Asked by lavonne
If 20.0mL of an unknown acid was titrated with 2.0 M KOH and 60.0 mL KOH was used what is the molarity of the unknown acid?
Answers
Answered by
bobpursley
If you don't know if the unknown acid was monoprotic, diprotic, or triprotic, you cannot determine molarity of the acid.
Assuming monoprotic (as in acetic acid, hydrochloric, nitric, citric)
Macid*Vacid=Mbase*Vbase
Macid=2M*60ml/20ml=6M
Normally, you should solve these equations using Normality as the concentration, but I suspect your teacher has not exposed you to that yet.
http://environmentalchemistry.com/yogi/chemistry/MolarityMolalityNormality.html
Assuming monoprotic (as in acetic acid, hydrochloric, nitric, citric)
Macid*Vacid=Mbase*Vbase
Macid=2M*60ml/20ml=6M
Normally, you should solve these equations using Normality as the concentration, but I suspect your teacher has not exposed you to that yet.
http://environmentalchemistry.com/yogi/chemistry/MolarityMolalityNormality.html
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