# 25 ml of a solution of barium hydroxide on titration with 0.1 molar solution of hydrochlroric acid gave a titre value of 35 ml . The molarity of sodium hydroxide is ?

Apr 29, 2017

You mean the molarity of the parent $\text{barium hydroxide}$ solution........

#### Explanation:

We assess the following stoichiometric equation:

$B a {\left(O H\right)}_{2} + 2 H C l \left(a q\right) \rightarrow B a C {l}_{2} \left(a q\right) + 2 {H}_{2} O \left(l\right)$.

And thus 2 equiv acid are required to neutralize each equiv barium hydroxide.

Now, $\text{concentration"="moles of solute"/"volume of solution}$, i.e. $C = \frac{n}{V}$, there were $0.1 \cdot m o l \cdot {L}^{-} 1 \times 0.035 \cdot L = 3.5 \times {10}^{-} 3 \cdot m o l$ WITH RESPECT to hydrochloric acid.......

And, thus, by the given stoichiometry, there was an initial concentration of .......

$\frac{3.5 \times {10}^{-} 3 \cdot m o l \times \frac{1}{2}}{0.025 \cdot L} = 0.070 \cdot m o l \cdot {L}^{-} 1$ with respect to the PARENT $B a {\left(O H\right)}_{2}$ solution. And I would like you to check on the solubilities of barium hydroxide to see if the question actually drew from experimental data.