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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 mixture having a volume of $10.00 mL$ and containing $0.1000 {MAg}^{+}$ and ${0.1000MHg}_{2}^{2 +}$ was titrated with $0.1000 MKCN$ to precipitate ${Hg}_{2} {(CN)}_{2}$ and $AgCN$ .

(a) Calculate ${pCN}^{-}$ at each of the following volumes of added KCN: $5.00, 10.00, 15.00, 19.90, 20.10, 25.00, 30.00, 35.00 mL$

(b) Should any AgCN be precipitated at $19.90 mL$ ?

Using Spreadsheets

Examine the procedure in Table $7 - 1$ for the Fajans titration of ${Zn}^{2 +}$ Do you expect the change on the precipitate to be positive or negative after the equivalence point?

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

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.

Limestone consists mainly of the mineral calcite, ${CaCO}_{3}$ .The carbonate content of 0.5413 g

powdered limestone was measured by suspending the powder in water, adding 10.00 mL of $1.396 MHCl$ and heating to dissolve the solid and expel role="math" localid="1654937947195" ${CO}_{2} {CaCO}_{3} (s) + 2 H^{+} \to {Ca}^{2 +} + {CO}_{2} ↑ + H_{2} O$ Calcium carbonate FM 100.087

The excess acid required $39.96 mL$ of $0.1004 MNaOH$ for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.

See all solutions

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