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
anor277
Apr 29, 2017

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

Explanation:

We assess the following stoichiometric equation:

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"="moles of solute"/"volume of solution", i.e. C=n/V, there were 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 .......

(3.5xx10^-3*molxx1/2)/(0.025*L)=0.070*mol*L^-1 with respect to the PARENT 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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