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Chapter 16: Problem 100

Order the following solids (a–d) from least soluble to most soluble. Ignore any potential reactions of the ions with water. a. \(\mathrm{AgCl} \quad K_{s p}=1.6 \times 10^{-10}\) b. \(\mathrm{Ag}_{2} \mathrm{S} \quad K_{\mathrm{sp}}=1.6 \times 10^{-49}\) c. \(\mathrm{CaF}_{2} \quad K_{\mathrm{sp}}=4.0 \times 10^{-11}\) d. \(\mathrm{CuS} \quad K_{\mathrm{sp}}=8.5 \times 10^{-45}\)

Short Answer

Expert verified
The order of the solubility of these solids based on their Ksp values is Ag2S < CuS < AgCl < CaF2, from least soluble to most soluble.

Step by step solution

01

List the given Ksp values for each solid

For each solid, we have the following Ksp values: a. AgCl: \(K_{sp} = 1.6 \times 10^{-10}\) b. Ag2S: \(K_{sp} = 1.6 \times 10^{-49}\) c. CaF2: \(K_{sp} = 4.0 \times 10^{-11}\) d. CuS: \(K_{sp} = 8.5 \times 10^{-45}\)
02

Identify the least soluble solid

From the given Ksp values, we can see that the solid with the lowest Ksp value is Ag2S with a Ksp of \(1.6 \times 10^{-49}\). This means that Ag2S is the least soluble solid among the four.
03

Identify the next least soluble solid

After Ag2S, the solid with the next lowest Ksp value is CuS with a Ksp of \(8.5 \times 10^{-45}\). This implies that CuS is the second least soluble solid among the four.
04

Identify the next least soluble solid

The solid with the next lowest Ksp value after CuS is AgCl with a Ksp of \(1.6 \times 10^{-10}\). This indicates that AgCl is the third least soluble solid among the four.
05

Identify the most soluble solid

Finally, the remaining solid is CaF2, which has a Ksp value of \(4.0 \times 10^{-11}\). By default, CaF2 is the most soluble solid among the four.
06

Order the solids from least soluble to most soluble

Taking all steps into account, we can order the solids as follows: 1. Ag2S (least soluble): \( K_{sp} = 1.6 \times 10^{-49} \) 2. CuS: \( K_{sp} = 8.5 \times 10^{-45} \) 3. AgCl: \( K_{sp} = 1.6 \times 10^{-10} \) 4. CaF2 (most soluble): \( K_{sp} = 4.0 \times 10^{-11} \) Thus, the order of the solubility of these solids is Ag2S < CuS < AgCl < CaF2.

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Most popular questions from this chapter

Write equations for the step wise formation of each of the following complex ions. a. \(N i(C N)_{4}^{2-}\) b. \(V\left(C_{2} O_{4}\right)_{3}^{3-}\)

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Nanotechnology has become an important field, with applications ranging from high-density data storage to the design of “nano machines.” One common building block of nano structured architectures is manganese oxide nano particles. The particles can be formed from manganese oxalate nano rods, the formation of which can be described as follows: $$\mathrm{Mn}^{2+}(a q)+\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(a q) \rightleftharpoons \mathrm{MnC}, \mathrm{O}_{4}(a q) \quad K_{1}=7.9 \times 10^{3}$$ $$\mathrm{MnC}_{2} \mathrm{O}_{4}(a q)+\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(a q) \rightleftharpoons \mathrm{Mn}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}^{2-}(a q) \quad K_{2}=7.9 \times 10^{1}$$ Calculate the value for the overall formation constant for \(\mathrm{Mn}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}^{2-} :\) $$K=\frac{\left[\mathrm{Mn}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}^{2-}\right]}{\left[\mathrm{Mn}^{2+}\right]\left[\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right]^{2}}$$
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