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Number of moles of a solute per kilogram...

Number of moles of a solute per kilogram of a solvent is called

A

Mole fraction

B

Molality

C

Molarity

D

Molar mass

Text Solution

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Refer solved Exampe 32 (page 36)
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The number of moles of solute per kg of a solvent is called its :

When the concentration is expressed as the number of moles of a solute per kg of solvent it is known as

State Raoult's law, If DeltaT is the elevation in boiling point of a solvent and m is no. of moles of solute per kilogram of solvent. What is the relationship between DeltaT and m ?

What is the molality of a solution made by dissolving 3.42 g of table sugar (sucrose, C_(12H_(22)O_(11)) in 50.0 mL of water? Strategy: Molality is the number of moles of solute dissolved per kilogram of solvent. Thus, we must find how many moles are present in 3.42 g of sucrose and how many kilograms are contained in 50.0 mL of water.

Molality : It is defined as the moles of the solute pressent in 1 kg of the solvent . It is denoted by m. Molality(m) =("Number of moles of solute")/("Number of kilograms of the solvent") let w_(A) grams of the solute of molecular mass m_(A) be present in w_(B) grams of the solvent, then: Molality(m) = (w_(A))/(m_(A)xxw_(B))xx1000 Relation between mole fraction and molality: X_(A)=(n)/(N+n) "and" X_(B)=(N)/(N+n) (X_(A))/(X_(B))=(n)/(N)=("Moles of solute")/("Moles of solvent")=(w_(A)xxm_(B))/(w_(B)xxm_(A)) (X_(A)xx1000)/(X_(B)xxm_(B))=(w_(A)xx1000)/(w_(B)xxm_(A))= m or (X_(A)xx1000)/((1-X_(A))m_(B))=m If the mole fraction of a solute is changed from (1)/(4) "to" (1)/(2) in the 800 g of solvent then the ratio tof molality will be:

Molality : It is defined as the moles of the solute pressent in 1 kg of the solvent . It is denoted by m. Molality(m) =("Number of moles of solute")/("Number of kilograms of the solvent") let w_(A) grams of the solute of molecular mass m_(A) be present in w_(B) grams of the solvent, then: Molality(m) = (w_(A))/(m_(A)xxw_(B))xx1000 Relation between mole fraction and molality: X_(A)=(n)/(N+n) "and" X_(B)=(N)/(N+n) (X_(A))/(X_(B))=(n)/(N)=("Moles of solute")/("Moles of solvent")=(w_(A)xxm_(B))/(w_(B)xxm_(A)) (X_(A)xx1000)/(X_(B)xxm_(B))=(w_(A)xx1000)/(w_(B)xxm_(A))= m or (X_(A)xx1000)/((1-X_(A))m_(B))=m The mole fraction of the solute in the 12 molal solution of CaCo_(3) is :

Molality : It is defined as the moles of the solute pressent in 1 kg of the solvent . It is denoted by m. Molality(m) =("Number of moles of solute")/("Number of kilograms of the solvent") let w_(A) grams of the solute of molecular mass m_(A) be present in w_(B) grams of the solvent, then: Molality(m) = (w_(A))/(m_(A)xxw_(B))xx1000 Relation between mole fraction and molality: X_(A)=(n)/(N+n) "and" X_(B)=(N)/(N+n) (X_(A))/(X_(B))=(n)/(N)=("Moles of solute")/("Moles of solvent")=(w_(A)xxm_(B))/(w_(B)xxm_(A)) (X_(A)xx1000)/(X_(B)xxm_(B))=(w_(A)xx1000)/(w_(B)xxm_(A))= m or (X_(A)xx1000)/((1-X_(A))m_(B))=m What is the quantity of water that should be added to 16 g methonal to make the mole fraction of methonal as 0.25?

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  2. Calculate the molarity of a solution containing 5 g of NaOH in 450 mL...

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  3. Converting molarity to mole fraction, mass percent and molality: A 0.7...

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  4. (a) Define the terms osmosis and osmotic pressure. Is the osmotic pres...

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  5. Number of moles of a solute per kilogram of a solvent is called

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  6. The van’t Hoff factor can be expressed as :

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  7. The vapour pressure of pure benzene at a certain temperature is 0.850 ...

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  8. The boiling a point of benzene is 353.23K. When 1.80 g of a non-volati...

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  9. (i) Prove that depression in freezing point is a colligative property...

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  10. (i) Prove that osmotic pressure is a colligative property. (ii) Calc...

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  11. Vapor pressure of a solution of Volatile components and composition of...

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  12. (a) Define the following terms: (i) Molarity (ii) Molal elevation ...

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  13. (a) Define the following terms : (i) Mole fraction (ii) Ideal solu...

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  14. (a) Explain the following : (i) Henry's law about dissolution of a ...

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  15. (a) State Raoult law for a solution containing volatile components. ...

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  16. A solution of glucose ("molar mass"= 180g mol^(-1)) in water is labell...

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  17. (a) Define the following terms: (i) Molarity (ii) Molal elevation ...

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  18. What type of devation is shown by a mixture of ethnol and acetone ? Wh...

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  19. (a) A 10% solution (by mass) of sucrose in water has freezing point of...

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  20. 30 g of urea (M=60g mol^(-1)) is dissolved in 846g of water. Calculate...

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