Question

A chemist conducts a titration on 50 mL of a solution of hydrobromic acid (HBr) of unknown strength. She finds the pH reaches the equivalency point with the addition of 15 mL of 0.30 M sodium hydroxide (NaOH). What is the concentration of the HBr solution?

Answer 1

The concentration of the HBr would be 0.09 M

What are stoichiometric problems?

First, let us look at the equation of the reaction:

$HBr + NaOH --- > NaBr + H_2O$

The mole ratio of HBr to NaOH is 1:1.

Mole of 15 mL, 0.30 M NaOH = 0.30 x 15/1000 = 0.0045 moles

Equivalent mole of HBr - 0.0045 moles

Molarity of HBr = mole/volume = 0.0045/50/1000 = 0.09 M

More on stoichiometric problems can be found here: brainly.com/question/15047541

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