Asked by Bella
Help please. Am doing a past exam paper and I hit a road block with this question:
Chloride in a brine solution is determined by a precipitation titration. A 10.00 mL
aliquot of the solution is titrated with 15.00mL of standard 0.1182 M AgNO3
solution. The excess silver is titrated with standard 0.1010 M KSCN solution,
requiring 2.38 mL to reach the red Fe(SCN)2+ endpoint. Calculate the
concentration of chloride in the brine solution, in g/1000mL.
Thank you! :)
Chloride in a brine solution is determined by a precipitation titration. A 10.00 mL
aliquot of the solution is titrated with 15.00mL of standard 0.1182 M AgNO3
solution. The excess silver is titrated with standard 0.1010 M KSCN solution,
requiring 2.38 mL to reach the red Fe(SCN)2+ endpoint. Calculate the
concentration of chloride in the brine solution, in g/1000mL.
Thank you! :)
Answers
Answered by
Bella
Do I calculate the moles of KSCN and the moles of AgNO3
.
Moles reacted: moles AgNO3 - moles KSCN
Then say : C =mols reacted/volume(the 10 ml volume x 10 to the minus 3)
Then multiple mol/L by g/mol then convert to g/ml
.
Moles reacted: moles AgNO3 - moles KSCN
Then say : C =mols reacted/volume(the 10 ml volume x 10 to the minus 3)
Then multiple mol/L by g/mol then convert to g/ml
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.