This is about back titration to determine the percentage of sodium carbonate in an unknown sample by reaction with excess sulfuric acid followed by the back titration of the acid with sodium hydroxideInformation_H2SO4M=0.05137Mass of impure sample of Na2CO3m=1.5033gPart A.Standardization of NaOH solution: 24.27ml NaOH25ml of H2SO4Part B.the impure carbonate is dissolved in 250ml of deionized watereach flask has:50 ml H2SO425ml of impure solutionthat has been back titrated with 38.15ml NaOHQuestions:1)How do you calculate the moles of sulfuric acid that remained in the solution after the reaction with the carbonate?2) calculate the moles of sulfuric acid that reacted with the carbonate3) calculate the moles of sodium carbonate present in the original 25.00ml and 250.0ml of solution.4) calculate the percent of sodium carbonate in the impure sample.there are other questions before this but i think i know how to do them. its just these questions that really got me stuck.thank you for your help!
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