Giving the density of water at 16^°c is 1.0037mg/ml.Show how you will prepare 250mls of 0.4M H2SO4 solution at this temperature from a stock solution with a specific gravity of 1.84 and concentration of 98%w/w.

Answer 1

Note: You made a typo. You must have meant that the density of H2O @ 16 C is 1.0037 g/mL and not 1.0037 mg/mL.
Specific Gravity of stock H2SO4 solution is 1.84.
Therefore, density of stock H2SO4 = S.G x density H2O @ 16 C.
So density of stock H2SO4 = 1.84 x 1.0037 g/mL = 1.8468 which I will round to 1.85 g/mL.
Then M = 1.85 g/mL x 1000 mL x 0.98 x (1 mol H2SO4/98 g H2SO4) = 18.5 M. Now use the dilution formula of
mL1 x M1 = mL2 x M2
250 mL x 0.4 M H2SO4 = mL2 x 18.5 M H2SO4
Solve for mL2. Take that many mL of the stock, transfer to a 250 mL volumetric flask, add DI or distilled water to the flask to the mark, stopper, mix thoroughly, label. Done.