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 ?

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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 ?

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Answer 1 · 2017-04-29T15:01:03

You mean the molarity of the parent $barium hydroxide$ $"barium hydroxide"$ solution........

Explanation:

We assess the following stoichiometric equation:

$B a {(O H)}_{2} + 2 H C l (a q) \to B a C l_{2} (a q) + 2 H_{2} O (l)$ $Ba(OH)_2 + 2HCl(aq) rarr BaCl_2(aq) + 2H_2O(l)$ .

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

Now, $concentration = \frac{moles of solute}{volume of solution}$ $"concentration"="moles of solute"/"volume of solution"$ , i.e. $C = \frac{n}{V}$ $C=n/V$ , there were $0.1 \cdot m o l \cdot L^{- 1} \times 0.035 \cdot L = 3.5 \times 10^{- 3} \cdot m o l$ $0.1*mol*L^-1xx0.035*L=3.5xx10^-3*mol$ WITH RESPECT to hydrochloric acid.......

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

$\frac{3.5 \times 10^{- 3} \cdot m o l \times \frac{1}{2}}{0.025 \cdot L} = 0.070 \cdot m o l \cdot L^{- 1}$ $(3.5xx10^-3*molxx1/2)/(0.025*L)=0.070*mol*L^-1$ with respect to the PARENT $B a {(O H)}_{2}$ $Ba(OH)_2$ solution. And I would like you to check on the solubilities of barium hydroxide to see if the question actually drew from experimental data.

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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 ?

1 Answer

Explanation:

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