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Chapter 15: Problem 2

Devise as many ways as you can to experimentally determine the \(K_{\mathrm{sp}}\) value of a solid. Explain why each of these would work.

Short Answer

Expert verified
There are several methods to experimentally determine the \(K_{sp}\) value of a solid: 1. Direct measurement method: Dissolve a known amount of solid in a known volume of solvent, allow the system to reach equilibrium, filter the saturated solution, and determine the ion concentrations using techniques like AAS, ICP-OES, or ion-selective electrodes. Calculate the \(K_{sp}\) using the expression. 2. Titrimetric method: Prepare a saturated solution, determine the concentration of one ion by titrating against a known solution, calculate the concentration of the other ion based on stoichiometry, and determine the \(K_{sp}\) using the equilibrium expression. 3. Conductivity method: Prepare a saturated solution, measure its conductivity, create a calibration curve using standard solutions, determine the ion concentrations from the calibration curve, and calculate the \(K_{sp}\) using the equilibrium expression. 4. Spectrophotometric method: Determine the concentration of ions in the saturated solution by monitoring their absorbance or emission of electromagnetic radiation, create a calibration curve using standard solutions, determine the ion concentrations from the calibration curve, and calculate the \(K_{sp}\) accordingly. Each method works by determining concentrations of ions in a saturated solution at equilibrium, essential for calculating the \(K_{sp}\) value. The choice of method depends on the solid's nature, ion solubility, and analytical technique availability.

Step by step solution

01

1. Direct measurement method

In this method, a known amount of the solid is dissolved in a known volume of solvent, and the system is left undisturbed until it reaches equilibrium. After this, an aliquot of the saturated solution is filtered to remove any excess solid. The concentrations of the ions in the filtered solution can be determined using techniques like atomic absorption spectroscopy (AAS), inductively coupled plasma optical emission spectroscopy (ICP-OES), or ion-selective electrodes. Once the concentrations are known, the \(K_{sp}\) can be calculated using the expression, \(K_{sp} = [A^{n+}][B^{m-}]\), where n and m are the charges of the ions, and [A] and [B] are their concentrations.
02

2. Titrimetric method

In this approach, a saturated solution is prepared, and the concentration of one of the ions (let's say A) is determined by titrating it against a solution of known concentration of a reagent that reacts with ion A. The endpoint of the titration is detected using an appropriate indicator, a pH meter, or a potentiometric method. Once the concentration of ion A is known, the concentration of the other ion (B) can be calculated using the stoichiometry of the dissolution reaction. The \(K_{sp}\) is then determined by plugging these concentrations into the equilibrium expression.
03

3. Conductivity method

This method is based on the fact that the conductivity of a solution is directly proportional to the concentration of the ions present in it. The experiment begins with preparing a saturated solution of the solid and measuring its conductivity. A calibration curve can be created by measuring the conductivity of a series of standard solutions with known concentrations of the ions. The concentrations of the ions in the saturated solution can then be determined by comparing its conductivity with the values from the calibration curve. The \(K_{sp}\) is subsequently calculated using the equilibrium expression.
04

4. Spectrophotometric method

In this technique, the concentration of the ions in the saturated solution is determined by monitoring the absorbance or emission of electromagnetic radiation at a specific wavelength. A calibration curve is generated by measuring the absorbance or emission of a series of standard solutions with known concentrations of the ions. The concentration of the ions in the saturated solution is then determined using this calibration curve, and the \(K_{sp}\) is calculated accordingly. Each of these methods works because they allow the determination of the concentrations of ions in a saturated solution at equilibrium, which is essential to calculate the \(K_{sp}\) value. Moreover, the choice of the method depends on the nature of the solid, the solubility of the ions, and the availability of the analytical techniques.

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Most popular questions from this chapter

The \(\mathrm{Hg}^{2+}\) ion forms complex ions with \(\mathrm{I}^{-}\) as follows: $$\begin{aligned} \mathrm{Hg}^{2+}(a q)+\mathrm{I}^{-}(a q) & \rightleftharpoons \mathrm{HgI}^{+}(a q) & & K_{1}=1.0 \times 10^{8} \\ \mathrm{HgI}^{+}(a q)+\mathrm{I}^{-}(a q) & \rightleftharpoons \mathrm{HgI}_{2}(a q) & & K_{2}=1.0 \times 10^{5} \\ \mathrm{HgI}_{2}(a q)+\mathrm{I}^{-}(a q) & \rightleftharpoons \mathrm{HgI}_{3}^{-}(a q) & & K_{3}=1.0 \times 10^{9} \\ \mathrm{HgI}_{3}^{-}(a q)+\mathrm{I}^{-}(a q) & \rightleftharpoons \mathrm{HgI}_{4}^{2-}(a q) & & K_{4}=1.0 \times 10^{8} \end{aligned}$$ A solution is prepared by dissolving 0.088 mole of \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}\) and 5.00 moles of NaI in enough water to make 1.0 L of solution. a. Calculate the equilibrium concentration of \(\left[\mathrm{HgI}_{4}^{2-}\right] .\) b. Calculate the equilibrium concentration of \(\left[\mathrm{I}^{-}\right] .\) c. Calculate the equilibrium concentration of \(\left[\mathrm{Hg}^{2+}\right]\).

Use the following data to calculate the \(K_{\mathrm{sp}}\) value for each solid. a. The solubility of \(\mathrm{CaC}_{2} \mathrm{O}_{4}\) is \(4.8 \times 10^{-5} \mathrm{mol} / \mathrm{L}\) b. The solubility of \(\mathrm{BiI}_{3}\) is \(1.32 \times 10^{-5} \mathrm{mol} / \mathrm{L}\)

Calculate the molar solubility of \(\mathrm{Cd}(\mathrm{OH})_{2}, K_{\mathrm{sp}}=5.9 \times 10^{-11}\).

\(\mathrm{Ag}_{2} \mathrm{S}(s)\) has a larger molar solubility than CuS even though \(\mathrm{Ag}_{2} \mathrm{S}\) has the smaller \(K_{\mathrm{sp}}\) value. Explain how this is possible.

The \(K_{\mathrm{sp}}\) for silver sulfate \(\left(\mathrm{Ag}_{2} \mathrm{SO}_{4}\right)\) is \(1.2 \times 10^{-5} .\) Calculate the solubility of silver sulfate in each of the following. a. water b. \(0.10 M\) AgNO \(_{3}\) c. \(0.20 M \mathrm{K}_{2} \mathrm{SO}_{4}\)
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