Question

An aqueous solution of hydrobromic acid is standardized by titration with a 0.189 m solution of calcium hydroxide. If 27.8 ml of base are required to neutralize 12.7 ml of the acid, what is the molarity of the hydrobromic acid solution?

Answer 1

The molarity of the hydrobromic acid solution is approximately 0.437 M.

Step-by-step explanation:

The molarity of hydrobromic acid solution can be calculated using the equation:

HBr(aq) + Ca(OH)2(aq) → CaBr2(aq) + 2H2O(l)

In the given equation, the mole ratio between hydrobromic acid (HBr) and calcium hydroxide (Ca(OH)2) is 1:1. This means that for every mole of hydrobromic acid, one mole of calcium hydroxide is required to neutralize it.

Using the given data:

• Volume of base (Ca(OH)2) required = 27.8 mL
• Volume of acid (HBr) = 12.7 mL
• Concentration of base (Ca(OH)2) = 0.189 M

We can set up the following equation to calculate the molarity of the hydrobromic acid solution:

(27.8 mL)(0.189 M) = (12.7 mL)(x M)

Simplifying the equation, we find that the molarity of the hydrobromic acid solution is approximately 0.437 M.