How many milliliters of 0.305M NaOH would be required to titrate a 5.00mL solution of 0.616M HBr?

Answer 1

MiVi=MfVf

Vi=MfVf/Mi

Vi=0.616M*5.00mL/0.305M

Vi=10.1mL

Answer 2

Since NaOH and HBr react in a 1:1 ratio, the moles of NaOH needed to titrate HBr can be calculated. Moles of NaOH = moles of HBr. Next, use the concentration and volume of HBr to find the moles present. Finally, use the concentration of NaOH to calculate the volume needed. In this case, approximately 2.41 mL of 0.305M NaOH would be needed.