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16 September, 08:58

An aqueous solution of potassium hydroxide is standardized by titration with a 0.122 M solution of hydrobromic acid. If 22.1 mL of base are required to neutralize 18.8 mL of the acid, what is the molarity of the potassium hydroxide solution?

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  1. 16 September, 09:04
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    The molarity of the potassium hydroxide solution is 0.104 M

    Explanation:

    Step 1: Data given

    Molarity of hydrobromic acid (HBr) = 0.122 M

    Volume of potassium hydroxide (KOH) = 22.1 mL = 0.0221 L

    Volume of hydrobromic acid = 18.8 mL = 0.0188 L

    Step 2: The balanced equation

    HBr (aq) + KOH (aq) → KBr (aq) + H2O (l)

    Step 3: Calculate moles of HBr

    Moles HBr = molarity HBr * volume HBr

    Moles HBr = 0.122 M * 0.0188 L

    Moles HBr = 0.0022936 moles

    Step 4: Calculate molarity of KOH

    We need 0.0022936 moles of KOH to neutralize the HBr

    Molarity = moles / volume

    Molarity KOH = 0.0022936 moles / 0.0221 L

    Molarity KOH = 0.104 M

    The molarity of the potassium hydroxide solution is 0.104 M
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