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Determine the amount of CaCl(2) dissolv...

Determine the amount of `CaCl_(2)` dissolved in 2.5L at `27^(@)C` such that its osmotic pressure is 0.75 atm at `27^(@)C`. (i for `CaCl_(2) = 2.47`)

Text Solution

Verified by Experts

For `CaCl_(2) , " " i= 2.47`
`pi = iCRT`
`=i(n_(B))/(V) xx RT`
`0.75 = (2.47 xx n_(B) xx 0.082 xx 300)/(2.5)`
`n_(B) = (0.75 xx 2.5)/(2.47 xx 0.082 xx 300)`
`n_(B) = 0.0308` mol
Amount = `0.0308` mol `xx` 111 g `mol^(-1)`
`= 3.148` g
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Determine the amount of CaCl_(2)(i=2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27^(@)C .

Determine the amount of CaCl_2 (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27^@C .

Knowledge Check

  • Determine the amount of CaCl_(2) (i = 2.47) dissolved in 2.5 L of water sucjh that its osmotic pressure is 0.75 atm at 27^(@)C .

    A
    1.0 g
    B
    9.2 g
    C
    3.42 g
    D
    2.42 g

  • What amount of CaCl_2 (i=2.47) is dissolved in 2 litres of water so that its osmotic pressure is 0.5 atm at 27^@ C ?

    A
    3.42 g
    B
    9.24 g
    C
    2.834 g
    D
    1.820 g

  • CaCl_(2) is used as

    A
    disinfectant
    B
    desiccating agent
    C
    medicine
    D
    None of these

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    Calculate the amount of CaCl_(2) (van't Hoff factor I =2*47 ) dissolved in 2*5 L solution so that its osmotic pressure at 300 K is 0*75 atmosphere. Given : Molar mass of CaCl_(2) is 111 g."mol"^(-1) , R=0*082L." atm "K^(-1)"mol^(-1) .

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    If osmotic pressure of a solution is 2 atm at 0^(@)C , then at 546K , the osmotic pressure is

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