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Chapter 15: Q36 E (page 873)

Calculate the concentration of F- required to begin precipitation ofCaF2 in a solution that is 0.010M in Ca2+.

Short Answer

Expert verified

The concentration of [F-] = 6.24×10-5M

Step by step solution

01

Define concentration

The concentration is the abundance of a constituent divided by the total volume of a mixture. Several types of mathematical descriptions can be distinguished: mass concentration, molar concentration, number concentration, and volume concentration.

02

Calculating the concentration of solution

Precipitation of F-will begin when the ion product value is higher thansolubility product constant value ofCaF2

\begin{aligned}{{K_{sp}}=3.9\times{{10}^{-11}}=\left[{{\rm{C}}{{\rm{a}}^{2+}}}\right]{{\left[{{{\rm{F}}^-}}\right]}^2}=0.010{{\left[{{{\rm{F}}^-}}\right]}^2}}\\{\left[{{F^-}}\right]=\sqrt{\frac{{3.9\times{{10}^{-11}}}}{{0.010}}}=6.24\times{{10}^{-5}}{\rm{M}}}\end{aligned}

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Most popular questions from this chapter

A \({\bf{0}}.{\bf{125}}{\rm{ }}{\bf{M}}\) solution of \({\bf{Mn}}{\left( {{\bf{N}}{{\bf{O}}_{\bf{3}}}} \right)_{\bf{2}}}\) is saturated with\({{\bf{H}}_{\bf{2}}}{\bf{S}}{\rm{ }}\left( {\left[ {{{\bf{H}}_{\bf{2}}}{\bf{S}}} \right]{\rm{ }} = {\rm{ }}{\bf{0}}.{\bf{10}}{\rm{ }}{\bf{M}}} \right)\). At what pH does MnS begin to precipitate?

\(MnS(s) \rightleftharpoons M{n^{2 + }}(aq) + {S^{2 - }}(aq)\quad {K_{sp}} = 4.3 \times 1{0^{ - 22}}\)

\({H_2}S(aq) + 2{H_2}O(l) \rightleftharpoons 2{H_3}{O^ + }(aq) + {S^{2 - }}(aq)\quad K = 1.0 \times 1{0^{ - 26}}\)

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?

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.

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

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

\(\begin{array}{l}(a)BaS{O_4}(S) \to nB{a^{2 + }}(aq) + SO_4^{2 - }(aq)\\ X - \\(b)A{g_2}S{O_4}(S) \to n2A{g^ + }(aq) + S{O_4}^{2 - }(a)\\ - X\\(c)Al{(OH)_3}(S) \to nA{l^{3 + }}(aq) + 3O{H^ - }(aq)\\ X \_ \\(d)Pb(OH)Cl(S) \to nP{b^{2 + }}(aq) + O{H^ - }(aq) + C{l^ - }(aq)\\ \_ X \_\\(e)C{a_3}{\left( {As{O_4}} \right)_2}(S) \to n3C{a^{2 + }}(aq) + 2AsO_4^{3 - }(aq)\\ 3x \_\end{array}\)

Identify all chemical species present in an aqueous solution of \(C{a_3}{\left( {P{O_4}} \right)_2}\)and list these species in decreasing order of their concentrations. (Hint: Remember that the \(PO_4^{3 - }\) ion is a weak base.)
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