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

a.

`HBr + KOH → KBr + H _(2) O`

b.

`1000 \: ml \: contains \: 0.685 \: moles \\ 55.4 \: ml \: contains \: ( (55.4 * 0.685)/(1000) ) \\ = 0.038 \:moles \\ 1 \: mole \: of \: hydrobromic \: acid \: produces \: 1 \: mole \: of \: water \\ 0.038 \: moles \: produce \: (0.038 * 1) \\ = 0.038 \: moles \\ 1 \: mole \: of \: water \: weighs \: 18 \: g \\ 0.038 \: moles \: weighs \: (0.038 * 18) \: g \\ = 0.684 \: g`

c.

0.042 M

d.

1.4