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Chapter 15: Q38 E (page 873)

What [Ag+] is required to reduce [CO32-] to 8.2 ×10-4M by precipitation of Ag2Co3?

Short Answer

Expert verified

The required [Ag+] = 9.9×10-5M

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 required precipitation

Substituting in solubility product

\[{K_{sp}}=8.1\times1{0^{-12}}={\left[{A{g^+}}\right]^2}\left[{CO_3^-}\right]\]

\[={\left[{A{g^+}}\right]^2}8.2\times1{0^{-4}}\]

\[\left[{A{g^+}}\right]=\sqrt{\frac{{8.1\times1{0^{-12}}}}{{8.2\times1{0^{-4}}}}}=9.9\times1{0^{-5}}M\]

03

Reducing precipitation

The required precipitation of [Ag+]

[Ag+] = 9.9×10-5M

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Most popular questions from this chapter

Calculate the concentration of PO43-when Ag3 PO4 starts to precipitate from a solution that is 0.0125M in Ag+.

Question: Using Lewis structures, write balanced equations for the following reactions:

\({\rm{\;}}(a)\;HCl(g) + P{H_3}(g) \to \)

\({\rm{\;}}(b)\;{H_3}{O^ + } + CH_3^ - \to \)

\({\rm{\;}}(c)\;CaO + S{O_3} \to \)

\(\;(d)\;NH_4^ + + {C_2}{H_5}{O^ - } \to \)

Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products):

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(d) \(Sr{(\;OH\;)_2} \times 8{H_2}O\)

(e) The mineral brucite, \(Mg{(\;OH\;)_2}\)

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What is the molar solubility of CaF2 in a 0.100 M solution of HF? Kafor HF = 7.2 × 10–4.
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