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Chapter 7: Q30P (page 160)

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 ${Ag}_{2} {CrO}_{4} (s)$

Short Answer

Expert verified

The graph of the titration is

Step by step solution

01

Define the equation for titration curve.

$The equation for titration curve of M^{+} with X^{-} is V_{M} = (\frac{{C_{x}}^{0} + [M^{+}] - [X^{-}]}{{C_{M}}^{°} + [M^{+}] - [X^{-}]}) Where, {C_{M}}^{°} is initial concentration of M^{+} {V_{M}}^{°} is volume of added M^{+} c_{x} is concentration of X^{-} V_{x} os volume of X^{-}$

02

plot the titration graph.

The graph of titration curve for silver chromate.

The spreadsheet for titration curve of silver ion is given as

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Most popular questions from this chapter

A 25.00 - mL solution containing 0.031 10 M ${Na}_{2} C_{2} O_{4}$ was titrated with 0.025 70 M $Ca ({NO}_{3})_{2}$ to precipitate calcium oxalate: $C a^{2 +} + C_{2} O_{4}^{-} \to C a C O_{4} (s)$ Find pCa²⁺ at the following volumes

of : $C a ({NO}_{3})_{2}$

(a) 10.00,

(b) Ve

(c) 35.00 mL

Ascorbic acid (vitamin C) reacts with ${I_{3}}^{-}$ 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.

A 2.000-g mixture containing only $K_{2} {CO}_{3}$ (FM 138.21) and ${KHCO}_{3}$ (FM 100.12) requiredof 15.00 mL of 1.000MHCIfor complete titration. Find the mass of each component of the mixture.

Consider precipitation of $X^{x -}$ with role="math" localid="1655098271650" $M^{m +}$ :

${xM}^{m +} + {mX}^{x -} ⇌ M_{x} X_{m} (s) K_{sp} = [M^{m +}]^{x} [X^{x -}]^{m}$ Write mass balance equations for M and X and derive the equation

$V_{M} = V_{x}^{0} \frac{({xC}_{X}^{0} + m [M^{m +}] - x [X^{x -}]}{({mC}_{M}^{0} - m [M^{m +}] + x [X^{x -}]} where [X^{x -}] = {(K_{sp} / [M^{m +}]^{x})}^{\frac{1}{m}}$

Why does the surface charge of a precipitate change sign atthe equivalence point?

See all solutions

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