A 4.36 g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid-base indicator is added, and the resulting solution is titrated with 2.50 M solution of HCl. The indicator changes colour, signalling that the equivalence point has been reached after 17.0 mL of the hydrochloric acid solution has been added.
Solution:
An Unknown Solute which is an Alkali Metal Hydroxide is dissolved in Water to Prepare a Solution.This Solution is Titrated with HCl Solution using an Acid-Base Indicator.
i) Here, 4.36g of Unknown Solute is Added.
Volume of HCl Added to the Aqueous Solution of the Solute to achieve Equivalence Point = 17ml = 0.017L.
Concentration of HCl = 2.5M
The Equivalence Point in an Acid- Base Titration is a Point where the Amount of Acid = Amount of Base in Solution.
So Number of Moles of Base Solute= Number of Moles of HCl.
Moles of Solute (n) = C×V = 2.5M× 0.017L = 0.0425moles.
Mass of Solvent(Water) = 100ml = 100g = 0.1Kg
Therefore Molality of Solution(m) = Moles of Solute÷ Mass of Solvent
m = 0.0425÷ 0.1 = 0.425 Kg^-1.
Mass of Solution = Mass of Solute + Mass of Solvent = 4.36 + 100 = 104.36g.
Therefore, Mass Percentage of the Solute (M%)= (Mass of Solute ÷Mass of Solution)×100
M% = (4.36÷104.36) ×100 = 4.18%.
ii) The Change in Boiling Point of Solution can be determined from the Molality of Solution by the following Equation:
∆Tb = Kb × m, where Kb is Molal Boiling Point Elevation Constant of Water (0.51°C/m) and m is the Molality of Solution.
Initial Temperature of Water = 100°C.
Tf is the Final Temperature of Solution after Addition of Solute
So; Tf - Ti = 0.51 × 0.425.
Tf - 100°C = 0.217.
Therefore, Tf = 0.217 + 100 = 100.217°C.
Therefore the Final Temperature of Solution after Adding the Solute is Increasing and is not a Significant Increase.
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