Question

It takes 32.35 mL of a 0.0895 M hydrochloric acid solution to reach the equivalence point in the reaction with 25.00 mL of barium hydroxide. 2HCl(aq) Ba(OH)2(aq) 2H2O(l) BaCl2(aq) What is the molar concentration of the barium hydroxide solution

Answer 1

Answer:

$M_{base}=0.0579M$

Explanation:

Hello there!

In this case, according to the given information in the undergoing chemical reaction, it is possible for us to realize that barium hydroxide reacts with hydrochloric acid in a 1:2 mole ratio, which means that at the equivalence point, we have:

$2n_{base}=n_{acid}$

That can be written in terms of molarity and volume:

$2M_{base}V_{base}=M_{acid}V_{acid}$

Thus, we solve for the molarity of the barium hydroxide to obtain:

$M_{base}=\frac{M_{acid}V_{acid}}{2V_{base}} \\\\M_{base}=\frac{0.0895M*32.35 mL}{2*25.00mL}\\\\M_{base}=0.0579M$

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