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# Stoicheometry as Potassium Salts

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A 2.9880g sample containing Cl- and ClO4- (as the potassium salts) was dissolved in sufficient water to give 250.0 mL of solution. a 50.00mL aliquot required 13.97mL of 0.08551M AgNO3 to titrate the Cl-. In a second 50.00mL aliquot, the ClO4- was reduced to Cl- with V2(SO4)3. Titration of the reduced sample required 40.12mL of the AgNO3 solution. Calculate the %KCl and %KClO4 in the sample.

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#### Solution Preview

2.9880g sample containing KCl and KClO4
Dissolve in 250mL

1) Take 50mL
13.97mL of a 0.08551 M AgNO3 solution = 0.0012 moles AgNO3

Since AgNO3 and KCl react 1 to 1 in stoichiometry, this means there is 0.0012 moles of KCl in the 50mL aliquot. So, 0.0012 x 5 = 0.06 moles of KCl in 250 mL solution ...

#### Solution Summary

The expert examines stoicheometry of potassium salts. The %KCl and %KClO4 are calculated.

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