163835
What would be the osmotic pressure of \(0.1 \mathrm{M} \mathrm{K}_2 \mathrm{SO}_4\) solution \(\left(90 \%\right.\) dissociated) at \(27^{\circ} \mathrm{C}\) :
1 \(6.89 \mathrm{~atm}\)
2 \(0.689 \mathrm{~atm}\)
3 \(0.344 \mathrm{~atm}\)
4 \(3.4 \mathrm{~atm}\)
Explanation:
\( i=1+(n-1) \alpha \) \( i=1+(3-1) 0.9 \) \( i=1+1.8=2.8 \) \( \pi=i C R T \) \( \pi=2.8 \times 0.0821 \times 300 \times 0.1 \) \( \pi=6.89 \mathrm{~atm} \)
NCERT-XII-24
4 RBTS PAPER
163836
The osmotic pressure of \(\mathbf{0 . 2}\) molar solution of urea at \(300 \mathrm{~K}(\mathrm{R}=\mathbf{0 . 0 8 2})\) litre atm \(\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\) is :
163838
A \(0.01 \mathrm{M}\) solution of glucose in water freezes at \(-0.186^{\circ} \mathrm{C}\). A \(0.01 \mathrm{M}\) solution of \(\mathrm{KCl}\) in water will freeze at temperature :
1 higher than \(-0.0186^{\circ} \mathrm{C}\)
2 \(0^{\circ} \mathrm{C}\)
3 \(0.0186^{\circ} \mathrm{C}\)
4 lower than \(-0.0186^{\circ} \mathrm{C}\)
Explanation:
\(\Delta \mathrm{T}_{\mathrm{f}}\) is more in \(\mathrm{KCl}\) for same molar concentration because it ionises in aqueous solutions.
163835
What would be the osmotic pressure of \(0.1 \mathrm{M} \mathrm{K}_2 \mathrm{SO}_4\) solution \(\left(90 \%\right.\) dissociated) at \(27^{\circ} \mathrm{C}\) :
1 \(6.89 \mathrm{~atm}\)
2 \(0.689 \mathrm{~atm}\)
3 \(0.344 \mathrm{~atm}\)
4 \(3.4 \mathrm{~atm}\)
Explanation:
\( i=1+(n-1) \alpha \) \( i=1+(3-1) 0.9 \) \( i=1+1.8=2.8 \) \( \pi=i C R T \) \( \pi=2.8 \times 0.0821 \times 300 \times 0.1 \) \( \pi=6.89 \mathrm{~atm} \)
NCERT-XII-24
4 RBTS PAPER
163836
The osmotic pressure of \(\mathbf{0 . 2}\) molar solution of urea at \(300 \mathrm{~K}(\mathrm{R}=\mathbf{0 . 0 8 2})\) litre atm \(\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\) is :
163838
A \(0.01 \mathrm{M}\) solution of glucose in water freezes at \(-0.186^{\circ} \mathrm{C}\). A \(0.01 \mathrm{M}\) solution of \(\mathrm{KCl}\) in water will freeze at temperature :
1 higher than \(-0.0186^{\circ} \mathrm{C}\)
2 \(0^{\circ} \mathrm{C}\)
3 \(0.0186^{\circ} \mathrm{C}\)
4 lower than \(-0.0186^{\circ} \mathrm{C}\)
Explanation:
\(\Delta \mathrm{T}_{\mathrm{f}}\) is more in \(\mathrm{KCl}\) for same molar concentration because it ionises in aqueous solutions.
163835
What would be the osmotic pressure of \(0.1 \mathrm{M} \mathrm{K}_2 \mathrm{SO}_4\) solution \(\left(90 \%\right.\) dissociated) at \(27^{\circ} \mathrm{C}\) :
1 \(6.89 \mathrm{~atm}\)
2 \(0.689 \mathrm{~atm}\)
3 \(0.344 \mathrm{~atm}\)
4 \(3.4 \mathrm{~atm}\)
Explanation:
\( i=1+(n-1) \alpha \) \( i=1+(3-1) 0.9 \) \( i=1+1.8=2.8 \) \( \pi=i C R T \) \( \pi=2.8 \times 0.0821 \times 300 \times 0.1 \) \( \pi=6.89 \mathrm{~atm} \)
NCERT-XII-24
4 RBTS PAPER
163836
The osmotic pressure of \(\mathbf{0 . 2}\) molar solution of urea at \(300 \mathrm{~K}(\mathrm{R}=\mathbf{0 . 0 8 2})\) litre atm \(\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\) is :
163838
A \(0.01 \mathrm{M}\) solution of glucose in water freezes at \(-0.186^{\circ} \mathrm{C}\). A \(0.01 \mathrm{M}\) solution of \(\mathrm{KCl}\) in water will freeze at temperature :
1 higher than \(-0.0186^{\circ} \mathrm{C}\)
2 \(0^{\circ} \mathrm{C}\)
3 \(0.0186^{\circ} \mathrm{C}\)
4 lower than \(-0.0186^{\circ} \mathrm{C}\)
Explanation:
\(\Delta \mathrm{T}_{\mathrm{f}}\) is more in \(\mathrm{KCl}\) for same molar concentration because it ionises in aqueous solutions.
163835
What would be the osmotic pressure of \(0.1 \mathrm{M} \mathrm{K}_2 \mathrm{SO}_4\) solution \(\left(90 \%\right.\) dissociated) at \(27^{\circ} \mathrm{C}\) :
1 \(6.89 \mathrm{~atm}\)
2 \(0.689 \mathrm{~atm}\)
3 \(0.344 \mathrm{~atm}\)
4 \(3.4 \mathrm{~atm}\)
Explanation:
\( i=1+(n-1) \alpha \) \( i=1+(3-1) 0.9 \) \( i=1+1.8=2.8 \) \( \pi=i C R T \) \( \pi=2.8 \times 0.0821 \times 300 \times 0.1 \) \( \pi=6.89 \mathrm{~atm} \)
NCERT-XII-24
4 RBTS PAPER
163836
The osmotic pressure of \(\mathbf{0 . 2}\) molar solution of urea at \(300 \mathrm{~K}(\mathrm{R}=\mathbf{0 . 0 8 2})\) litre atm \(\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\) is :
163838
A \(0.01 \mathrm{M}\) solution of glucose in water freezes at \(-0.186^{\circ} \mathrm{C}\). A \(0.01 \mathrm{M}\) solution of \(\mathrm{KCl}\) in water will freeze at temperature :
1 higher than \(-0.0186^{\circ} \mathrm{C}\)
2 \(0^{\circ} \mathrm{C}\)
3 \(0.0186^{\circ} \mathrm{C}\)
4 lower than \(-0.0186^{\circ} \mathrm{C}\)
Explanation:
\(\Delta \mathrm{T}_{\mathrm{f}}\) is more in \(\mathrm{KCl}\) for same molar concentration because it ionises in aqueous solutions.
