It takes 38.65 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?

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Diorsimmons Diorsimmons · Answer 1 · 2020-05-14T17:36:21+02:00

Answer:

0.138 M

Explanation:

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topeadeniran2 topeadeniran2 · Answer 2 · 2021-08-17T15:28:25+02:00

The molar concentration of the barium hydroxide solution is 0.0692M

2HCl(aq) + Ba(OH)₂(aq) = 2H₂O(l) + BaCl₂(aq)

It should b noted that for one mole of Ba(OH)₂, 2 moles of HCl are needed.

M₁V₁ = 2M₂V₂

where,

M₁ = Moles of HCl

M₂ = moles of Ba(OH)₂

V₁ = Volume of HCl

V₂ = Volume of Ba(OH)₂

M₁V₁ = 2M₂V₂

(0.0895 × 38.65) = (2 × M₂ × 25)

= (0.0895 × 38.65) / 50M₂

M₂ = (0.0895 × 38.65) / 50

M₂ = 3.459175/50

M₂ = 0.0691835

M₂ = 0.0692M

Therefore, the molar concentration of the barium hydroxide solution is 0.0692M

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