201. Which of the following can be measured by the Ostwald-Walker dynamic method? [KCET 2008]

1) Relative lowering of 2) Lowering of vapour vapour pressure pressure 3) Vapour pressure of 4)All of the above the solvent

202. The freezing point \(\left(\mathrm{in}^{\circ} \mathrm{C}\right)\) of solution containing \(0.1 \mathrm{~g}\) of \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right](\mathrm{mol}\).wt 329) in \(100 \mathrm{~g}\) of water \(\left(K_{f}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)\) is

1) \(-2.3 \times 10^{-2}\)

2) \(-5.7 \times 10^{-2}\)

3) \(-5.7 \times 10^{-3}\)

4) \(-1.2 \times 10^{-2}\)

203. The degree of dissociation ( \(\alpha\) ) of a weak electrolyte \(A_{x} B_{y}\) is related to van't Hoff factor (i) by the expression [AIEEE 2003]

1) \(\alpha=\frac{i-1}{(x+y-1)}\)

\(\alpha=\frac{i-1}{x+y+1}\)

3) \(\alpha=\frac{x+y-1}{i-1}\)\[

\alpha=\frac{x+y+1}{i-1}

\]

204. If \(\alpha\) is the degree of dissociation of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) the van't Hoff factor (i) used for calculating the molecular mass is [AIEEE 2005]

1) \(1-2 \alpha\)

2) \(1+2 \alpha\)

3) \(1-\alpha\)

4) \(1+\alpha\)

205. Van't hoff factor of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) is [BCECE 2008]

1) One

2) Two

3) Three

4) four

206. Van't Hoff factor more than unity indicates that the solute in solution has [Manipal 2008]

1) Dissociated

2)Associated

3)Both (a) and (b)

4) Cannot say anything

207. Abnormal colligative properties are observed only when the dissolved non-volatile solute in a given dilute solution [J\&K CET 2008]

1) Is a non-electrolyte 2) Offers an intense colour

3)Associates of

4) Offers no colour dissociates

208.0.004 \(\mathrm{MNa}_{2} \mathrm{SO}_{4}\) is isotonic with \(0.01 \mathrm{M}\) glucose.Degree of dissociation of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is

[IIT JEE 2004]

1) \(75 \%\)

2) \(50 \%\)

3) \(25 \%\)

4) \(85 \%\)

209. Phenol dimerises in benzene having van't Hoff factor 0.54 . What is the degree of association?

[OJEE 2007]

1) 1.92

2) 0.98

3) 1.08

4) 0.92 210. Van't hoff factor of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) is [Jamia Millia Islamia 2008]

1) Benzoic acid is an

2) Benzoic acid has organic solute

3) Benzoic acid gets associated in benzene higher molar mass than benzene

4) Benzoic acid gets dissociated in benzene

211. Van't Hoff factor of aq \(\mathrm{K}_{2} \mathrm{SO}_{4}\) at infinite dillution has value equal to [AMU 2009]

1) 1

2) 2

3) 3

4) Between 2 and 3

212. If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water \(\left(\Delta T_{f}\right)\), when 0.01 mole of sodium sulphate is dissolved in \(1 \mathrm{~kg}\) of water, is ( [AIEEE 2010]

1) \(0.0372 \mathrm{~K}\)

2) \(0.0558 \mathrm{~K}\)

3) \(0.0744 \mathrm{~L}\)

4) \(0.0186 \mathrm{~K}\)

213.0.004 \(\mathrm{MNa}_{2} \mathrm{SO}_{4}\) is isotonic with \(0.01 \mathrm{M}\) glucose.Degree of dissociation of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is

[Manipal 2003]

1) 61

2) 244

3) 366

4) 122

214. The elevation in boiling point of a solution of \(13.44 \mathrm{~g}\) of \(\mathrm{CuCl}_{2}\) in \(1 \mathrm{~kg}\) of water using the following information will be (molecular weight of \(\mathrm{CuCl}_{2}=134.4\) and [IIT JEE 2005]

1) 0.16

2) 0.05

3) 0.1

4) 0.2

215. Observe the following abbrevations

\(\pi_{o b s}=\) observed colligative property

\(\pi_{c a l}=\) theoretical colligative property

assuming normal behaviour of

solute.

Van't Hoff factors (i) is given by [J\&K CET

2006]

1) \(i=\pi_{o b s} \times \pi_{c a l}\)

2) \(i=\pi_{o b s}+\pi_{c a l}\)

3) \(i=\pi_{o b s}-\pi_{c a l}\)

4) \(i=\frac{\pi_{o b s}}{\pi_{c a l}}\)

216. When \(20 \mathrm{~g}\) of naphthoic acid \(\left(\mathrm{C}_{11} \mathrm{H}_{8} \mathrm{O}_{2}\right)\) is dissolved in \(50 \mathrm{~g}\) of benzene (

\(k_{f}=1.72 \mathrm{Kkg} \mathrm{mol}^{-1}\) ), a freezing point depression of \(2 \mathrm{~K}\) is observed. The van't Hoff factor (i) is [IIT JEE 2007]

1) 0.5

2) 1

3) 2

4) 3

217. The van't Hoff factor of \(\mathrm{BaCl}_{2}\) at \(0.01 \mathrm{M}\) concentration is 1.98. The percentage of dissociation of \(\mathrm{BaCl}_{2}\) at this concentration is

[Kerala CEE 2005]

1) 49

2) 69

3) 89

4) 98

5) 100

218. The van't hoff factor for \(0.1 \mathrm{mBa}\left(\mathrm{NO}_{3}\right)_{2}\) solution is 2.74 . The degree of dissociation is [J\&K CET 2003]

1) \(91.3 \%\)

2) \(87 \%\)

3) \(100 \%\)

4) \(74 \%\)

219. If the various terms in the below given expressions have usual meanings, the van't Hoff factor (i) cannot be calculated by which one of the expressions? [DCE 2009]

1)

\(\pi V=\sqrt{i n R T}\)

2)

\(\Delta T_{f}=i k_{f} \cdot m\)

3)

\(\Delta T_{b}=i k_{b} \cdot m\)

4) \(\frac{p_{\text {solvent }}^{\circ}-p_{\text {solution }}}{p_{\text {solvent }}^{\circ}}=i\left(\frac{n}{N+i}\right.\)

220. One gram of silver gets distributed between \(10 \mathrm{~cm}^{3}\) of molten zinc and \(100 \mathrm{~cm}^{3}\) of molten lead at \(8000^{\circ} \mathrm{C}\). The percentage of silver still left in the lead layer in approximately [WB JEE

\section{6]}

1) Henry

2) Van't Hoff

3) Nernst's

4) Ostwald

221. One gram of silver gets distributed between \(10 \mathrm{~cm}^{3}\) of molten zinc and \(100 \mathrm{~cm}^{3}\) of molten lead at \(8000^{\circ} \mathrm{C}\). The percentage of silver still left in the lead layer in approximately [KCET 2011]

1) 2

2) 5

3) 3

4) 1

222. Molecular weight of glucose is 180 . A solution of glucose which contains \(18 \mathrm{~g} / \mathrm{L}\), is

1) 0.1 molal

2) 0.2 molal

3) 0.3 molal

4) 0.4 molal

223. A molar solution of \(\mathrm{NaCl}\) has a density of

1. \(21 \mathrm{~g} \mathrm{~mL}^{-1}\). The molarity of this solution is

1) 2.35

2) 1.143

3) 2.95

4) 1.356 224.19.85 mL of \(0.1 \mathrm{~N} \mathrm{NaOH}\) reacts with \(20 \mathrm{~mL}\) of \(\mathrm{HCl}\) solution for complete neutralization. The molarity of \(\mathrm{HCl}\) solution is

1) 9.9

2) 0.99

3) 0.099

4) 0.0099

225. When \(W_{B}\) g solute (molecular mass \(M_{B}\) ) dissolves in \(W_{A}\) g solvent, the molality \(M\) of the solution is

1) \(\frac{W_{B}}{M_{B}} \times \frac{1000}{W_{A}}\)

2) \(\frac{W_{A}}{M_{B}} \times \frac{1000}{W_{B}}\)

3) \(\frac{W_{B}}{W_{A}} \times \frac{M_{A}}{1000}\)

4) \(\frac{W_{A}}{W_{B}} \times \frac{M_{B}}{1000}\)

226. In a solution of \(7.8 \mathrm{~g}\) benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) and \(46.0 \mathrm{~g}\) toluene \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}\right)\), the mole-fraction of benzene is

1) \(\frac{1}{2}\)

2) \(\frac{1}{3}\)

3) \(\frac{1}{5}\)

4) \(\frac{1}{6}\)

227. Molarity of \(0.2 \mathrm{~N}_{2} \mathrm{SO}_{4}\) is

1) 0.1

2) 0.2

3) 0.3

4) 0.4

228. Normality of \(2 \mathrm{M}\) sulphuric acid is

1) \(2 \mathrm{~N}\)

2) \(4 \mathrm{~N}\)

3) \(\frac{N}{2}\)

4) \(\frac{N}{4}\)

229. Conc \(\mathrm{H}_{2} \mathrm{SO}_{4}\) has a density of \(1.98 \mathrm{~g} / \mathrm{mL}\) and is \(98 \% \mathrm{H}_{2} \mathrm{SO}_{4}\) by weight. Its normality is

1) \(19.6 \mathrm{~N}\)

2) \(29.6 \mathrm{~N}\)

3) \(39.6 \mathrm{~N}\)

4) \(49.6 \mathrm{~N}\)

230.3.0 molal \(\mathrm{NaOH}\) solution has a density of 1.110

\(\mathrm{g} / \mathrm{mL}\). The molarity of the solution is

1) 3.9732

2) 2.9732

3) 1.9732

4) 0.9732

231. The molarity of a solution made by mixing 50 \(\mathrm{mL}\) of \(\mathrm{ConcH}_{2} \mathrm{SO}_{4}(36 \mathrm{~N})\) with \(50 \mathrm{~mL}\) of water is

1) \(9 \mathrm{~m}\)

2) \(10 \mathrm{~m}\)

3) \(11 \mathrm{~m}\)

4) \(12 \mathrm{~m}\)

232. Which is correct about Henry's law?

1) There should not be 2) The gas in contact any chemical with the liquid interaction between should behave as an the gas and liquid ideal gas

3) The pressure applied4) All of the above should be high 233. Molarity of a solution prepared by dissolving \(75.5 \mathrm{~g}\) of pure \(\mathrm{KOH}\) in \(540 \mathrm{~mL}\) solution is

1) \(1.50 \mathrm{M}\)

2) \(2.50 \mathrm{M}\)

3) \(3.50 \mathrm{M}\)

4) \(5.01 \mathrm{M}\)

234. What is the molarity of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution that has a density \(1.84 \mathrm{~g} / \mathrm{cc}\) at \(35^{\circ} \mathrm{C}\) and contains \(98 \%\) solute by weight?

1) \(4.18 \mathrm{M}\)

2) \(1.84 \mathrm{M}\)

3) \(8.41 \mathrm{M}\)

4) \(18.4 \mathrm{M}\)

235.20 g of hydrogen is present in a \(5 \mathrm{~L}\) vessel. The molar concentration of hydrogen is

1) 1

2) 2

3) 3

4) 4

236. Dilute \(1 \mathrm{~L}\) one molar \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution by \(5 \mathrm{~L}\) water, the normality of that solution is

1) \(0.33 \mathrm{~N}\)

2) \(33.0 \mathrm{~N}\)

3) \(0.11 \mathrm{~N}\)

4) \(11.0 \mathrm{~N}\)

237. The normality of \(10 \%\) (weight/volume) acetic acid is

1) \(1 \mathrm{~N}\)

2) \(1.3 \mathrm{~N}\)

3) \(1.7 \mathrm{~N}\)

4) \(1.9 \mathrm{~N}\)

238.9.8 \(\mathrm{g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is present in \(2 \mathrm{~L}\) of a solution.

The molarity of the solution is

1) \(0.05 \mathrm{M}\)

2) \(0.01 \mathrm{M}\)

3) \(0.03 \mathrm{M}\)

4) \(0.02 \mathrm{M}\)

239. Mole fraction \((X)\) of any solution is equal to

1) \(\frac{\text { no. of moles of solute }}{\text { volume of solution in litre }}\) 2) no. of gram-equivalent of

3) \(\frac{\text { no. of moles of solute }}{\text { mass of solvent in } \mathrm{kg}}\)

4) \(\frac{\text { no. of moles of any con }}{\text { total number of moles of ali }}\)

240. The amount of anhydrous \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) present in \(250 \mathrm{~mL}\) of \(0.25 \mathrm{M}\) solution is

1) \(6.0 \mathrm{~g}\)

2) \(6.625 \mathrm{~g}\)

3) \(66.25 \mathrm{~g}\)

4) \(6.225 \mathrm{~g}\)

241. The amount of anhydrous \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) present in \(250 \mathrm{~mL}\) of \(0.25 \mathrm{M}\) solution is

1) \(6.625 \mathrm{~g}\)

2) \(66.25 \mathrm{~g}\)

3) \(662.5 \mathrm{~g}\)

4) \(6625 \mathrm{~g}\)

242. The solubility of a gas increases in a liquid with

1) Decrease in

2) Increases in temperature temperature

3) Reduction of gas

4)Amount of liquid pressure taken

243. The weight of \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}\) required to pressure \(500 \mathrm{~mL}\) of \(0.2 \mathrm{~N}\) solution is

1) \(63 \mathrm{~g}\)

2) \(6.3 \mathrm{~g}\)

3) \(0.63 \mathrm{~g}\)

4) \(126 \mathrm{~g}\) 244. The number of moles of a solute in its solution is 20 and total number of moles are 80 . The mole fraction of solute is

1) 0.25

2) 0.50

3) 1.00

4) 1.25

245. If \(20 \mathrm{~mL}\) of \(0.4 \mathrm{~N} \mathrm{NaOH}\) solution completely neutralizes \(40 \mathrm{~mL}\) of a dibasic acid, the molarity of the acid solution is

1) \(0.1 \mathrm{M}\)

2) \(0.3 \mathrm{M}\)

3) \(0.5 \mathrm{M}\)

4) \(0.7 \mathrm{M}\)

246. The statement, "The mass of a gas dissolved in a given mass of a solvent at any temperature is proportional to the pressure of the gas above the solvent" is

1) Henry's law

2) Law of mass action

3) Dalton's law

4) None of these

247.3.65 \(\mathrm{g}\) of \(\mathrm{HCl}\) is dissolved in \(16.2 \mathrm{~g}\) of water.

The mole fraction of \(\mathrm{HCl}\) in the resulting solution is

1) 0.1

2) 0.2

3) 0.3

4) 0.4

248. If \(5.85 \mathrm{~g} \mathrm{NaCl}\) (molecular weight 58.5) is dissolved in water and the solution is made up to \(0.5 \mathrm{~L}\), the molarity of the solution will be

1) 0.1

2) 0.2

3) 0.3

4) 0.4

249. The normality of a \(100 \mathrm{~mL}\) solution of sodium hydroxide which contains \(4 \mathrm{~g}\) of \(\mathrm{NaOH}\), is

1) 0.5

2) 1.0

3) 1.5

4) 2.0

\(250.100 \mathrm{~mL}\) of \(0.3 \mathrm{HCl}\) is mixed with \(200 \mathrm{~mL}\) of \(0.6 \mathrm{NH}_{2} \mathrm{SO}_{4}\). The final normality of the resulting solution will be

1) \(0.3 \mathrm{~N}\)

2) \(0.2 \mathrm{~N}\)

3) \(0.5 \mathrm{~N}\)

4) \(0.1 \mathrm{~N}\)

251. The normality of \(0.3 \mathrm{M}\) phosphorous acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{3}\right)\) is

1) 0.2

2) 0.4

3) 0.6

4) 0.8

252. Which of the following solutions has the highest normality?

1) 6 g of \(\mathrm{NaOH} / 100 \mathrm{~mL} 2)^{0.5 \mathrm{MH}_{2} \mathrm{SO}_{4}}\)

3) N phosphoric acid 4) \(8 \mathrm{~g}\) of \(\mathrm{KOH} / \mathrm{L}\)

253. Calculate the molarity of \(1 \mathrm{~L}\) solution of \(93 \%\) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (weight/volume). The density of the solution is \(1.84 \mathrm{~g} / \mathrm{mL}\)

1) 11.05

2) 12.05

3) 13.05

4) 14.05

254. The normality of \(2.3 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution is

1) \(4.6 \mathrm{~N}\)

2) \(5.6 \mathrm{~N}\)

3) \(6.6 \mathrm{~N}\)

4) \(7.6 \mathrm{~N}\)

255. When a non-volatile solute is dissolved in a solvent, the relative lowering of vapour pressure is equal to

1) Mole fraction of

2) Mole fraction of solute solvent

3) Concentration of the 4) Concentration of the solute in gram per solute in gram per litre \(100 \mathrm{~mL}\)

256. An azeotropic solution of two liquids has boiling point lower than either when it

1) Shows a negative

2) Shows a positive deviation from deviation from Raoult's law Raoult's law

3) Shows no deviation 4) Is saturated from Raoult's law

257. Which of the following is not correct for ideal solution?

1) \(\Delta V_{\text {mix }}=0\)

2) \(\Delta H_{\text {mix }}=0\)

3) \(\Delta S_{\text {mix }}=0\)

4) Obeys Raoult's law

258. An aqueous solution of methanol in water has vapour pressure

1) Less than that of

2) More than that of water water

3) Equal to that of

4) Equal to that of water methanol

259. The vapour pressure of water at \(20^{\circ} \mathrm{C}\) is 17.54 \(\mathrm{mm}\). When \(20 \mathrm{~g}\) of a non-ionic, substance is dissolved in \(100 \mathrm{~g}\) of water, the vapour pressure is lowered by \(0.30 \mathrm{~mm}\). What is the molecular mass of the substance?

1) 200.8

2) 206.88

3) 210.5

4) 215.2

260. When attraction between \(A-B\) is more than that of \(A-A\) and \(B-B\), the solution will show.....deviation from Raoult's law

1) Positive

2) Negative

3) No

4) Cannot predicted

261. Which of the following is the expression of Raoult's law?

( \(p\) =vapour pressure of pure solvent, \(p_{s}=\) vapour pressure of the solution)

1) \(\frac{p-p_{s}}{p}=\frac{n}{n+N}\)

2) \(\frac{p_{s}-p}{p}=\frac{N}{N+n}\) 

3) \(\frac{p-p_{s}}{p_{s}}=\frac{N}{N-n}\)

4) \(\frac{p_{s}-p}{p_{s}}=\frac{N-n}{N}\)

262. Vapour pressure ofCCl\({ }_{4}\) at \(25^{\circ} \mathrm{C}\) is \(143 \mathrm{~mm}\) of \(\mathrm{Hg}\) and \(0.5 \mathrm{~g}\) of a non-volatile solute (mol. \(w t=65)\) is dissolved in \(100 \mathrm{~mL} \mathrm{CCl}_{4}\). Find the vapour pressure of the solution. (Density of \(\left.\mathrm{CCl}_{4}=1.58 \mathrm{~g} / \mathrm{cm}^{2}\right)\)

1) \(94.39 \mathrm{~mm}\)

2) \(141.93 \mathrm{~mm}\)

3) \(134.44 \mathrm{~mm}\)

4) \(199.34 \mathrm{~mm}\)

263. Azeotropic mixture are

1) Constant

2) Those which boils at temperature boiling different mixture temperatures

3) Mixture of two solids4) None of the above

264. The vapour pressure of a liquid in a closed container depends upon

1)Amount of liquid

2) Surface area of the container

3) Temperature

4) None of the above

265. An ideal solution is that which

1) Obey Raoult's law

2) Shows positive deviation from Raoult's law

3) Shows negaitive

4) Has no connection deviation from with Raoult's law

Raoult's law

266. For determination of molecular weights, Raoult's law is applicable only to

1) Dilute solutions of

2) Concentration electrolytes solution of electrolytes

3) Dilute solutions of

4) Concentration non electrolytes solution of non electrolytes

267. For a dilute solution, Raoult's law states that

1) The lowering of

2) The relative lowering vapour pressure is of vapour pressure is equal to mole equal to mole fraction of solute fraction of solute

3) The relative lowering of vapour 4) The vapour pressure of the solution is pressure is equal to the mole proportional to the fraction of solvent amount of solute in solution

268. When two liquids \(A\) and \(B\) are mixed then their boiling points becomes greater than both of them. What is the nature of this solution?

1) Ideal solution

2) Normal solution

3) Negative deviation

4) Positive deviation with non-ideal with non-ideal solution solution

269. The atmospheric pressure is sum of the

1) Pressure of the

2) Vapour pressure of biomolecules atmospheric constituents

3) Vapour pressure of

4) Pressure created on chemicals and to atmospheric vapour pressure of molecules volatiles

270. Which of the following is true when components forming an ideal solution are mixed?

1) \(\Delta H_{m}=\Delta V_{m}=0\)

2) \(\Delta H_{m}<\Delta V_{m}\)

3) \(\Delta H_{m}=\Delta V_{m}=1\)

4) \(\Delta H_{m}>\Delta V\)

271. Which of the following liquid pair shows a positive deviation from Raoult's law?

1) Water-nitric acid

2)Acetone-chloroform

3) Water-hydrochloric

4) Benzene-methanol acid

272. What happens when an egg is kept in saturated solution of \(\mathrm{NaCl}\) after removing its hard shell in dilHCl?

1) Egg will swell

2) Egg will shrink

3) Egg will remain

4) Egg will first shrink same and then swell

273. A solution of sucrose (molar mass \(=342 \mathrm{~g} / \mathrm{mol}\) ) is prepared by dissolving \(68.4 \mathrm{~g}\) of it per litre of the solution, what is its osmotic pressure ( \(R=0.082 \mathrm{Latm}^{-1} \mathrm{~mol}^{-1}\) ) at \(273 \mathrm{~K}\) ?

1) \(3.92 \mathrm{~atm}\)

2) \(4.48 \mathrm{~atm}\)

3) \(5.92 \mathrm{~atm}\)

4) \(29.4 \mathrm{~atm}\)

274. Isotonic solution have the same

1) Normality

2) Density

3) Molar concentration

4) None of these

275. An aqueous solution of glucose was prepared by dissolving \(18 \mathrm{~g}\) of glucose in \(90 \mathrm{~g}\) of water. The relative lowering in vapour pressure is

1) 0.01

2) 0.02

3) 1

4) 20

276. Pressure cooker reduces cooking time for food because

1) Boiling point of

2) Heat is more evenly water involved in distributed in the cooking is increased cooking space 3) The higher pressure 4) Cooking involves inside the cooker chemical changes crushes the food helped by a rise in material temperature

277. The freezing point of one modal \(\mathrm{NaCl}\) solution assuming \(\mathrm{NaCl}\) to be \(100 \%\) dissociated in water is (modal depression constant \(=1.86\) )

1) \(-2.72^{\circ} \mathrm{C}\)

\(2)^{-3.72^{\circ} \mathrm{C}}\)

3) \(2.72^{\circ} \mathrm{C}\)

4) \(3.72^{\circ} \mathrm{C}\)

278. The modal elevation constant of water is

\(0.52^{\circ} \mathrm{C}\). The boiling point of 1.0 modal aqueous \(\mathrm{KCl}\) solution (assuming complete dissociation of \(\mathrm{KCl})\), therefore, should be

1) \(98.96^{\circ} \mathrm{C}\)

2) \(100.52^{\circ} \mathrm{C}\)

3) \(101.04^{\circ} \mathrm{C}\)

4) \(107.01^{\circ} \mathrm{C}\)

279. Colligative properties are used for the determination of

1) Molar mass

2) Equivalent weigh

3) Arrangement of

4) Melting and boiling molecules points

280. The molecular weight of \(\mathrm{NaCl}\) determined by studying freezing point depression of its \(0.5 \%\) aqueous solution is 30 . The apparent degree of dissociation of \(\mathrm{NaCl}\) is

1) 0.60

2) 0.50

3) 0.30

4) 0.95

281. The molar freezing point constant for water is

\(1.86^{\circ} \mathrm{C} \mathrm{mol}^{-1}\). If \(342 \mathrm{~g}\) of cane sugar

\(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) is dissolved in \(1000 \mathrm{~g}\) of water, the solution will freeze at

1) \(-1.86^{\circ} \mathrm{C}\)

2)^{-2.86^{\circ} \mathrm{C}}\)

3) \(-1.86^{\circ} \mathrm{C}\)

4) \(+2.86^{\circ} \mathrm{C}\)

282. The freezing point depression of \(0.001 \mathrm{~m}\), \(K_{x}\left[F e(C N)_{6}\right]_{\text {is }} 7.10 \times 10^{-3} \mathrm{~K}\). If for water, \(k_{f}\) is \(1.86 \mathrm{~K} \mathrm{Kg} \mathrm{mol}^{-1}\), value of \(x\) will be

1) 4

2) 3

3) 2

4) 1

283. When \(10 \mathrm{~g}\) of a non-volatile solute is dissolved in \(100 \mathrm{~g}\) of benzene, it raises boiling point by \(1^{\circ} \mathrm{C}\) then molecular mass of the solute is \(\left(k_{b}\right.\) for \(\mathrm{C}_{6} \mathrm{H}_{6}=2.53 \mathrm{~kg}-\mathrm{mol}^{-1}\) )

1) \(223 \mathrm{~g}\)

2) \(233 \mathrm{~g}\)

3) \(243 \mathrm{~g}\)

4) \(253 \mathrm{~g}\)

284. If \(0.15 \mathrm{~g}\) of a solute dissolved in \(15 \mathrm{~g}\) of solvent is boiled at a temperature higher by \(0.216^{\circ} \mathrm{C}\) than that of the pure solvent, the molecular weight of the substance is (molal elevation constant for the solvent is \(2.16^{\circ} \mathrm{C}\) )

1) 100

2) 102

3) 104

4) 1.02

285. What is the freezing point of a solution containing \(8.1 \mathrm{~g} \mathrm{HBr}\) in \(100 \mathrm{~g}\) water assuming the acid to be \(90 \%\) ionised \(\left(k_{f}\right.\) for water \(\left.=1.86 \mathrm{~kg} \mathrm{~mol}^{-1}\right)\) ?

1) \(-0.35^{\circ} \mathrm{C}\)

2) \(-1.35^{\circ} \mathrm{C}\)

\(3)^{-2.35^{\circ} \mathrm{C}}\)

4) \(-3.53^{\circ} \mathrm{C}\)

286. Which of the following is a colligative property?

1) Boiling point

2) Freezing point

3) Osmotic pressure

4) Vapour pressure

287.0smatic pressure is 0.0821 atm at temperature of \(300 \mathrm{~K}\). Find concentration in mole per litre

1) 0.33

2) \(0.22 \times 10^{-2}\)

3) \(0.33 \times 10^{-2}\)

4) \(0.44 \times 10^{-2}\)

288. Which of the following solutions will have the highest boiling point?

1) \(0.1 \mathrm{MBaCl}_{2}\)

2) \(0.1 \mathrm{MFeCl}_{3}\)

3) \(0.1 \mathrm{M} \mathrm{NaCl}\)

4) 0.1 M urea

289. Which one of the statements given below concerning properties of solutions, describes a colligative effect?

1) Vapour pressure of 2)Boiling point of pure pure water water decreases by decreases by the the addition of addition of nitric ethanol acid

3) Boiling point of pure 4) Vapour pressure of benzene increases pure benzene by the addition of decreases by the toluene addition of naphthalene

290. At low concentrations, the statements that equimolal solutions under a given set of experimental conditions have equal osmotic pressure is true for

1) Solutions of

2) Solutions of non-electrolytes only electrolytes only 

3)All solutions

4) None of the above

291. Which of the following is incorrect?

1) Relative lowering of 2) Vapour pressure of a vapour pressure is solution is lower independent than the vapour pressure of the solvent

3) The vapour pressure 4) The relative lowering is a colligative of vapour pressure is property directly proportional to the mole fraction solute

292. Which of the following associated with isotonic solutions is not correct?

1) They will have the

2) They will have the same osmotic same vapour pressure pressure

3) They have same

4) Osmosis does not weight take place when the concentrations two solutions are separated by a semipermeable membrane

293. The relationship between osmotic pressure at \(273 \mathrm{~K}\) when \(10 \mathrm{~g}\) glucose \(\left(p_{1}\right), 10 \mathrm{~g}\) urea \(\left(p_{2}\right)\) and \(10 \mathrm{~g}\) sucrose \(\left(p_{3}\right)\) are dissolved in \(250 \mathrm{~mL}\) of water is

1) \(p_{1}>p_{2}>p_{3}\)

\({ }_{2)} p_{3}>p_{2}>p_{1}\)

3) \(p_{2}>p_{1}>p_{3}\)

4) \(p_{2}>p_{3}>p_{1}\)

294. Colligative properties of a solution depends upon

1) Nature of both

2) Nature of solute only solvent and solute

3) Nature of solvent

4) The relative number only of solute and solvent particles

295. Lowering of vapour pressure is highest for

1) \(0.1 \mathrm{MBaCl}_{2}\)

2) \(0.1 \mathrm{M}\) glucose

3) \(0.1 \mathrm{M} \mathrm{MgSO}_{4}\)

4) Urea

296. The amount of ice that will separate out on cooling a solute containing \(50 \mathrm{~g}\) of ethylene glycol in \(200 \mathrm{~g}\) water to \(-9.3^{\circ} \mathrm{C}\) will be

1) \(8.37 \mathrm{~g}\)

2) \(161.3 \mathrm{~g}\)

3) \(3.87 \mathrm{~g}\)

4) \(38.7 \mathrm{~g}\)

297.An aqueous solution of glucose is \(10 \%\) in strength. The volume in which \(1 \mathrm{~g}\)-mole of it is dissolved will be

1) \(0.18 \mathrm{~L}\)

2) \(1.8 \mathrm{~L}\)

3) \(0.9 \mathrm{~L}\)

4) \(9.0 \mathrm{~L}\)

298. The osmatic pressure of \(0.4 \%\) urea solution is \(1.66 \mathrm{~atm}\). and that of a solutions of sugar of \(3.42 \%\) is \(2.46 \mathrm{~atm}\). When both the solutions are mixed then the osmatic pressure of the resultant solution will be

1) \(1.02 \mathrm{~atm}\)

2) \(2.06 \mathrm{~atm}\)

3) \(3.04 \mathrm{~atm}\)

4) \(0.02 \mathrm{~atm}\)

299. Which of the following aqueous solutions produce the same osmotic pressure?

(i) \(0.1 \mathrm{M} \mathrm{NaCl}\) solution

(ii) \(0.1 \mathrm{M}\) glucose solution

(iii) \(0.6 \mathrm{~g}\) urea in \(100 \mathrm{~mL}\) solution

(iv) \(1.0 \mathrm{~g}\) of a non-electrolyte solute \((X)\) in 50

mL solution (molar mass of \(X=200\) )

1)(i), (ii), (iii)

2) (ii), (iii), (iv)

3)(i), (ii), (iv)

4) (i), (iii), (iv)

300. In a 0.2 molal aqueous solution of a weak acid \(H X\), the degree of ionization is 0.3 . Taking \(K_{f}\) for water as 1.85 , the freezing point of the solution will be nearest to

1) \(-360^{\circ} \mathrm{C}\)

2) \(0.260^{\circ} \mathrm{C}\)

3) ^{0.480^{\circ} \mathrm{C}}\)

4)^{-0.480^{\circ} \mathrm{C}}\)

301. Two solutions of glucose have osmotic pressure 1.0 and \(3.5 \mathrm{~atm}\). If \(1 \mathrm{~L}\) of first solution is mixed with \(V \mathrm{~L}\) of second solution, the osmotic pressure of the resultant solution becomes \(2.5 \mathrm{~atm}\). Volume of second solution is

1) \(1.0 \mathrm{~L}\)

2) \(1.5 \mathrm{~L}\)

3) \(2.5 \mathrm{~L}\)

4) \(3.5 \mathrm{~L}\)

302.A \(0.025 \mathrm{M}\) solution of monobasic acid had a freezing point of \(-0.060^{\circ} \mathrm{C}\). The \(p K_{a}\) for the acid is

1) 1.2

2) 2

3) 2.5

4) 5.7

303. Two solutions of \(\mathrm{KNO}_{3}\) and \(\mathrm{CH}_{3} \mathrm{COOH}\) are prepared separately. Molarity of both is \(0.1 \mathrm{M}\) and osmatic pressures are \(p_{1}\) and \(p_{2}\) respectively. The correct relationship between the osmatic pressures is

1) \(p_{1}=p_{2}\)

2) \(p_{1}>p_{2}\) 

\({ }_{3)} p_{2}>p_{1}\)

4) \(\frac{p_{1}}{p_{1}+p_{2}}+\frac{p_{2}}{p_{1}+p_{2}}\)

304. The molarity of pure water is

1) 55.6

2) 5.56

3) 6.55

4) 65.5

305. If for a sucrose solution elevation in boiling point is \(0.1^{\circ} \mathrm{C}\) then what will be boiling point of \(\mathrm{NaCl}\) solution for the same molal concentration?

1) 0.1

2) 0.2

3) 0.16

4) 0.26

306. Increasing the temperature of an aqueous solution will cause

1) Decrease in molarity 2) Decrease in molarity

3) Decrease in mole fraction

4) Decrease in \(\% w / w\)

307.0.1 molal aqueous solution of \(\mathrm{NaBr}\) freezes at - \(0.335^{\circ} \mathrm{C}\) at atmospheric pressure \(k_{f}\) for water is \(1.86^{\circ} \mathrm{C}\). The percentage of dissociation of the salt in solution is

1) 90

2) 80

3) 58

4) 98

308. How many grams of a sucrose (mol \(w t .=342)\) should be dissolved in \(100 \mathrm{~g}\) water in order to produce a solution with a \(105.0^{\circ} \mathrm{C}\) difference between the freezing point and boiling temperature? \(\left(k_{f}=1.86 \mathrm{C} / \mathrm{m}, k_{b}=0.151^{\circ} \mathrm{C}\right)\)

1) \(34.2 \mathrm{~g}\)

2) \(72 \mathrm{~g}\)

3) \(342 \mathrm{~g}\)

4) \(460 \mathrm{~g}\)

309. The osmatic pressure of a 5\% (wt./vol) solution of cane sugar at \(150^{\circ} \mathrm{C}\) is

1) \(3.078 \mathrm{~atm}\)

2) \(4.078 \mathrm{~atm}\)

3) \(5.078 \mathrm{~atm}\)

4) \(2.45 \mathrm{~atm}\)

310. The azeotropic mixture of water (b. pt. \(100^{\circ} \mathrm{C}\) ) and \(\mathrm{HCl}\) (b.pt. \(85^{\circ} \mathrm{C}\) ) boils at \(108.5^{\circ} \mathrm{C}\). When this mixture is distilled it is possible to obtain

1) Pure \(\mathrm{HCl}\)

2) Pure water

3) Pure water as well as Neither \(\mathrm{HCl}\) nor \(\mathrm{H}_{2} \mathrm{O}\) \(\mathrm{HCl}\) in their pure states

311. Which of the following compounds correspond to maximum van'thoff factor for dilute solution?

1) \(\mathrm{HCl}\)

2) \(\mathrm{MgSO}_{4}\)

3) \(\mathrm{K}_{2} \mathrm{SO}_{4}\)

4) \(K_{4} F e(C N)_{6}\)

312. Which of the following solution in water possesses the lowest vapour pressure?

1) \(0.1(N) \mathrm{BaCl}_{2}\)

2) \(0.1(\mathrm{M}) \mathrm{NaCl}\)

3) 0.1 (M) \(\mathrm{KCl}\)

4) None of these

313. A certain substance ' \(A\) ' tetramerises in water to the extent of \(80 \%\). A solution of \(2.5 \mathrm{~g}\) of \(A\) in \(100 \mathrm{~g}\) of water lowers the freezing point by \(0.3^{\circ} \mathrm{C}\). The molar mass of \(A\) is

1) 31

2) 62

3) 122

4) 244

314. \(6.02 \times 10^{20}\) molecules of urea are present in 100 \(\mathrm{mL}\) of its solution. The concentration of urea solution is

1) \(0.1 \mathrm{M}\)

2) \(0.01 \mathrm{M}\)

3) \(0.001 \mathrm{M}\)

4) \(0.02 \mathrm{M}\)

315. The vant's Hoff factor for \(0.1 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) solution is 2.74. The degree of dissociation is

1) \(91.3 \%\)

2) \(87 \%\)

3) \(100 \%\)

4) \(74 \%\)

316. Which one of the following aqueous solutions will exhibit highest boiling point?

1) \(0.01 \mathrm{MNa}_{2} \mathrm{SO}_{4}\)

2) \(0.01 \mathrm{MKNO}_{3}\)

3) \(0.015 \mathrm{M}\) urea

4) \(0.015 \mathrm{M}\) glucose

317. The average osmotic pressure of human blood is 7.8 bar at \(37^{\circ} \mathrm{C}\). What is the concentration of an aqueous \(\mathrm{NaCl}\) solution that could be used in the blood steam?

1) \(0.16 \mathrm{~mol} / \mathrm{L}\)

2) \(0.31 \mathrm{~mol} / \mathrm{L}\)

3) \(0.60 \mathrm{~mol} / \mathrm{L}\)

4) \(0.45 \mathrm{~mol} / \mathrm{L}\)

318. When mercuric iodide is added to the aqueous solution of potassium iodide, the

1) Freezing point is

2) Freezing point is raised lowered

3) Freezing point does

4) Boiling point does not change not change

319. The mole fraction of water in \(20 \%\) aqueous solution of \(\mathrm{H}_{2} \mathrm{O}_{2}\) is

1) \(\frac{20}{80}\)

2) \(\frac{80}{20}\)

3) \(\frac{68}{77}\)

4) \(\frac{77}{68}\)

320. The mole fraction of the solute in one modal aqueous solution is

1) 0.018

2) 0.027

3) 0.036

4) 0.048

\section{Multiple Correct Answers Type}

321. Molecular weight of urea is 60 . A solution of urea containing \(6 \mathrm{~g}\) of urea in one litre is a 

1) \(1 \mathrm{~N}\)

2) \(0.1 \mathrm{M}\)

3) \(0.1 \mathrm{~N}\)

4) \(1 \mathrm{M}\)

322. The solution (s) which will boil at the highest temperature is/are

1) \(0.1 \mathrm{M}\) urea

2) \(0.1 \mathrm{MHNO}_{3}\)

3)

4) \(0.1 \mathrm{MBaCl}_{2}\)

323. Which of the following is/are not affected by temperature?

1) Molarity

2) Molality

3) Normality

4) Mole fraction

324. Osmotic pressure in dilute solution is

1) Inversely

2) Directly proportional

proportional to the to temperature

moles of non-volatile

solution

3) Directly

4) Independent of

proportional to the temperature and

molarity of solution moles of solute dissolved

325. The dissolution of which of the following compounds is exothermic

1) \(\mathrm{Na}_{2} \mathrm{SO}_{4}\)

2) \(\mathrm{NaOH}\)

3) \(\mathrm{CaCl}_{2}\)

4) \(L i B r\)

\section{Assertion - Reasoning Type}

This section contain(s) 12 question(s) numbered 326 to 337. Each question containsSTATEMENT 1(Assertion) and STATEMENT 2(Reason). Each question has the 4 choices (1), (2), (3) and (4) out of which ONLY ONE is correct.

1) Statement 1 is True, Statement 2 is True; Statement 2 is correct explanation for Statement 1

2) Statement 1 is True, Statement 2 is True; Statement 2 is not correct explanation for Statement 1

3) Statement 1 is True, Statement 2 is False

4) Statement 1 is False, Statement 2 is True 326

Statement 1: The mass of acetic acid molecule in benzene is more than the actual value of the solute. Statement 2: Molecules of acetic acid dimerise in benzene due to hydrogen bonding.

327

Statement 1: Azeotropic mixture are formed only by nonideal solution and they may have boiling points either greater than both the components or less than both the components.

Statement 2: The composition of the vapour phase is same as that of the liquid phase of an azeotropic mixture.

Statement 1: If a liquid solute more volatile than the solvent is added to the solvent the vapour pressure of the solution may increase ie \(\mathrm{P}_{\mathrm{s}}>\mathrm{P}^{0}\).

Statement 2: In presence of a more volatile liquid solute only the solute will form the vapour and solvent will not.

Statement 1: \(\quad\) The boiling point of \(0.1 \mathrm{M}\) urea solution is less than that of \(0.1 \mathrm{M} \mathrm{KCl}\) solution.

Statement 2: Elevation of boiling point is directly proportional to the number of species present in the solution.

330

Statement 1: The water pouch of instant cold pack for treating athletic injuries breaks when squeezed and \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) dissolves lowering point of temperature.

Statement 2: Addition of non volatile solute into solvent result in depression of freezing point solvent. Statement 1: If red blood cells were removed from the body and placed in pure water pressure inside the cells increase.

Statement 2: The concentration of salt content in the cells increase.

332

Statement 1: The molecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different.

Statement 2: Water is polar and benzene is non polar.

333

Statement 1: The elevation in boiling point of a solution of non-electrolyte is proportional to its molality

Statement 2: The molal elevation constant is the ratio of the elevation in boiling point to its molality

334

Statement 1: The difference in the boiling points of equimolar solution of \(\mathrm{HCl}\) and \(\mathrm{HF}\) decreases as their molarity is decreased

Statement 2: The extent of dissociation decreases steadily with increasing dilution

335

Statement 1: \(\Delta H_{\text {mix }}\) and \(\Delta V_{\text {mix }}\) in an ideal solution are zero

Statement 2: \(A-B\) interactions in ideal solutions are same as between \(A-B\) and \(B-B\)

336

Statement 1: On adding \(\mathrm{NaCl}\) to water its vapour pressure increase

Statement 2: Addition of non-volatile solute decreases the vapour pressure 

3) 0.75

4) 0.15

Paragraph for Question Nos. 341 - 343

The variation of vapour pressure of the solvent and that of the solution with temperature are given by the respective solvent-vapour and solution-vapour curves of the phase diagram

For a given value of the external pressure, the pure solvent will boil at temperature \(T_{b}^{*}\) and at temperature \(T_{b}\) let \(p_{e x t}\) be equal to \(p^{*}\), the vapour pressure of pure solvent

Applying the Clausius-Clapeyron equation to the solution vapour equilibrium for the two values of \(p, T_{b}^{*}\) and \(p^{*}, T_{b}\) we have

In \(\frac{p^{*}}{p}=\frac{\Delta_{v a p} H_{1 m}}{R}\left(\frac{1}{T_{b}^{*}}-\frac{1}{T_{b}}\right)\)

\(=\frac{\Delta_{v a p} H_{1 m}}{R} \frac{\Delta T_{b}}{T_{b}^{*} T_{b}}\)

341.The phase diagram for the pure solvent and solution are recorded below. The quantity indicated by \(\mathrm{L}\) in the figure is


1) \(\Delta p\)

2) \(k_{b} \cdot m\)

3) \(k_{f}^{m}\)

4) \(m\)

342.The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with equimolar solution of benzene and toluene is

1) 0.50

2) 0.93

3) 0.6

4) 0.27

343.At certain hill-station, pure water boils at 99. \(725^{\circ} \mathrm{C}\). If \(K_{b}\) for water is \(0.513^{\circ} \mathrm{C} \mathrm{kg} \mathrm{mol}\), the boiling point of \(0.69 \mathrm{~m}\) solution of urea will be

1) \(100.359^{\circ} \mathrm{C}\)

2) \(103^{\circ} \mathrm{C}\)

3) \(100.073^{\circ} \mathrm{C}\)

4) Unpredictable