Last Updated On [03-11-2023]
The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is
(a)
16 × 10−4
(b)
4 × 10−4
(c)
6 × 10−2
(d)
4 × 10−2
The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is
(a)
16 × 10−4
(b)
4 × 10−4
(c)
6 × 10−2
(d)
4 × 10−2
Question ID - 52580 :-
The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is
(a)
16 × 10−4
(b)
4 × 10−4
(c)
6 × 10−2
(d)
4 × 10−2
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The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl2 in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L-1) in solution is |
|||
|
(a) |
16 × 10−4 |
(b) |
4 × 10−4 |
|
(c) |
6 × 10−2 |
(d) |
4 × 10−2 |
2[XY] = 4 ×(0.01)× 3
10−2 
Next Question :
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Consider the van der Waals constants, a and b, for the following gases. Gas Ar Ne Kr Xe a/(atm dm6 mol−2) 1.3 0.2 5.1 4.1 b/(10−2 dm3 mol−1) 3.2 1.7 1.0 5.0 Which gas is expected to have the highest critical temperature? |
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|
(a) |
Ne |
(b) |
Kr |
|
(c) |
Xe |
(d) |
Ar |
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