A 4.00 cm34.00\text{ cm}^34.00 cm3 sample of a concentrated solution of nitric acid, HNO3\text{HNO}_3HNO3, was carefully diluted with distilled water. More water was then added until the final volume of the solution was 250 cm3250\text{ cm}^3250 cm3 (0.250 dm30.250\text{ dm}^30.250 dm3).
In an experiment, a student found that 25.0 cm325.0\text{ cm}^325.0 cm3 of this diluted nitric acid reacted completely with 15.00 cm315.00\text{ cm}^315.00 cm3 of barium hydroxide (Ba(OH)2\text{Ba(OH)}_2Ba(OH)2) solution with a concentration of 0.0500 mol/dm30.0500\text{ mol/dm}^30.0500 mol/dm3.
The equation for the reaction is:
2HNO3+Ba(OH)2→Ba(NO3)2+2H2O 2\text{HNO}_3 + \text{Ba(OH)}_2 \rightarrow \text{Ba(NO}_3)_2 + 2\text{H}_2\text{O} 2HNO3+Ba(OH)2→Ba(NO3)2+2H2OCalculate the amount, in moles, of barium hydroxide in the 15.00 cm315.00\text{ cm}^315.00 cm3 of barium hydroxide solution.
Use your answer to (i) to calculate the amount, in moles, of nitric acid in the 25.0 cm325.0\text{ cm}^325.0 cm3 of diluted acid.
Use your answer to (ii) to calculate the concentration, in mol/dm3\text{mol/dm}^3mol/dm3, of the diluted nitric acid.
Use your answer to (iii) to calculate the concentration, in mol/dm3\text{mol/dm}^3mol/dm3, of the original, concentrated nitric acid.
