Ask Question
7 October, 14:57

A chemist must prepare 900.0mL of potassium hydroxide solution with a pH of 13.80 at 25°C. He will do this in three steps: Fill a 900.0mL volumetric flask about halfway with distilled water. Weigh out a small amount of solid potassium hydroxide and add it to the flask. Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits.

+3
Answers (1)
  1. 7 October, 17:32
    0
    The chemist needs 39 grams of potassium hydroxide

    Explanation:

    Step 1: Data given

    Volume = 900 mL = 0.9 L

    pH = 13.80

    Temperature = 25 °C

    Step 2: Calculate pOH

    pH + pOH = 14

    pOH = 14 - 13.80 = 0.20

    Step 3: Calculate [OH-]

    pOH = 0.20 = - log[OH-]

    [OH-] = 10^-0.20

    [OH-] = 0.631

    Step 4: calculate moles of KOH

    KOH is a strong base, this means [OH-] = [KOH]

    [KOH] = moles KOH / volume KOH

    moles KOH = [KOH] / volume KOH

    moles KOH = 0.631 / 0.9 L

    moles KOH = 0.701 moles

    Step 5: Calculate mass of KOH

    mass KOH = Number of moles KOH * Molar mass KOH

    mass KOH = 0.701 moles * 56.106 = 39.33 grams ≈ 39 grams

    The chemist must weight out 39 grams of potassium hydroxide
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “A chemist must prepare 900.0mL of potassium hydroxide solution with a pH of 13.80 at 25°C. He will do this in three steps: Fill a 900.0mL ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers