During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. How many moles of acid are present in 2.0 liters of this unknown solution?

The moles of the acid in 2.0 liters of the unknown solution would be 8.0 moles

Since the acid is monoprotic, 1 mole of the acid will be required to stoichiometrically react with 1 mole of NaOH.

Using the formula:

Substitute into the equation:

Concentration of acid = 40/10 = 4.0 M

To determine the number of moles of acid present in 2.0 liters of the unknown solution:

           Number of moles = Molarity x volume

                                   = 4.0 x 2.0 = 8.0 moles

More on stoichiometric calculations can be found here: link

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .