Achemist dissolves 377.mg of pure potassium hydroxide in enough water to make up 130.ml of solution. calculate the ph of the solution. (the temperature of the solution is 25°c.) round your answer to 3 significant decimal places.

The answer to your question is pH = 1.36

Explanation:

Data

Mass = 377 mg of KOH

Volume = 130 ml

pH = ?

pH = -log[H⁺¹]

Process

1.- Calculate the moles of KOH

molecular mass of KOH = 39 + 16 + 1 = 56 g

                          56 g of KOH 1 mol of KOH

                         0.377 g KOH    x

                                x = (0.377 x 1) / 56

                                x = 0.0057 moles

2.- Calculate the concentration

Molarity = number of moles / volume

Molarity = 0.0057 / 0.13

Molarity = 0.044

3.- Calculate the pH of the solution

pH = - log [0.044]

pH = 1.36

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