Question

Predict what volume (mL) of 0.3000 M NaOH is required to titrate the 25.00 mL of 0.3000 M HCl to the equivalence point.

a) 12.5 mL
b) 25.00 mL
c) 50.00 mL
d) 37.50 mL

Answer 1

The volume of 0.3000 M NaOH required to titrate 25.00 mL of 0.3000 M HCl to the equivalence point is 25.00 mL, as equal molarity and stoichiometry lead to equal volumes at neutrality.

Step-by-step explanation:

To predict the volume of 0.3000 M NaOH required to titrate 25.00 mL of 0.3000 M HCl to the equivalence point, we use the concept of molarity and the stoichiometry of the neutralization reaction between NaOH and HCl. Since both are monoprotic (one mole of acid reacts with one mole of base) and they are at the same concentration, the moles of HCl will be equal to the moles of NaOH at the equivalence point.

Using the formula:

• n(NaOH) = V(NaOH) × M(NaOH)
• n(HCl) = V(HCl) × M(HCl)

Because n(NaOH) = n(HCl) and M(NaOH) = M(HCl), we can equate the volumes directly:

V(NaOH) = V(HCl)

Therefore, 25.00 mL of NaOH is required to reach the equivalence point, matching option (b) 25.00 mL.