A 10.00 mL chloride sample required 33.65 mL of 0.01251 M AgNO_3 to reach the en

Question

A 10.00 mL chloride sample required 33.65 mL of 0.01251 M AgNO_3 to reach the end point. a) How many moles of CI^- were present in the sample? b) What was the molarity of the CI^- sample? Would the following errors increase, decrease or not change the molarity of CI^- as calculated is part lb? Explain your answer (use a calculation if needed)! a) The student was past the end point of the titration when final volume was recorded. b) The student incorrectly read the molarity of AgNO_3 as 0.01521 M

Explanation / Answer

Q2.

a)

if the student get past the end point, then, there is more moles of titrant than there are of specie, i.e. the amount will be highly miscalculated, expect am increase in the actual value of molarity/moles of specie being titrated

b)

M = 0.01521 M instead of 0.01251

so.. the molarity of titrant is higher than the real one

when peroforming his calculations, he will account for a higher molarity --> high number of moles

so it will increase the [Cl-]

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