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Class 12 · Chemistry
→When 4 g of a solute is dissolved in 500 g of water, the freezing-point depression is 0.186 K. If the solute is an AB-type solute that dissociates by 50%, what is its true molar mass? Take Kf for water as 1.86 K kg mol⁻¹.
Class 12 · Chemistry
→A substance forms trimers. If its van’t Hoff factor is i = 0.6, what is the degree of association?
Class 12 · Chemistry
→A solute forms dimers. Its true molar mass is 60 g mol⁻¹, while its observed molar mass is 80 g mol⁻¹. What is the degree of association?
Class 12 · Chemistry
→The true molar mass of CaCl₂ is 111 g mol⁻¹. If its observed molar mass is 55.5 g mol⁻¹, what is the degree of dissociation?
Class 12 · Chemistry
→If the observed molar mass of an AB-type solute is 5/8 of its true molar mass, what is the degree of dissociation?
Class 12 · Chemistry
→If the true molar mass of NaCl is 58.5 g mol⁻¹ and the colligative-property method gives an observed molar mass of 39 g mol⁻¹, what is the approximate van’t Hoff factor, i?
Class 12 · Chemistry
→A solute has a true molar mass of \(120\,\mathrm{g\,mol^{-1}}\), but its observed molar mass is \(240\,\mathrm{g\,mol^{-1}}\). What is the most suitable conclusion?
Class 12 · Chemistry
→The true molar mass of a solute is \(180\,\mathrm{g\,mol^{-1}}\), but a colligative-property measurement gives an apparent molar mass of \(90\,\mathrm{g\,mol^{-1}}\). What is the value of the van’t Hoff factor \(i\)?
Class 12 · Chemistry
→A \(1\,\mathrm{L}\) solution is prepared from \(6\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(1.23\,\mathrm{atm}\). The solute is non-dissociating. What is its molar mass?
Class 12 · Chemistry
→When \(2\,\mathrm{g}\) of a non-dissociating solute is dissolved in \(100\,\mathrm{g}\) of solvent, the boiling-point elevation is \(0.208\,\mathrm{K}\). If \(K_b=0.52\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?
Class 12 · Chemistry
→When \(3.2\,\mathrm{g}\) of a solute is dissolved in \(400\,\mathrm{g}\) of water, the depression in freezing point is \(0.186\,\mathrm{K}\). Taking \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?
Class 12 · Chemistry
→A solution of volume \(500\,\mathrm{mL}\) is prepared using \(1.5\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(0.615\,\mathrm{atm}\). If \(R=0.082\,\mathrm{L\,atm\,mol^{-1}\,K^{-1}}\), what is the molar mass of the solute?
Class 12 · Chemistry
→When \(5\,\mathrm{g}\) of a non-dissociating solute is dissolved in \(250\,\mathrm{g}\) of solvent, the boiling point rises by \(0.104\,\mathrm{K}\). If \(K_b=0.52\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?
Class 12 · Chemistry
→When \(2.4\,\mathrm{g}\) of a non-dissociating solute is dissolved in \(200\,\mathrm{g}\) of water, the freezing point decreases by \(0.372\,\mathrm{K}\). If \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?
Class 12 · Chemistry
→A \(0.001\,\mathrm{M}\) solution is prepared to determine the molar mass of a protein. Which measurement is most useful for such a very dilute solution?
Class 12 · Chemistry
→A sample has a normal molar mass of \(98\,\mathrm{g\,mol^{-1}}\), but its experimentally determined molar mass is \(49\,\mathrm{g\,mol^{-1}}\). Which statement best explains this result?
Class 12 · Chemistry
→If \(0.10\,\mathrm{mol}\) of solute has a mass of \(9.0\,\mathrm{g}\), and the same amount of solute is obtained from a colligative-property measurement, what is its molar mass?
Class 12 · Chemistry
→A solution has relative lowering of vapour pressure \(0.02\). If the total number of moles in the solution is \(5.0\), how many moles of solute are present?
Class 12 · Chemistry
→Why is the vapour-pressure method considered comparatively difficult for molar mass determination?
Class 12 · Chemistry
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