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Chapter 15: Q1 E (page 870)

Precipitation and Dissolution

1. Complete the changes in concentrations for each of the following reactions:

\(\begin{array}{l}(a)AgI(s) \to nA{g^ + }(aq) + {I^ - }(aq)\\ x \_ \\(b)CaC{O_3}(s) \to C{a^{2 + }}(aq) + C{O_3}^{2 - }(aq)\\ \_\quad x\\(c)Mg{(OH)_2}(s) \to nM{g^{2 + }}(aq) + 2O{H^ - }(aq)\\ x \quad \_\_\\(d)M{g_3}{\left( {P{O_4}} \right)_2}(s) \to n3M{g^{2 + }}(aq) + 2P{O_4}^{3 - }(aq)\\ x\_\\(e)C{a_5}{\left( {P{O_4}} \right)_3}OH(s) \to n5C{a^{2 + }}(aq) + 3P{O_4}^{3 - }(aq) + O{H^ - }(aq)\\ \_ \_ x\end{array}\)

Short Answer

Expert verified

Precipitation reactions can be defined as reaction in which two ionic bonds combine in aqueous solution chemically resulting in the formation of an insoluble salt.

(a) x

b) x

c) 2 x

d) 3 x

e) 5 x

Step by step solution

01

Step 1:To find  the changes in concentrations for each of the following reactions

\(AgI\;(s) \to A{g^ + }\;(aq) + {I^ - }\;(aq)\)

By dissolving\(AgI\) in water, solution of mixed silver and chloride ions is produced. In this case, both silver and chloride ions produce an equal amount of the solid

02

:To find  the changes in concentrations for each of the following reactions

\(CaC{O_3}(\;s) \to C{a^{2 + }}(aq) + CO_3^{2 - }(aq)\)

03

Step 3:To find  the changes in concentrations for each of the following reactions

\(Mg{(OH)_2}\;(\;S) \to \;M{g^{2 + }}\;(aq) + \;2O{H^ - }(aq)\)

By dissolving\(CaC{O_3}\)in water, solution of mixed magnesium and hydroxide ions is produced. On the contrary to a) and

b), one ion of magnesium and two hydroxide ions are needed to produce one molecule of the solid.

04

To find the changes in concentrations for each of the following reactions

\(M{g_3}{\left( {P{O_4}} \right)_2}(S) \to \;3M{g^{2 + }}(aq) + 2PO_4^{3 - }(aq)\)

05

Step 5:To find  the changes in concentrations for each of the following reactions

\(C{a_5}{\left( {P{O_4}} \right)_3}OH(S) \to \;5C{a^{2 + }}(aq) + 3PO_4^{3 - }(aq)\)

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Most popular questions from this chapter

Question: Calculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe (CN)6] is added to a solution with 0.0.00010 M CN鈥�.

To a \({\bf{0}}.{\bf{10M}}\) solution of \({\bf{Pb}}{\left( {{\bf{N}}{{\bf{O}}_{\bf{3}}}} \right)_{\bf{2}}}\) is added enough \({\bf{HF}}\left( {\bf{g}} \right)\) to make\(\left[ {{\bf{HF}}} \right]{\rm{ }} = {\rm{ }}{\bf{0}}.{\bf{10}}{\rm{ }}{\bf{M}}\).

(a) Does \({\bf{Pb}}{{\bf{F}}_{\bf{2}}}\) precipitate from this solution? Show the calculations that support your conclusion.

(b) What is the minimum pH at which \({\bf{Pb}}{{\bf{F}}_{\bf{2}}}\) precipitates?

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.

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

Question: What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases, it may be necessary to control the \(pH\).(Hint: Consider the \({K_{sp}}\)values given in

(a) \(H{g_2}^{2 + }\;and\;C{u^{2 + }}\)

(b) \(S{O_4}^{2 - }\;and\;C{l^ - }\)

(c) \(H{g^{2 + }}\;and\;C{o^{2 + }}\)

(d) \(Z{n^{2 + }}\;and\;S{r^{2 + }}\)

(e) \(B{a^{2 + }}\;and\;M{g^{2 + }}\)

(f) \(CO_3^{2 - }\;and\;O{H^ - }\)

What [F-] is required to reduce [Ca2+] to 1.0脳10-4M by precipitation of CaF2?
See all solutions

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