Answer to Question #109113 in General Chemistry for sam

Question

the titration of 19.30 mL of HBr solution of unknown concentration requires 18.11 mL of a 0.100 M KOH solution to reach the equivalence point. What is the concentration of the unknown HBr solution in M?

Answer 1

In equivaelence point n(HBr_initial)=n(KOH_added). Then if concentration of HBR was x,

19.30/1000*x = 18.11/1000*0.1

$1={\frac {18.11*0.100} {19.30*x}}$

$x={\frac {18.11*0.100} {19.30}}=0.094$

Concentration of HBr solution is 0.094 M