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Predict the osmotic pressure order for t...

Predict the osmotic pressure order for the following:
(I) `0.1 N` urea
(II) `0.1 N NaCl`
(III) `0.1 N Na_(2)SO_(4)`
(IV) `0.1 N Na_(3)PO_(4)`

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The correct Answer is:
(a) Urea `ltNaClltNa_(2)SO_(4)ltNa_(3)PO_(4)` (b) `6.15` atm
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Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . The correct order of osmotic pressure for the solutions : (I) 1N urea , (II) 1N NaCl (III) 1N Na_(2)SO_(4) , (IV) 1N Na_(3)PO_(4) is:

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 : (P) The order of osmotic pressure is, NaCl gt Na_(2)SO_(4) gt Na_(3)PO_(4) gt urea (Q) pi = (DeltaT_(b))/(K_(b)) xx ST for urea solution (R) Addition of salt on ice increases its melting point (S) Addition of salt on ice brings in melting earlier

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 .

The ionic stregth of Na^(+) on mixing 100 mL 0.1 NaCl and 100 mL 0.1 N Na_(2)SO_(4) is:

Out of the following three solutions, which has the highest freezing point and why ? (a) 0.1 M urea (b) 0.1 M BaCl_(2) (c) 0.1 M Na_(2) SO_(4)

Properties such as boiling point, freezing point, and vapour pressure of a pure solvent change when solute molecules are added to get homogenous solution. These are called colligative properties. Anwer the following questions: i.0.1 M ethanol ii. 0.1 m Ba_(3)(PO_(4))_(3) iii. 0.1 m Na_(2)SO_(4) Increasing order of freezing points

Correct order of freezing point of given solution I. 0.1 M glucose II. 0.2 M urea III.0.1 M NaCl IV. 0.05 M CaCl_2

If osmotic pressure of 1M urea is pi , what will be the osmotic pressure for 0.1 M NaCl?

Which is the correct relation between osmotic pressure of 0.1 M NaCl solution and 0.1 M Na_(2)SO_(4) solution ?

Arrange the following solutions in order of increasing osmotic pressure. Assume 100% isonisation for electrolytes: {:(1N NaCl,1N Na_(2)SO_(4),IN Na_(3)PO_(4),,),(I,II,III,,):}

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