If 25.0 ml of an hbr solution were titrated with 29.15 ml of a 0.205 m lioh solution to reach the equivalence point then what is the molarity of the hbr solution?

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

HBr + LiOH —> LiBr + H2O

Stoichiometry of HBr to LiOH is 1:1

The number of LiOH moles reacted - 0.205 mol/L x 0.02915 L = 0.00598 mol

The number of HBr moles reacted = number of LiOH moles reacted

Therefore the number of HBr moles reacted = 0.00598 mol

If 25.0 mL of HBr contains - 0.00598 mol

Then 1000 mL of HBr contains - 0.00598 / 25.0 mL x 1000 mL = 0.239 mol

The molarity of HBr is -0.239 mol/L

idk

explanation:

dasdad

your answer would be “dry”