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.

14,16 18 reacts with group

your answer is c) plasma

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