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Addition of non-volatile solute to solvent lowers its vapoure pressure. Therefore, the vapour pressure of a solution (i.e, V.P. of solvent in a solution) is lower than that of pure solvent in a solution) is lower than that of pure solvent, at the same temperature. A higher temperature is needed to raise the vapour pressure upto one atmosphere pressure, when boiling point is attined. However, increase in b.pt. is small . for example, 0.1 molal aqueous sucrose solution boils at 10.05^(@)C Sea water, an aqueous solution, which is rich in Na^(+) and Cl^(-) ions, freezes about 1^(@)C lower than frozen water . At the freezing point of a pure-solvent, the reates at which two molecule stick together to form the solid and leave it to return to liquid are equal when solute is present. Few solvent molecules are in contact with surface of solid. However, the rate at which the solvent molecules leave, surface of solid remains unchanged. That is why, temperature is lowered to restore the equalibrium. The freezing depression in a dilute solution is proportional to molality of the solute. The freezing point of a 5g CH_(3)COOH(aq) per 100 g water is -1.576^(@)C . Then van't Hoff factor ( K_(f) of water = 1.86 K "mol"^(-1) kg ) :

(a). What effect does the concentration of H^(+) (aq) ions have on the nature of a solution? (b). What effect does the concentration of OH^(-) ions have on the nature of a solution? (c). Someone put some universal indicator paper into vinegar. The pH is 3. What does this tell you about the vinegar? (d). Someone put some universal indicator paper onto wet soap. the pH is 8. What does this tell you about the soap? (e). State whether a solution is acidic, alkali or neutral if its pH is: (i) 9 (ii) 4 (iii) 7 (iv) 1 (v) 10 (vi) 3.

Addition of non-volatile solute to a solvent always inceases the colligative properties such as osmotic pressure, DeltaP, DeltaT_(b) and DeltaT_(f) . All these colligative properties are direactly propertional to molality if solutions are dilute. The increase in colligative properties on addition of non-volatile solute is due to incease in number of solute particles. For different aqueous solutions of 0.1 N NaCl, 0.1 N urea, 0.1 N Na_(2)SO_(4) and 0.1 N Na_(3)PO_(4) solution at 27^(@)C , the correct statement are : 1g mixture of glucose and urea present in 250 mL aqueous solution shows an osmotic pressure of 0.74 atm at 27^(@) C . Assuming solution to be dilture, which are correct ? (P) Percentage of urea in solute mixture is 17.6 (Q) Relative lowering in vapour pressure of this solutions is 5.41 xx 10^(-4) . (R) The solution will boil at 100.015^(@)C , if K_(b) of water is 0.5 K "molality"^(-1) (S) If glucose is replaced by same amount of sucrose, the solution will show higher osmotic pressure at 27^(@)C (T) If glucose is repalced by same amount of NaCl , the solution will show lower osmotic pressure at 27^(@)C .

A 50 mL sample of hard water containing Ca^(2+) and Mg^(2+) ions is titrated with 50 mL. 0.005 M EDTA solution at pH=10 , using eriochrome balck -T indicator to reach equivalence point. In a equal amount of hard water sample, Mg^(2+) ions are precipated as Mg(OH)_(2) by adding suitable amount of NaOH . the solution, after precipation of Mg(OH)_(2) , is strired and then titrated with EDTA solution using calcon as indicator, and it requires 10 mL of above EDTA solution to reach equivalence point. a. Calculate the strength of Ca^(2+) and Mg^(2+) ions present in hard water. b. Calculate the hardness due to Ca^(2+) ions in p p m of CaCO_(3) . c. Calculate the hardnesss due to Mg^(2+) ions in p p m of CaCO_(3) . d. Calculate the total hardness of water in p p m of CaCO_(3) .

100 mL sample of hard water is titrated with 500 mL of 0.001 MEDTA solution at pH=10 , using eriochrome black -T indicator to reach equivalence point. An equal another amount of hard water sample is boiles for 30 mi n . After filtration and cooling, the same sample is titrated with 200 mL of 0.001 M EDTA solution at pH=10 using Mg-EDTA complex solution and erichrome black -T indicator to reach equivalence point. a. Calculate the total hardness of water sample (temprary +permanent) in p p m of CaCO_(3) . b. Calculate the permanent hardness of water sample is p p m of CaCO_(3) . c. Calculate the temporary hardness of water sample is p p m of CaCO_(3) .

(i) Four samples A, B, C and D change the colour of pH paper or solution to Green, Reddish-pink, Blue and Orange. Their pH was recorded as 7, 2, 10.5 & 6 respectively. Which of the samples has the highest amount of Hydrogen ion concentration? Arrange the four samples in the decreasing order of their pH. (ii) Rahul found that the Plaster of Paris, which he stored in a container, has become very hard and lost its binding nature. What is the reason for this? Also, write a chemical equation to represent the reaction taking place (iii) Give any one use of Plaster of Paris other than for plastering or smoothening of walls.