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17 April, 23:42

Can Magnesium hydroxide be used as the base for this titration? Why or why not? 5. Describe the procedure that you will follow to prepare 250 ml of a. 100 M soliution of KHP. 6. 25.0 ml of. 100M KHP is required to neutralize 10.0 ml of barium hydroxide. Find the molarity of the barium hydroxide solution.

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  1. 18 April, 01:22
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    A.

    Yes

    B.

    2KHP + Mg (OH) 2 = 2KOH + Mg (HP) 2

    KHP is an acidic salt which reacts with Mg (OH) 2 which is a base via double displacement/decomposition reaction.

    C.

    • One approach is to prepare the solution volumetrically using KHP crystals.

    • Preparing 1 liter of 0.1 M KHP you would add 0.1 moles of KHP

    Molar mass of KHP (C8H5KO4)

    = (12*8) + (5*1) + 39 + (16*4)

    = 204 g/mol

    Number of moles = mass/molar mass

    = 20.4/204

    = 0.1 mol.

    • This is added to a 1 liter volumetric flask, add deionized water until near the fill line, stopper and mix

    D.

    Number of moles = molar concentration * volume

    = 0.025 * 0.100

    = 0.0025 mol

    Equation for the reaction:

    Ba (OH) 2 + 2KHP - -> Ba (KP) 2 + 2H2O

    1 mole of Ba (OH) 2 reacted with 2 moles of KHP. By stoichiometry,

    Number of moles of Ba (OH) 2 = 0.0025/2

    = 0.00125 mol.

    Molarity = number of moles/volume

    = 0.00125/0.01

    = 0.125 M of Ba (OH) 2.
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