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Titration Calculations

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Note: You may assume that the densities of all solutions are 1.00 g/mL unless stated otherwise

1. A 10.00-mL sample of a solution containing the weak acid, formic acid, was placed in a 25-mL volumetric flask and diluted to the mark with water. A 10.00-mL sample of the diluted formic acid solution was then titrated with 0.1322 M sodium hydroxide. If the titration required 15.80 mL of sodium hydroxide to reach the equivalence point, calculate the molarity and percentage by mass of formic acid in the original solution before dilution.

2. A student titrated a solution of formic acid with sodium hydroxide. The student plotted pH versus volume (mL) of NaOH added and found that the titration required 26.66 mL of NaOH to reach the equivalence point. Describe how you would use the student's titration curve to determine the Ka for formic acid.

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This solution contains step-by-step titrations calculation to determine the molarity and percentage by mass of formic acid in the original solution and also how to find the ka.

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Potentiometer titration calculation

A 25 ml mixture of HCl-H3PO4 was diluted with 75ml with dH2O, total volume 100ml, and then 25 ml of that was removed and added with 75 ml of dH2O. This mixture was then titrated with 0.1M NaOH, attached is data that was found. What are the molarities of the HCl and H3PO4 in the original solution?

First equivalence point:
HCl + NaOH -> H2O + NaCl
H3PO4 + NaOH -> NaH2PO4 +H2O

Second equivalence point:
NaH2PO4 + NaOH -> Na2HPO4 +H2O

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