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Factors Affecting Boiling Point

19. Freezing ...

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19. Freezing point of 100 g water decreases by 0.15^° C when 1 g monobasic acid is added in water. If 60 m of N / 20 NaOH is required for the complete neutralization of 0.5 g of the same acid, then the degree of dissociation of acid will be (Kf for water = 1.86 K/molal)

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Q. 1g of a monobasic acid in 100 g water lowers the freezing point by

{0.168}^{o}

C. If 0.2 g of the same acid requires 15 ml of

\frac{N}{10}

alkali solution for complete neutralization, the degree of dissociation of acid is nearly:

K_{f}

H_{2} O = 1.86 K k g m o l^{- 1})

Q. 1.5 g of a monobasic acid, when dissolved in 150g of water, lowers the freezing point by

{0.165}^{\circ}

C. 0.5 g of the same acid when titrated, after dissolution in water, requires 37.5 ml of N/10 alkali. Calculate the degree of dissociation of the acid ?(

K_{f}

{1.86}^{\circ}

^{- 1}) .

1.0 g

of a monobasic acid

H A

100 g

water lowers the freezing point by

0.155 K

0.75 g

, of same acid requires

15

N / 5 N a O H

solution for complete neutralisation then %, degree of ionization if acid is (

K_{f} o f H_{2} O = 1.86 K k g m o l^{- 1}

Q. 1.0 g of a weak monobasic acid (

H A

), when dissolved in 150 mL water, lowers the freezing point by

{0.186}^{o} C

. Also 1.0 g of the same acid required 125 mL of a 0.10N Nate solution for complete neutralisation. Determine dissociation constant

(k_{a})

of the weak acid.

k_{f}

of water is 1.86 K kg

m o l^{- 1}

Q. 2.5 g of a monobasic acid when dissolved in 100 g of water elevates the boiling point of the solution by

{0.256}^{\circ} C

. If 0.5 g of the acid requires 8 milliequivalents of NaOH for complete neutralisation, then the degree of dissociation of the acid is: [

K_{b}

= 0.512 K k g m o l^{- 1}

]

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