A 0.201 M aqueous solution of NaOH was used to titrate HCl in an aqueous solution. 30.5 ml of the NaOH was needed to neutralize 20.0 ml the acid a) write a balanced molecular equation of the reaction b) how many moles of NaOH were consumed for the reaction c) how many moles of HCl were neutralized d) calculate the concentration of the HCl solution

Question

Clarence Chase

Chemistry

24 July, 17:17

A 0.201 M aqueous solution of NaOH was used to titrate HCl in an aqueous solution. 30.5 ml of the NaOH was needed to neutralize 20.0 ml the acid a) write a balanced molecular equation of the reaction b) how many moles of NaOH were consumed for the reaction c) how many moles of HCl were neutralized d) calculate the concentration of the HCl solution

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Jessica Espinoza · Answer 1

chemical equation

(a) NaOH + HCL - - - >NaCl + H2O

(b) THE number of moles reacted is = molarity x volume in litres

hence the number of moles of NaOH = (o. 201 x 30.5ml) / 100ml=0.00613 moles

(C) the number of moles of Hcl that were reacted, from the reaction above the recting ratio of NaOH to HCl is 1:1 thus the moles of HCl is also 0.00613

(D) my of HCl is = moles/volume in litres

that is (0.00613/20) x 1000=0.306M