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31 July, 12:56

In testing the effectiveness of an antacid compound, 20.0g of Hydrochloric Acid is mixed with 28.0g of Magnesium Hydroxide. will the base neutralize all of the acid? How much of which substance is in excess?

2HCL + Mg (OH) 2 - -> MgCl2 + 2H2O

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  1. 31 July, 16:05
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    The base will neutralize all of the acid. There will remain 12.0 grams of Mg (OH) 2 in excess.

    Explanation:

    Step 1: Data given

    Mass of Hydrochloric acid (HCl) = 20.0 grams

    Mass of Magnesium hydroxide (Mg (OH) 2)

    Molar mass of HCl = 36.46 g/mol

    Molar mass of Mg (OH) 2 = 58.32 g/mol

    Step 2: The balanced equation

    2HCL + Mg (OH) 2 → MgCl2 + 2H2O

    Step 3: Calculate moles of HCl

    Moles HCl = 20.00 grams / 36.46 g/mol

    Moles HCl = 0.5485

    Step 4: Calculate moles of Mg (OH) 2

    Moles Mg (OH) 2 = 28.00 grams / 58.32 g/mol

    Moles Mg (OH) 2 = 0.4801 moles

    Step 5: Determine the limiting reactant

    For 2 moles HCl we need 1 mol of Mg (OH) 2 to produce 1 mol of MgCl2 and 2 moles of H2O

    HCl is the limiting reactant. It will completely be consumed (0.5485 moles).

    Mg (OH) 2 is in excess. There will react 0.5485/2 = 0.27425 moles

    There will remain 0.4801 - 0.27425 = 0.20585‬ moles of Mg (OH) 2

    Remaining mass of Mg (OH) 2 = 0.20585 moles * 58.32 g/mol = 12.0 grams

    The base will neutralize all of the acid. There will remain 12.0 grams of Mg (OH) 2 in excess.
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