In an acid-base titration, a student uses 21.35 mL of 0.150 M NaOH to neutralize 25.00 mL of H2SO4. How many moles of acid are in the flask?

There are 0.006 moles of acid in the flask.

Explanation:

Given: = 21.35 mL,         = 0.150 M

= 25.0 mL,           = ?

Formula used to calculate molarity of is as follows.

Substitute the values into above formula as follows.

As molarity is the number of moles of a substance present in a liter of solution.

Total volume of solution =

= 21.35 mL + 25.0 mL

= 46.36 mL  (1 mL = 0.001 L)

= 0.04636 L

Therefore, moles of acid required are calculated as follows.

Thus, we can conclude that there are 0.006 moles of acid in the flask.

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