1. For very dilute solutions, the osmotic pressure follows the equation,
`pi = ("n"_2 "RT")/"V"` ....(1)
2. If the mass of solute in V litres of a solution is W2 and its molar mass is
`"M"_2`, then `"n"_2 = "W"_2/"M"_2`
Substituting the value of n2 in equation (1), we get
`pi = ("W"_2 "RT")/("M"_2 "V")`
∴ `"M"_2 = ("W"_2 "RT")/(pi "V")`
This formula can be used for the calculation of molar mass of a nonionic solute (i.e., nonelectrolyte), by osmotic pressure measurement.
derive an expression to calculate molar mass of non volatile solute by osmotic pressure measurement
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derive an expression to calculate molar mass of non volatile solute by osmotic pressure measurement
answer :∴π=mW×V1×S. T⟶ From this equation molar mass can be determined.
Solution : According to Van.t Hoff equation<br>`pi= CRT`<br> `c=n/V` <br> Here, n= number of moles of solute dissolved in .V. litre of the solution.<br> Therefore, `pi =n/Vxx RT` or<br>`piV = nRT`<br> In the solution is prepared by dissolving `w_B` g of non-volatile solute in `w_A` gof solvent, then the number of moles .n. is,<br>n=`w_B/M_B`<br> since M = molar mass of the solute<br> Substituting them in (I), we get<br>`pi= (w_B)/(V) (RT)/(pi)" "...(2)`<br> From the equation (2). molar mass of the solute can be calculated
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- How molar mass of a solute is determined from osmotic pressure measurements?
- How molar mass of a solute is determined from osmotic pressure measurements?
- How molar mass of a solute is determined from osmotic pressure mea
- How molar mass of a solute is determined from osmotic pressure measurements?
- Determination Of Molecular Mass Of Non
- Determination of molecular mass of non-volatile solute from osmotic pressure
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Answer derive an expression to calculate molar mass of non volatile solute by osmotic pressure measurement
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answer :∴π=mW×V1×S. T⟶ From this equation molar mass can be determined.
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How molar mass of a solute is determined from osmotic pressure measurements?
Osmotic pressure symbol= πMedium Open in App Solution Verified by Toppr π∝C [Molarity] π∝T
∴π=STC where S= solution constant
∵ Molarity=
(V) Volume in litres
Moles and moles= Molar mass(m) weight(W) ∴π= m W × V 1
×S.T⟶ From this equation molar mass can be determined.
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How molar mass of a solute is determined from osmotic pressure mea
Solution For How molar mass of a solute is determined from osmotic pressure measurements?
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How molar mass of a solute is determined from osmotic pressure measurements?
Solution
Osmotic pressure symbol= ππ∝C [Molarity] π∝T
∴π=STC where S= solution constant
∵ Molarity=
(V) Volume in litres
Moles and moles= Molar mass(m) weight(W) ∴π= m W × V 1
×S.T⟶ From this equation molar mass can be determined.
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Each question contains STATEMENT-I(Assertion) and STATEMENT-2(Reason).the statement carefully and mark the correct answer accoring to the instrution given below:
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Determination Of Molecular Mass Of Non
The osmotic pressure is a colligative property.For a given solvent the osmotic pressure depends only upon the molar concentration of solute but does not depend upon its nature…
DETERMINATION OF MOLECULAR MASS OF NON-VOLATILE SOLUTE FROM OSMOTIC PRESSURE (P)
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Colligative Properties
Determination of Molecular Mass of non-volatile Solute from Osmotic Pressure (p)
Determination of molecular mass of non-volatile solute from osmotic pressure
The osmotic pressure is a colligative property.For a given solvent the osmotic pressure depends only upon the molar concentration of solute but does not depend upon its nature. The following relation relates osmotic pressure to the number of moles of the solute,
According to Boyle Van't Hoff law (at conc. temp.)
..... (i)
According to Gaylussac Van't Hoff law (at conc. temp.)
..... (ii)
From equation (i) and (ii)
, (Van't Hoff equation)
;
Here, C = concentration of solution in moles per litre
R = gas constant; T = temperature
n = number of moles of solute; V = volume of solution
m = molecular weight of solute; w = weight of solute
(iii) Conditions for getting accurate value of molecular mass are,
(a) The solute must be non-volatile.
(b) The solution must be dilute.
(c) The solute should not undergo dissociation or association in the solution.
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Solution : According to Van.t Hoff equation<br>`pi= CRT`<br> `c=n/V` <br> Here, n= number of moles of solute dissolved in .V. litre of the solution.<br> Therefore, `pi =n/Vxx RT` or<br>`piV = nRT`<br> In the solution is prepared by dissolving `w_B` g of non-volatile solute in `w_A` gof solvent, then the number of moles .n. is,<br>n=`w_B/M_B`<br> since M = molar mass of the solute<br> Substituting them in (I), we get<br>`pi= (w_B)/(V) (RT)/(pi)" "...(2)`<br> From the equation (2). molar mass of the solute can be calculated
1. For very dilute solutions, the osmotic pressure follows the equation,
`pi = ("n"_2 "RT")/"V"` ....(1)
2. If the mass of solute in V litres of a solution is W2 and its molar mass is
`"M"_2`, then `"n"_2 = "W"_2/"M"_2`
Substituting the value of n2 in equation (1), we get
`pi = ("W"_2 "RT")/("M"_2 "V")`
∴ `"M"_2 = ("W"_2 "RT")/(pi "V")`
This formula can be used for the calculation of molar mass of a nonionic solute (i.e., nonelectrolyte), by osmotic pressure measurement.