An HNO3 solution has a pH of 3.47. What volume of 0.015 M LiOH will be required to titrate 65.0 mL of the HNO3

Question

An HNO3 solution has a pH of 3.47. What volume of 0.015 M LiOH will be required to titrate 65.0 mL of the HNO3 solution to reach the equivalence point?

Answer 1

We have to convert the pH to a [H+]. So we convert: [H+]= 3.2x10-4 (poof!). So we can use the relation
Vol x conc (HNO3) = Vol x conc (LiOH)
Just dump in the numbers and solve.

Answer 2

i trust that in a good acid/base reaction the volume of the acid is a similar because the volume of the bottom. Use M1V1=M2V2 (a million.500mol/liter)(0.03220 liter)= (a million.420 mol/L)(X). X is the unknown volume. clean up for x. x= 0.0340 L=34.00 mL