Question

Assume that the reaction of aqueous hydrobromic acid solution and potassium hydroxide base undergoes a complete neutralization reaction.
a. Write a balanced chemical equation.

b. How many grams of water can be produce from the complete reaction of excess hydrobromic acid and 55.4 mL of 0.685 M potassium hydroxide solution, assuming that potassium hydroxide is the limiting reactant?

A solution of hydrobromic acid is formed by dissolving 5.00 grams in enough water to make 1.5 L solution.

c.. What was the molarity of this solution?

d. What is the pH of this solution?

Answer 1

Answer:

a.

$HBr + KOH → KBr + H _{2} O$

b.

$1000 \: ml \: contains \: 0.685 \: moles \\ 55.4 \: ml \: contains \: ( \frac{55.4 \times 0.685}{1000} ) \\ = 0.038 \:moles \\ 1 \: mole \: of \: hydrobromic \: acid \: produces \: 1 \: mole \: of \: water \\ 0.038 \: moles \: produce \: (0.038 \times 1) \\ = 0.038 \: moles \\ 1 \: mole \: of \: water \: weighs \: 18 \: g \\ 0.038 \: moles \: weighs \: (0.038 \times 18) \: g \\ = 0.684 \: g$

c.

0.042 M

d.

1.4