2+}}}\right)\left({SO_4^{2-}}\right)\)

\({K_i}=1.6\times1{0^{-8}}\)

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Most popular questions from this chapter

Question: 28. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate \({K_{sp}}\)for each of the slightly soluble solids indicated:

(a) \(AgBr:\left( {A{g^ + }} \right) = 5.7 \times 1{0^{ - 7}}M,\left( {B{r^ - }} \right) = 5.7 \times 1{0^{ - 7}}M\)

(b) \(CaC{O_3}:\left( {C{a^{2 + }}} \right) = 5.3 \times 1{0^{ - 3}}M,\left( {C{O_3}^{2 - }} \right) = 9.0 \times 1{0^{ - 7}}M\)

(c) \(Pb{F_2}:\left( {P{b^{2 + }}} \right) = 2.1 \times 1{0^{ - 3}}M,\left( {{F^ - }} \right) = 4.2 \times 1{0^{ - 3}}M\)

(d) \(A{g_2}Cr{O_4}:\left( {A{g^ + }} \right) = 5.3 \times 1{0^{ - 5}}M,3.2 \times 1{0^{ - 3}}M\)

(e) \(In{F_3}:\left( {I{n^{3 + }}} \right) = 2.3 \times 1{0^{ - 3}}M,\left( {{F^ - }} \right) = 7.0 \times 1{0^{ - 3}}M\)

Question: How many grams of \(Pb{(OH)_2}\)will dissolve in 500 mL of a \(0.050 - MPbC{l_2}\;solution\;\left( {{K_{sp}} = 1.2 \times 1{0^{ - 15}}} \right)?\)

The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem:

MgF2 (S) ⇌ Mg2+(aq) + 2F- (aq)

In a saturated solution of MgF2 at 18 °C, the concentration ofMg2+is 1.21×10-3 M.

The equilibrium is represented by the preceding equation.

(a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 °C.

(b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2solution at 18 °C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible.

(c) Predict whether a precipitate of MgF­2 will form whensolution of 100.0mL of a 3.00 ×10-3 -M Mg(NO3)2 is mixed with 200.0 mL of a 2.00 × 10–3 -M solution of NaF at 18 °C. Show the calculations to support your prediction.

(d) At 27 °C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17×10-3 M. Is the dissolving of MgF2 in water an endothermic or an exothermic process? Give an explanation to support your conclusion.

Magnesium hydroxide and magnesium citrate function as mild laxatives when they reach the small intestine. Why do magnesium hydroxide and magnesium citrate, two very different substances, have the same effect in your small intestine. (Hint: The contents of the small intestine are basic.)

Iron concentrations greater than 5.4×10-6M in water used for laundrypurposes can cause staining. What [OH-] is required to reduce [Fe2+] to this level by precipitation of Fe(OH)2?
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