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10 May, 02:54

A chemist dissolves 156. mg of pure hydrobromic acid in enough water to make up 220. mL of solution.

Calculate the pH of the solution.

Be sure your answer has the correct number of significant digits.

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Answers (2)
  1. 10 May, 03:36
    0
    The pH of the solution is 2.06

    Explanation:

    Step 1: Data given

    Mass of hydrobromic acid (HBr) = 156 mg = 0.156 grams

    Molar mass HBr = 80.91 g/mol

    Volume of the solution = 220 mL = 0.220 L

    Step 2: Calculate moles HBr

    Moles HBr = mass HBr / molar mass HBr

    Moles HBr = 0.156 grams / 80.91 g/mol

    Moles HBr = 0.00193 moles

    Step 3: Calculate moles H+

    For 1 mol HBr we have 1 mol H+

    For 0.00193 moles HBr we have 0.00193 moles H+

    Step 4: Calculatemolarity of H+

    Molarity H + = moles H + / volume

    Molarity H + = 0.00193 moles / 0.220 L

    Molarity H + = 0.00877 M

    Step 5: Calculate the pH

    pH = - log[H+]

    pH = - log (0.00877)

    pH = 2.06

    The pH of the solution is 2.06
  2. 10 May, 05:29
    0
    Answer: 2.06

    Explanation:

    m=156mg=0.156g

    Volume=220mL=0.22L

    Molar mass = 80.91g/mol

    Mole = reacting mass / molar mass

    Mole of HBr=0.156/80.91

    Mole of HBr=0.00193moles

    Since H+Br-

    Therefore, one mole of H + will give 1*0.00193

    H+=0.00193moles

    The molarity of H + in 0.22L = 0.00193/0.22

    Molarity of H + = 0.00876mol/L

    Since PH = - log (H+)

    PH = - log (0.00876)

    PH=2.06
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