# A solution of sodium hydroxide is standardized against potassium hydrogen phthalate. From the following data, calculate the molarity of NaOH solution? (See details below)

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Mass of KHP used: 0.4536 g

Buret reading before titration: 0.23 ml

Buret reading

How many liters of the standardized NaOH will be needed to neutralize a water solution with 0.1453 g Oxalic acid dissolved?

Mass of KHP used: 0.4536 g

Buret reading before titration: 0.23 ml

Buret reading

How many liters of the standardized NaOH will be needed to neutralize a water solution with 0.1453 g Oxalic acid dissolved?

##### 1 Answer

We need (i) a stoichiometric equation........

#### Explanation:

We need (i) a stoichiometric equation:

And (ii) stoichiometric quantities of

Of course, you have not quoted a volume of titrant; i.e. the end reading on the burette. And thus we cannot assess the molarity of the sodium hydroxide solution. Once such a volume is reported, we make the following calculation:

A stoichiometrically balanced equation is absolutely basic to such acid/base titrations.

For the next reaction with the standardized titrant, we follow the stoichiometric equation: