Assuming that an acetic acid solution is 12% by mass and that the density of the solution is 1.00 g/ml, what volume of 1 m naoh is needed to fully neutralize a 10 ml aliquot of the acetic acid solution

Explanation:

Let us assume that total mass of the solution is 100 g. And, as it is given that acetic acid solution is 12% by mass which means that mass of acetic acid is 12 g and 88 g is the water.

Now, calculate the number of moles of acetic acid as its molar mass is 60 g/mol.

    No. of moles =

                           =

                           = 0.2 mol

Molarity of acetic acid is calculated as follows.

              Density =

                 1 g/ml =

                    volume = 100 ml

Hence, molarity =

                           =

                           = 2 mol/l

As reaction equation for the given reaction is as follows.

So,          moles of NaOH = moles of acetic acid

Let us suppose that moles of NaOH are "x".

              (as 1 L = 1000 ml)

                        x = 20 L

Thus, we can conclude that volume of NaOH required is 20 ml.                    

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.