(a) Concentrated acid H2SO4, has a density of 1.8 g/ml and contains 49% acid by weight. Compute molarity of the solution.
(b) What is the molarity of a solution which is prepared by dissolving 100 ml of concentrated H2SO4, in part (a) in sufficient water to make 500 ml of solution?
pls explain in detail (b).
Answers
Explanation:
a) H2so4 = 98 U
b) Assuming that you add 100ml of the conc. acid to 900ml of water in order to dilute the solution to 1000ml, then your final concentration and normality will be 10% that of the original. All you do is look at the concentration on the bottle and divide by 10 - you shouldn’t even need a calculator (if you do - try learning your times tables).
Since the original concentration / normality is not mentioned, the calculation cannot go further. However…
…if your original sulfuric acid is 98%, then the original molarity would be 18.4M and the Normality would be 36.8N, making the diluted solution 1.84 M and 3.68N respectively. These values are theoretical and unlikely to be accurate for your sample. Rounding values down to whole numbers is probably more than adequate.