A 13.8 mL aliquot of 0.176 M H₃PO₄ (aq)is to be titrated with 0.110 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point? A)7.29 B)22.1 C)199 D)66.2 E)20.9

Question

Quizplus · Accepted Answer

To solve the problem, we can use the formula for calculating the volume of base required to reach the equivalence point: V(base) = (V(acid) x N(acid) x M(acid)) / M(base) where V(acid) is the volume of the acid solution (13.8 mL), N(acid) is the number of acidic hydrogen atoms (which is 1 in this case, since H₃PO₄ has only one acidic hydrogen), M(acid) is the molarity of the acid solution (0.176 M), and M(base) is the molarity of the base solution (0.110 M). Plugging in the numbers, we get: V(base) = (13.8 mL x 1 x 0.176 M) / 0.110 M = 22.2 mL Therefore, the volume of base required to reach the equivalence point is 22.2 mL or approximately 66.2 mL (as given in option D).

A 138 ML Aliquot of 0