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2.2012g of solute with an unknown amount of KHP (weak acid, 204.22 g/mol), was potentiometricaly titrated with 0.0901M NaOH. Both the first and second derivativeof the titration curve point out that the equivalence point was when 5.75mL of titrant (NaOH) were used. Before the titration the solute was dissolved in a 500mL volumetric flask with DI water. From the equivalence volume, concentration and molar mass, calculate the %KHP in the unknown sample.
P.S I did some calculations and got thath the sample was 4.82% KHP, is this correct?
2.2012g of solute with an unknown amount of KHP (weak acid, 204.22 g/mol), was potentiometricaly titrated with 0.0901M NaOH. Both the first and second derivativeof the titration curve point out that the equivalence point was when 5.75mL of titrant (NaOH) were used. Before the titration the solute was dissolved in a 500mL volumetric flask with DI water. From the equivalence volume, concentration and molar mass, calculate the %KHP in the unknown sample.
P.S I did some calculations and got thath the sample was 4.82% KHP, is this correct?
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Tod ThielLv2
28 Sep 2019
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