Question

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

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