Question

What is the ph at the equivalence point when 0.10 m hno3 is used to titrate a volume of solution containing 0.30 g of koh?

Answer 1

pH at equivalence point will be 7

Step-by-step explanation:

• 
  `HNO_(3)` is a strong acid and KOH is a strong base. Hence a neutral salt would appear from acid-base reaction between them.
• Acid-base reaction:
  `HNO_(3)+KOH\rightarrow KNO_(3)+H_(2)O`
• At equivalence point,
  `KNO_(3)` and water exists in medium.
• As
  `KNO_(3)` is a neutral salt therefore pH of medium will be equal to 7 (neutral).
• So, pH at equivalence point will be 7.

Answer 2

Answer;

pH = 7

Explanation;

• HNO3 is a strong acid. KOH is a strong base. At the equivalence point, the solution will be neutral.
• Therefore; the pH at the equivalence point when 0.10 m HNO3 is used to titrate a volume of solution containing 0.30 g of KOH will be 7.
• The neutralization of a strong base with a strong acid gives a salt solution at the equivalence point. The salt contains ions that do not change the pH of water.