Question

Be sure to answer all parts. Find the pH of the equivalence point and the volume (mL) of 0.0895 M KOH needed to reach the equivalence point in the titration of 23.4 mL of 0.0390 M HNO,. Volume: mL KOH pH =

Answer 1

pH = 7

Volume of 0.0895 M KOH = 2.15 mL

Step-by-step explanation:

(Assuming HNO, should be HNO₃)

The balanced chemical equation is:

HNO₃ + KOH ⇒ H₂O + KNO₃

At the equivalence point, the amount of KOH added is equivalent to the amount of HNO₃ present, which is calculated as follows:

(23.4mL)(0.0390mol/L) = 0.9126 mmol HNO₃

Since HNO₃ and KOH react in a 1:1 molar proportion, 0.9126 mmol of KOH is required to reach the equivalence point. Therefore, the volume of KOH solution required is:

(0.1926mmol) ÷ (0.0895mol/L) = 2.15 mL KOH solution

The HNO₃ and KOH react completely and neither is in excess, so only the products of the reaction remain (H₂O and KNO₃). Since KNO₃ can be considered a neutral salt, the pH at the equivalence point is 7.