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Chapter 15: Q53E (page 875)

Question: Perform the following calculations involving concentrations of iodate ions:

(a) The iodate ion concentration of a saturated solution of \(La{\left( {I{O_3}} \right)_3}\)was found to be\(3.1 \times 1{0^{ - 3}}mol/L\). Find the\({K_{sp}}\).

(b) Find the concentration of iodate ions in a saturated solution of \(Cu{\left( {I{O_3}} \right)_2}\left( {{K_{5p}} = 7.4 \times 1{0^{ - 8}}} \right)\).

Short Answer

Expert verified

(a).\({K_{sp}} = 3.0 \times {10^{ - 11}}\)

(b). The concentration of iodate ions is \(\begin{array}{l}\left( {C{u^{2 + }}} \right) = 2.64 \times {10^{ - 3}}{\rm{M}};\\\left( {IO_3^ - } \right) = 5.3 \times {10^{ - 3}}{\rm{M}}\end{array}\)

Step by step solution

01

Find \({K_{sp}}\).:

\(\begin{array}{l}{K_{sp}} = \left( {L{a^{3 + }}} \right){\left( {IO_3^ - } \right)^3}\\ = \left( {\frac{1}{3} \times 3.1 \times {{10}^{ - 3}}} \right){\left( {3.1 \times {{10}^{ - 3}}} \right)^3}\\ = 3.0 \times {10^{ - 11}}\end{array}\)

02

Find the concentration of iodate ions:

\(\begin{array}{l}{K_{sp}} = \left( {C{u^{2 + }}} \right){\left( {IO_3^ - } \right)^2}\\ = x{(2x)^2}\\ = 7.4 \times {10^{ - 8}}\end{array}\)

Where x,

\(\begin{array}{l}x = \sqrt(3){{\frac{{7.4 \times {{10}^{ - 8}}}}{4}}}\\ = 2.64 \times {10^{ - 3}}\end{array}\)

\(\left( {C{u^{2 + }}} \right) = 2.64 \times {10^{ - 3}}M\)

\(\begin{array}{l}\left( {IO_3^ - } \right) = 2 \times 2.64 \times {10^{ - 3}}\\ = 5.3 \times {10^{ - 3}}{\rm{M}}\end{array}\)

The solutions are \(\begin{array}{l}\left( {C{u^{2 + }}} \right) = 2.64 \times {10^{ - 3}}{\rm{M}};\\\left( {IO_3^ - } \right) = 5.3 \times {10^{ - 3}}{\rm{M}}\end{array}\)

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Most popular questions from this chapter

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.

\(\begin{array}{l}(a)BaSi{F_6},0.026\;g/100\;mL(contains Si{F_6}^2 - ions)\\(b)Ce{\left( {I{O_3}} \right)_4},1.5 \times 1{0^{ - 2}}\;g/100\;mL\\(c)G{d_2}{\left( {S{O_4}} \right)_3},3.98\;g/100\;mL\\(d){\left( {N{H_4}} \right)_2}PtB{r_6},0.59\;g/100\;mL(contains PtB{r_6}^{2 - } ions)\end{array}\)

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions.

(a) \(TlCl(s)\) in \(0.025MTlN{O_3}\)

(b) \(Ba{F_2}(\;s)\) in \(0.0313M\;KF\)

(c) \(Mg{C_2}{O_4}\) in \(2.250\;L\)of a solution containing \(8.156\;g\) of \(Mg{\left( {N{O_3}} \right)_2}\)

(d) \(Ca{(OH)_2}(\;s)\) in an unbuffered solution initially with a pH of \(12.700\)

Question: Calculate [HgCl42-] in a solution prepared by adding 0.0200 mol of NaCl to 0.250 L of a 0.100 M HgCl2 solution.

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.

\(\begin{array}{l}(a)BaSe{O_4},0.0118\;g/100\;mL\\(b)Ba{\left( {Br{O_3}} \right)_2} \times {H_2}O,0.30\;g/100\;mL\\(c)N{H_4}MgAs{O_4} \times 6{H_2}O,0.038\;g/100\;mL\\(d)L{a_2}{\left( {Mo{O_4}} \right)_3},0.00179\;g/100\;mL\end{array}\)

Calculate the volume of 1.50MCH3CO2H required to dissolve a precipitate composed of 350mg each of and CaCO3,SrCO3,BaCO3
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