Question

Hydrobromic acid solution of unknown concentration is titrated with a 0.500M LiOH solution.

20.00mL of the acid are poured into an Erlenmeyer flask.

40.00mL of the base solution is required to reach the equivalence point.

What is the molarity of the Hydrobromic acid solution?

Answer 1

1.00 M

Step-by-step explanation:

Step 1: Write the balanced equation

HBr + LiOH ⇒ LiBr + H₂O

Step 2: Calculate the reacting moles of lithium hydroxide

40.00 mL of 0.500 M solution react. The reacting moles of LiOH are:

`40.00 * 10^(-3) L * (0.500mol)/(L) = 0.0200 mol`

Step 3: Calculate the reacting moles of hydrobromic acid

The molar ratio of HBr to LiOH is 1:1. The reacting moles of hydrobromic acid are 1/1 × 0.0200 mol = 0.0200 mol.

Step 4: Calculate the molarity of hydrobromic acid

0.0200 moles of HBr are in 20.00 mL of the solution. The molarity of the hydrobromic acid solution is:

`M= (0.0200 mol)/(20.00 * 10^(-3) L ) =1.00 M`