A 5.00 cm3 sample of a concentrated solution of sulfuric acid, H2SO4\text{H}_2\text{SO}_4H2SO4, was carefully diluted with distilled water. More water was then added until the final volume of the solution was 500 cm3 (0.500 dm3).
In an experiment, a student found that 20.0 cm3 of this diluted sulfuric acid reacted completely with 25.00 cm3 of potassium hydroxide (KOH\text{KOH}KOH) solution with a concentration of 0.160 mol/dm3.
The equation for the reaction is:
2KOH+H2SO4→K2SO4+2H2O 2\text{KOH} + \text{H}_2\text{SO}_4 \rightarrow \text{K}_2\text{SO}_4 + 2\text{H}_2\text{O} 2KOH+H2SO4→K2SO4+2H2OCalculate the amount, in moles, of potassium hydroxide in the 25.00 cm3 of potassium hydroxide solution.
Use your answer to (i) to calculate the amount, in moles, of sulfuric acid in the 20.0 cm3 of diluted acid.
Use your answer to (ii) to calculate the concentration, in mol/dm3\text{mol/dm}^3mol/dm3, of the diluted sulfuric acid.
Use your answer to (iii) to calculate the concentration, in mol/dm3\text{mol/dm}^3mol/dm3, of the original, concentrated sulfuric acid.
