I need help solving this

Question

What volume (in mL) of 0.2600M HBr is required to neutralize 40.00mL of 0.8000 M NaOH?

Answer 1

Look at the balanced equation:

HBr + NaOH ==> NaBr + H2O ... balanced equation

This tells us that it takes 1 mol of HBr to react (neutralize) 1 mole of NaOH

moles NaOH present = 40.00 ml x 1 L/1000 ml x 0.8000 mol/L = 0.032 moles NaOH

So it will take 0.032 moles of HBr to neutralize the NaOH. To find the volume of HBr needed ...

(x L)(0.2600 mol/L) = 0.032 moles

x = 0.123 L = 123 mls of HBr is needed