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59.6 ml of 0.303 m hydrobromic acid is added to 29.0 ml of calcium hydroxide, and the resulting solution is found to be acidic. 21.2 ml of 0.186 m barium hydroxide is required to reach neutrality. what is the molarity of the original calcium hydroxide solution?

Sagot :

Neetoo

The molarity of the original calcium hydroxide solution will be 0.176 molar.

First, we will write the chemical equations for both reactions:

  HBr + Ca(OH)₂  →  H₂O + CaBr₂

  HBr + Ba(OH)₂  →   H₂O + BaBr₂

Balance the chemical equations

  2HBr + Ca(OH)₂  →  2H₂O + CaBr₂

  2HBr + Ba(OH)₂  →  2H₂O + BaBr₂

Concentration of hydrobromic acid (HBr) = 59.6 ml x 0.303 M / 1000

Concentration of hydrobromic acid (HBr) = 0.0181 mol

Hence

  0.5 equivalent Ca or Ba hydroxide = 0.0181 mol x 0.5 mol

  0.5 equivalent Ca or Ba hydroxide = 0.00905 Moles

  Concentration of Barium hydroxide = 21.2 ml x 0.186 / 1000

  Concentration of Barium hydroxide = 0.00394 mol

  Concentration of Calcium hydroxide = 0.00905 - 0.00394

  Concentration of Calcium hydroxide = 0.00511 mol

Molar solution of Calcium hydroxide = 0.00511 x 1000 / 29.0 ml

Molar solution of Calcium hydroxide = 0.176 molar calcium hydroxide solution is needed.

You can also get help with molarity from the following question:

https://brainly.com/question/16587536

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