Question

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6. (6pt) You measure 5.1050 g of KHP and dissolve it in 50mL of distilled water. The molar mass of KHP is 204.2 g/mole a. what is molarity of KHP solution? 5.1050 b. What is molarity of the NaOH if it took 20 mL to reach end point of titration?

Answer 1

Given Data weight of KHP = 5.1050 g Volume of distilled water = 50 ml Molar mass of KHP = 204.2 Molarity of KHP = ? formula for calculation of molarity (a) Molarity is defined as the number of moles of solute present in one litre of solution. Molarity = number of moles/Litre of solution Molarity = omega t/m omega times 1/V (volume in litres) Molarity = omega t/m middot omega times 1000/v (volume in ml) Molarity = 5.1050/204.2 times 1000/50 = 0.5 M (b) The Reaction is HK C_8 H_4 O_4 + NaOH rightarrow Na K C_8 H_4 O_4 + H_2 O (KHP) one mole + one mole rightarrow one mole Number of moles KHP = omega t of KHP/moles mass of KHP = 5.1050/204.2 = 0.025 moles From the Above Reaction one mole KHP reacts with one mole NaOH so 1 mole KHP = 1 mole NaOH Now number of moles of KHP = 0.025 moles rightwardsdoublearrow 0.025 moles KHP = 0.025 moles NaOH Given volume of NaOH = 20 ml = 20 times 10^-3 Lt Molarity = number of moles/Volume of solution in Litre