Home
Class 11
CHEMISTRY
4.5g of urea (molar mass = 60g "mol"^(-1...

4.5g of urea (molar mass = 60g `"mol"^(-1)`) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

Text Solution

Verified by Experts

Mass of Urea = 4.5 g
Moles of Urea `=("Mass ")/( "Molar Mass ")=(4.5g)/(60 g " mol "^(-1))`
`=0.075` mol
Volume of Solution = 1000 ml =`(100)/(1000)L`
`=0.1 L`
Molarity of Solution =`(" Mass of solute in g")/("Volume of Solution in litres ")`
`=(0.075)/(0.12) " mol " = 0.75`M
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CHEMICAL CALCULATION

    NCERT GUJARATI|Exercise PROBLEM|4 Videos

  • CHEMICAL CALCULATION

    NCERT GUJARATI|Exercise EXAMPLE|3 Videos

  • CHEMICAL BONDING

    NCERT GUJARATI|Exercise Questions(E. Explain briefly on the following)|1 Videos

  • CHEMICAL EQUILIBRIUM - I

    NCERT GUJARATI|Exercise Questions(E. Explain briefly on the following)|2 Videos

Similar Questions

Explore conceptually related problems

The density of 3 molal solution of NaOH is 1.110 g mL^(-1) . Calculate the molarity of the solution.

4 gm NaOH dissolve in 250 ml water and solution is prepared. Find molarity of the solution.

Knowledge Check

  • If 500 mL of a 5M solution is diluted to 1500 mL, what will be the molarity of the solution obtained ?

    A
    1.5M
    B
    1.66M
    C
    0.017M
    D
    1.59M

  • A 5.25 % solution of a substance is isotonic with a 1.5% solution of urea (molar mass = 60 g. mol^(1) ) in the same solvent. If the densities of both the solutions are assumed to be equal to 1.0 g cm^(-3) , then molar mass of the substance will be

    A
    `90 g mol^(-1)`
    B
    `115 g mol^(-1)`
    C
    `105 g mol^(-1)`
    D
    `210 g mol^(-1)`

    • Similar Questions

    Explore conceptually related problems

    A 100 cm^(3) solution is prepared by dissolving 2g of NaOH in water. Calculate the normality of the solution.

    The density of 3 M solution of NaCl is 1.25 g mL^(-1) . Calculate molality of the solution.

    A 5.25% solution of a substance is isotonic with a 1.5% solution of urea (molar mass = 60g mol^(-1) ) in the same solvent. If the densities of both the solutions are assumed to be equal to 1.0 g cm^(-3) , molar mass of the substance will be:

    3.0 molal NaOH solution has a density of 1.110 g//mL . The molarity of the solution is:

    100 g of liquid A (molar mass 140 g mol^(-1) ) was dissolved in 1000 g of liuquid B (molar mass 180 g mol^(-1) ). The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 Torr.

    If 6.022xx10^(23) atoms are present in 100 mL of urea solution then find out the molarity of urea solution.

    Home
    Profile