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Chapter 7: Q28P (page 160)

Use Equation 7-12 to reproduce the curves in Figure 7-3. Plot your results on a single graph.

Short Answer

Expert verified

The graph of the silver halide titration curve:

Step by step solution

01

Concept used.

The equation for titration curve of $M^{+}$ with $X^{-}$ is

$V_{M} = {V_{X}}^{°} (\frac{{C_{x}}^{°} + [M^{+} l - [X^{-}]}{C_{M} - [M^{+}] - [X^{-} l})$

$C_{M} i$ is initial concentration of $M^{+}$

$C_{x} is concentration of X^{-} V_{x} is volume of X^{-}$

02

Plot the graph

The graph of a silver halide titration curve.

The spreadsheet for the silver iodide titration curve is as follows:

The graph of the silver halide titration curve looks like this:

As the solubility product of halides declines, so does the solubility of halides. Silver iodide has the steepest slope, indicating that it is least soluble. Because is dependent on the concentration of silver ions, the values rise as the solubility product decreases.

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Most popular questions from this chapter

Arsenic(III) oxide $({As}_{2} O_{3})$ is available in pure form and is a useful (but carcinogenic) primary standard for oxidizing agents such as ${MnO}_{4}^{-}$ .The $({As}_{2} O_{3})$ is dissolved in base and then titrated with in acidic solution. A small amount of iodide ${MnO}_{4}^{-}$ or iodate $({IO}_{3}^{-})$ is used to catalyze the reaction between $H_{3} {AsO}_{3}$ and ${MnO}_{4}^{-}$ .

${As}_{2} O_{3} + 4 OH □ 2 {HAsO}_{3}^{2 -} + H_{2} {OHAsO}_{3}^{2 -} + 2 H^{+} □ H_{3} {AsO}_{3} 5 H_{3} {AsO}_{3} + 2 {MnO}_{4}^{-} + 6 H^{+}$

$\to 5 H_{3} {AsO}_{4} + 2 {Mn}^{2} + 3 H_{2} O$

(c) It was found that 0.1468 g of ${As}_{2} O_{3}$ required 29.98 mL of ${KMnO}_{4}$ solution for the faint color of unreacted ${MnO}_{4}^{-}$ to appear. In a blank titration, 0.03 mL of ${MnO}_{4}^{-}$ was required to produce enough color to be seen. Calculate the molarity of the permanganate solution.

A solid mixture weighing 0.05485 gcontained only ferrous ammonium sulfate and ferrous chloride. The sample was dissolved in $1 {MH}_{2} {SO}_{4}$ , and the ${Fe}^{2 +}$ required 13.39mLof $0.01234 {MCe}^{4 +}$ for complete oxidation to ${Fe}^{3 +} ({Ce}^{4 +} + {Fe}^{2 +} \to {Ce}^{3 +} + {Fe}^{3 +})$ . Calculate the weight percent CI ofin the original sample.

Use the equation in Problem 7-29 to calculate the titration curve for $10.0 mL$ of $0.100 {MCrO}_{4}^{2 -}$ titrated with $0.100 {MAg}^{+}$ to produce ${Ag}_{2} {CrO}_{4} (s)$

What is the difference between a reagent-grade chemical and a primary standard?

Ammonia reacts with hypobromite, ${OBr}^{-}, {OBr}^{-}$ by the reaction ${2NH}_{3} + 30 {Br}^{-} \to N_{2} + 3 {Br}^{-} + 3 H_{2} O$ . What is the molarity of a hypobromite solution $1.00 mL$ of the ${OBr}^{-}$ solution reacts with $1.69 mg of {NH}_{3}$

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