A 50.00 mL sample containing two unknown anions was titrated using 0.1021 M AgNO

Question

A 50.00 mL sample containing two unknown anions was titrated using 0.1021 M AgNO3 in the presence of 1.00 mL of HNO3 and produced the following titration curve: a. (4 pts) In a general sense (using the symbol ''X'' for the analyze) write out BOTH the titration reaction AND the reduction half-reaction actually occurring at the indicator electrode in this titration. Titration: Indicator: b. (5 pts) What was the initial concentration of the second anion titrated? c. (10 pts) Based on the given list of possible anions, what is the Identity of the second anion titrated?

Explanation / Answer

a) Titration: AgNO3 + X -----> AgX + NO3-

     Indicator: Ag+ + e- ----> Ag

b) Volume of AgNO3 consumed for second anion = 29.8 ml

     Concentration of AgNO3 = 0.1021 M

    Volume of unknown sample = 50 ml

    Concentration of Second anion (X) = 29.8 x 0.1021 / 50 = 0.061 M

  

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