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
A) 6.0 moles
B) 7.0 moles
C) 8.0 moles
D) 9.0 moles
E) None of the above

Question

Quizplus · Accepted Answer

First we need to find the number of moles of NaOH used in the titration:

1.0 mol NaOH = 1 L NaOH

Therefore:

40 mL NaOH x (1 L / 1000 mL) x (1 mol NaOH / 1 L) = 0.04 mol NaOH

Since the acid is monoprotic (meaning it donates only one proton/H+), the number of moles of acid is equal to the number of moles of NaOH used in the titration:

0.04 mol H+ = 0.04 mol acid

Now we can calculate the concentration of the unknown acid solution:

0.04 mol / 0.01 L = 4 mol/L

Finally, to find the number of moles in 2 liters of this solution:

4 mol/L x 2 L = 8 mol

Therefore, the answer is C) 8.0 moles.

During a Titration the Following Data Were Collected