A chemistry student weighs out 0.09666 g of phosphoric acid (H3PO4), a triprotic acid, into a 250.volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000 M NaoH solution. Calculate the volume of NaoH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits.

14.62 ml

Explanation:

Molarity is defined as the number of moles of solute dissolved per liter of the solution.

where,

n= moles of solute  

= volume of solution in ml = 250 ml

Now put all the given values in the formula of molarity, we get

To calculate the volume of base, 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 NaOH.

We are given:

Putting values in above equation, we get:

Thus the volume of NaOH solution the student will need to add to reach the final equivalence point is 14.62 ml

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