What is the concentration of an hbr solution if 12.0 ml of the solution is neutralized by 15.0 ml of a 0.25 m koh solution?

The balanced equation for the reaction between KOH and HBr is as follows;

KOH + HBr - - > KBr + H₂O

stoichiometry of KOH to HBr is 1:1

number of KOH moles reacted - 0.25 mol/L x 0.015 L = 0.00375 mol

according to molar ration

number of KOH moles reacted = number of HBr moles reacted

number of HBr moles reacted - 0.00375 mol

if 12 mL of HBr contains - 0.00375 mol

then 1000 mL of HBr contains - 0.00375 mol / 12 mL x 1000 mL = 0.313 mol

therefore molarity of HBr is 0.313 M