How much of 0.5 M HNO3 is necessary to titrate 25.0 mL of 0.05 M KOH
solution to the endpoint?
Show all work using the titrations formula.

2.5 ml of 0.5 M HNO3 is necessary to titrate 25.0 mL of 0.05 M KOH

solution to the endpoint

Explanation:

To calculate the volume of acid, we use the equation given by neutralization reaction:

where,

are the n-factor, molarity and volume of acid which is

are the n-factor, molarity and volume of base which is KOH.

We are given:

Putting values in above equation, we get:

Thus 2.5 ml of 0.5 M HNO3 is necessary to titrate 25.0 mL of 0.05 M KOH

solution to the endpoint

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