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Chapter 15: Q37 E (page 873)

Calculate the concentration of Ag+ required to begin precipitation of Ag2CO3 in a solution that is 2.50 脳 10-6M in CO3 2-

Short Answer

Expert verified

The required [Ag+] =1.8脳10-3 M

Step by step solution

01

Define  Ksp

The solubility product constant is the equilibrium constant for the dissolution of a solid substance into an aqueous solution. It is denoted by the symbol Ksp.

02

Determining the concentration

Precipitation of Ag+ will begin when the ion product value is higher than solubility product constant value of Ag2CO3

\({K_{sp}}=8.2\times1{0^{-12}}\)

\(={\left( {A{g^+}}\right)^2}\left({CO_3^{2-}}\right)\)

\(={\left({A{g^+}}\right)^2}2.5\times1{0^{-6}}\)

03

Determining the concentration in precipitate

\(\left( {A{g^+}}\right)=\sqrt{\frac{{8.2\times1{0^{-12}}}}{{2.5\times1{0^{-6}}}}}\)

=1.8脳10-3M

The required (Ag+)=1.8脳10-3 M

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Most popular questions from this chapter

Perform the following calculations:

(a) Calculate \(\left[ {A{g^ + }} \right]\)in a saturated aqueous solution of\(AgBr\).

(b) What will \(\left[ {A{g^ + }} \right]\)be when enough \(KBr\)has been added to make \(\left[ {B{r^ - }} \right] = 0.050M\) ?

(c) What will \(\left[ {B{r^ - }} \right]\)be when enough \(AgN{O_3}\)has been added to make\(\left[ {A{g^ + }} \right] = 0.020M\)?

What mass of NaCN must be added to 1L of 0.010MMg (NO3)2in order to produce the first trace of Mg(OH)2?

A volume of \(50mL\) of \(1.8MN{H_3}\)is mixed with an equal volume of a solution containing\(0.95g\;of\;MgC{l_2}\). What mass of \(N{H_4}Cl\)must be added to the resulting solution to prevent the precipitation of \(Mg{(OH)_2}?\)

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

Question 31: Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix \(J\) for \({K_{sp}}\) values.)

(a) \(CaC{O_3}:\left( {C{a^{2 + }}} \right) = 0.003M,\left( {CO_3^{2 - }} \right) = 0.003M\)

(b) \(Co{(OH)_2}:\left( {C{o^{2 + }}} \right) = 0.01M,\left( {O{H^ - }} \right) = 1 \times 1{0^{ - 7}}M\)

(c) \(CaHP{O_4}:\left( {C{a^{2 + }}} \right) = 0.01M,\left( {HP{O_4}^{2 - }} \right) = 2 \times 1{0^{ - 6}}M\)

(d) \(P{b_3}{\left( {P{O_4}} \right)_2}:\left( {P{b^{2 + }}} \right) = 0.01M,\left( {PO_4^{3 - }} \right) = 1 \times 1{0^{ - 13}}M\)

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