In your lab you fill the burette with 0.10 M NaOH and the conical flask with 25.0 mL of 0.10 M HCl. The indicator turns from colourless to pink at the equivalence point.
Formula Sheet
n = C × VpH = −log[H⁺]Kw = [H⁺][OH⁻] = 10⁻¹⁴How many moles of HCl are in the 25.0 mL flask?
What volume of 0.10 M NaOH is needed to reach the equivalence point?
What is the pH at the equivalence point of this strong acid–strong base titration?
Which indicator is MOST suitable for this titration (equivalence at pH 7)?