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

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell