The amount of sulphuric acid required by a student to perform an experiment was 1500 ml of 2.30M. Explain how you would prepare the required amount of acid to perform an experiment if the label on the available concentrated commercial sulphuric acid bottle indicates 96.4% by mass acid with specific gravity as 1.84?

2 answers

1.5L*2.30M= moles

Moles*98.079g/mole= mass of H2SO4

Mass of H2SO4/total=0.964 and mass of H2SO4/0.964= Y

Y/1.84= volume needed

But there is no such thing as a 1.5L volumetric flask. So you would need to perform this with a 2L volumetric flask and use 2L for your initial calculations. Just measure out only 1.5L to be used in your experiment. Add the volume needed and then add water. Shake well.
Didn’t pay attention. This is acid, so you add water, acid then water to the mark. Shake well. ===> safer that way.