Which of the following is a substitutional solid solution ?
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Chemistry MCQs for NEET — Practice Questions with Answers
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$ Solute + solvent \rightleftharpoons solution; \triangle H \gt O $ . what would be the change in solubility of substance on increasing the temperature at equilibrium ?
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Explanation
The given equation represents an endothermic process (ΔH > 0). According to Le Chatelier's principle, an increase in temperature favors the endothermic reaction, thereby increasing the solubility of the substance.
Which of the following is a colligative property ?
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What will be the ratio of any colligative properties of 1.0 m aqueons solutions of $ Nacl, Na_2So_4 ad K_4 [Fe(CN)_6] $ (Assume that solute completely (100%) dissociates in the solution)
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At constant temperature, vapour pressure of aqueous solutions of $ Na_2So_4, urea and AlCl_3 are equal with the vapour pressure of aqueous solution of 1.2 m kcl solution; then molality of an aqueons of Na_2So_4, urea and AlCl_3 $ are respectively –
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Explanation
$ n_1.m_1 = n_2 .m_2 $ Where n_1 = number of ions produce when 1 st substance is dissolved in $ H_2 O $ $ m_1$ = mulality of 1st substance $ n_2 = number of ions produced when 2 nd substance is dissolved in H_2O $ according to its formula The values of $n_1 for Na_2 SO_4 , ureq and AlCl_3 $ are 3 ,1 and 4 respectively We get 0.8 m, 2.4 m, 0.6 m for $ Na_2 SO_4 , ureq and AlCl_3 $
In Binary ideal solution forms by liquid A and B, at constant temperature, mole-fraction of liquid A in vapour state is 0.4 and its partial vapour pressure is 400 mm, then what will be the partial vapour pressure of B ?
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Explanation
$ Y_A = 0.4 and P_A = 400 mm $ $ P_B = 1000 - 400 = 600 mm $ $ P_A = P_{Total} \times Y_A $ $ \therefore 400 = P \times 0.4 $ $ \therefore P_{Total} = 1000 mm $
1.0 molal aqueous solution of a substance boils at $ 100.55 ^\circ C ; then, at what approximate temperature, it freezes ? (Kb = 0.51 ^\circ C – kg - mole^{-1} and Kb = 1.86 ^\circ C – kg - mole^{-1}) $
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Explanation
$ { \triangle Tf \over \triangle Tb } = { kf \over Kb } $ $ \therefore \triangle T_f = { Kf \over Kb } \times \triangle T_b $ $ = { 1.86 \over 0.51 } \times 0.55 = 2 K $ $ \therefore T_f = 273 - 2 = 271 K $
Ionic substances are completely dissociates, then aqueous solution of which of the following substances having least freezing point ?
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Explanation
The freezing point depression of a solution is directly proportional to the number of particles present in the solution. Al2(SO4)3 dissociates into five ions (2Al^3+ and 3SO4^2-), which is the highest number of particles compared to the other options, leading to the greatest freezing point depression.
0.2 M aqueous solution of $ NH_4Cl$ is isotonic with which of the following aqueous solution ?
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At constant temperature, osmotic pressure of an aqueous solution of 1.5 M $ NH_4NO_3 and xN Al_2(SO_4)_3 $ are equal, then mention the value of X. (Assume that ionic solid substances completely dissociates in the solution)
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Explanation
$ n_1 M_1 = n_2 M_2$ $ For NH_4 NO_3 values for n_1 and M_1 are 2 and 1.5 resp$ $ For Al_2 (SO)_4 n_2 = 5 $ $ \therefore M_2 = {2 \over 5 } \times 1.5 = 0.6 $ $ normality of Al_2(SO_4) _3 = 6 \times molarity $ $ = 6 \times 0.6 $ $ = 3.6 N $
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