20.0 ml of 0.06 m hcl (in a flask) is titrated with 0.04 m naoh (in a burette). how many milliliters of naoh needs to be used to reach the equivalence point?
a.0.03 ml
b.20.0 ml
c.20 ml
d.30 ml

2.which of the following would you identify a titration curve that involved a strong acid titrated by a weak base?
a. the ph at the equivalence point is lower than 7.
b. the ph at the equivalence point is higher than 7.
c. the titration curve begins at a higher ph and ends at a lower ph.
d. there is a rapid change in ph near the equivalence point (ph = 7).

There is a rapid change in pH near the equivalence point (pH = 7).

Explanation:

At equivalence point the moles of base used is equal to moles of acid taken.

Let us calculate the moles of acid taken.

Moles = molarity X volume (L)

Given

molarity = 0.06 M

Volume =20.0 mL = 20 X 10⁻³ L

moles of HCl = 0.06 X 20 X 10⁻³= 1.2 X 10⁻³

moles of NaOH required = 1.2 X 10⁻³

Thus volume of NaOH used at equivalence point = 30 mL

2) For pH titration curve (for example strong acid and weak base) we observe a rapid change in pH near equivalence point.

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