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.

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.