Aqueous barium hydroxide, $\text{Ba(OH)}_2$, is allowed to react with dilute nitric acid, $\text{HNO}_3$. This produces aqueous barium nitrate, $\text{Ba(NO}_3)_2$, together with water. During a titration, $15.2\,\text{cm}^3$ of $0.75\,\text{mol dm}^{-3}$ aqueous barium hydroxide is needed to neutralise $20.0\,\text{cm}^3$ of dilute nitric acid. Calculate the concentration of the nitric acid.
- A$0.29\,\text{mol dm}^{-3}$
- B$0.57\,\text{mol dm}^{-3}$
- C$1.14\,\text{mol dm}^{-3}$
- D$2.03\,\text{mol dm}^{-3}$