Which one of the following solutions of compounds show highest osmotic pressure? $\left(A B, A B_2\right.$…
Which one of the following solutions of compounds show highest osmotic pressure? $\left(A B, A B_2\right.$ and $A_2 B_3$ are ionic compounds)
- $5.0 \mathrm{M}$ urea $i=1.0$ and temperature is $67^{\circ} \mathrm{C}$
- $1.5 \mathrm{M} A_2 B_3$ type $i=4.1$ and temperature is $27^{\circ} \mathrm{C}$
- $3.0 \mathrm{M} A B$ type $i=1.6$ and temperature is $27^{\circ} \mathrm{C}$
- $2.5 \mathrm{M} \mathrm{AB} B_2$ type $i=2.5$ and temperature is $57^{\circ} \mathrm{C}$
Solution
$\because \quad \pi=i C R T$.
(a) $\pi$ for $5.0 \mathrm{M}$ urea is
$\pi=1 \times 5 \times 0.0821 \times 340 \mathrm{~K}$
$\pi=139.57 \mathrm{~atm}$
(b) $\pi$ for $1.5 \mathrm{M} A_2 B_3$ type is $(i=4)$
$\pi=4.1 \times 1.5 \times 0.0821 \times 300 \mathrm{~K}$
$\pi=151.47 \mathrm{~atm}$
(c) $\pi$ for $3.0 \mathrm{M} A B$ type is $(i=1.6)$
$\pi=1.6 \times 3 \times 0.0821 \times 300 \mathrm{~K}$
$\pi=118.22 \mathrm{~atm}$
(d) $\pi$ for $2.5 \mathrm{M} A B_2$ type is $(i=2.5)$
$\pi=2.5 \times 2.5 \times 0.0821 \times 330 \mathrm{~K}$
$\pi=169.33 \mathrm{~atm}$
Hence $A B_2$ highest osmotic pressure at $57^{\circ} \mathrm{C}$ shows.
Asked in: AP EAMCET 2017 (26 Apr Shift 1)
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