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Chapter 7: Q23P (page 159)

The text claims that precipitation of $l^{-}$ is not complete before ${Cl}^{-}$ begins to precipitate in the titration in Figure 7-4. Calculate the concentration ${Ag}^{+}$ of at the equivalence point in the titration of $l^{-}$ alone. Show that this concentration ${Ag}^{+}$ of ${Cl}^{-}$ will precipitate.

Short Answer

Expert verified

The concentration of silver ion at equivalence point in given titration is $9.1 脳 10^{- 9} M$ .

Step by step solution

01

Concept used.

In titration, the equivalence point is the point at which the quantity of standard solution and analysis becomes equal and neutralisation occurs.
The end point is when the colour changes at a specific point in the titration.

02

The concentration of Ag+ at the equivalence point in the titration of alone.

The first equivalence point where silver iodide precipitates first because

$V_{c} 脳 0.0845 M = 0.040 L 脳 0.0502 M V_{c} = \frac{0.040 L 脳 0.0502 M}{0.0845 M} = 0.023676 L = 23.76 mL At the equivalence point, the concentrations of silver and iodide ions are the same . [{Ag}^{+}] [I^{-}] = x^{2} = K_{sp} [{Ag}^{+}] [{Cl}^{-}] = x^{2} = 8.3 脳 10^{- 17} [{Ag}^{+}] = 9.1 脳 10^{- 9} M Q = [{Ag}^{+}] [{Cl}^{-}] = 2.8 脳 10^{- 10} The Q value which is greater than solubility product constant of silver chloride . Thus silver ions can precipitate .$

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Most popular questions from this chapter

What is wrong with this procedure? According to Table 7-1, carbonate can be measured by a Volhard titration. Removal of the precipitate is required. To analyse an unknown solution of, ${Na}_{2} {CO}_{3}$ , l acidified the solution with freshly boiled and cooled ${HNO}_{3}$ to give ,0.5 M ${HNO}_{3}$ . Then I added excess standard, but no ${Ag}_{2} {CO}_{3}$ precipitate formed. What happened?

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 ${MnO}_{4}^{-}$ .

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

$鈫� 5 H_{3} {AsO}_{4} + 2 {Mn}^{2} + 3 H_{2} O$

(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 solution of NaOH was standardized by gravimetric titration of a known quantity of the primary standard, potassium hydrogen phthalate:

The was then used to find the concentration of an unknown solution of $H_{2} {SO}_{4}$

$H_{2} {SO}_{4} + 2 NaOH 鈫� {Na}_{2} {SO}_{4} + 2 H_{2} O$

A 10.00-mL aliquot of $H_{2} {SO}_{4}$ solution required 57.911 g of NaOH solution to reach the phenolphthalein end point. Find the molarity of $H_{2} {SO}_{4}$

Sulfamic acid is a primary standard that can be used to standardize $NaOH .$

$^{+} H_{3} {NSO}_{3}^{-} + OH 鈫� H_{2} {NSO}_{3}^{-} + H_{2} O$ Sulfamic acidFM 97.094What is the molarity of a sodium hydroxide solution if $34.26 mL$ react with $0.3337 g$ of sulfamic acid?

Ascorbic acid (vitamin C) reacts with according to the equation

Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when the first fraction of a drop of unreacted ${I_{3}}^{-}$ remains in the solution.

(a) Verify that the structures above have the chemical formulas written beneath them. You must be able to locate every atom in the formula. Use atomic masses from the periodic table on the inside cover of this book to find the formula mass of ascorbic acid.

(b) If 29.41 mL of ${I_{3}}^{-}$ solution are required to react with 0.197 0 g of pure ascorbic acid, what is the molarity of the ${I_{3}}^{-}$ solution?

(c) A vitamin C tablet containing ascorbic acid plus inert binder was ground to a powder, and 0.424 2 g was titrated by 31.63 mL of ${I_{3}}^{-}$ . Find the weight percent of ascorbic acid in the tablet.

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