Solutions

What is the solute in 'Mist' or 'Fog' which are considered liquid in gas systems?

Which of the following substances forms a non-aqueous solution when dissolved in carbon tetrachloride?

An example of a 'Solid in Solid' solution found in jewelry is:

When a small amount of liquid solute is dissolved in a large amount of solid solvent, the solution is called:

Binary solutions are classified into nine distinct types based on the physical state of the solute and the solvent. Based on the components and their states illustrated in the flowchart below, which substance is a correct example of the resulting solution?

The property 'like dissolves like' explains why:

Which of the following solutions contains a solid solvent?

The total vapor pressure of a solution containing $1\text{ mole}$ of $A$ and $2\text{ moles}$ of $B$ is $450\text{ torr}$. If the vapor pressure of pure $A$ is $400\text{ torr}$ and that of pure $B$ is $500\text{ torr}$, calculate the deviation from Raoult's law if any.

Which of the following pairs is most likely to form a nearly ideal solution?

Why does a solution of Ethanol and Cyclohexane show a positive deviation from Raoult's Law?

Which of the following is an application of Henry's Law in the human body?

The solubility of $CO_2$ in water at $298 K$ is higher than that of $O_2$. This means the $K_H$ value of $CO_2$ is:

Which property of a gas makes it follow Henry's law more closely?

A diver in deep sea breathes air at a higher pressure than at the surface. What is the effect on the amount of dissolved nitrogen in their blood?

What is the reason why Nitrogen is not used alone by deep-sea divers and is instead diluted with Helium?

Which of the following statements about $K_H$ is FALSE?

Which graph correctly depicts Henry's Law for a gas-liquid solution?

Given that $K_H$ for $CO_2$ in water at $298\ K$ is $1.67 \times 10^8\ Pa$. If the total pressure of a mixture of $CO_2$ and $H_2O$ vapor is $101.325\ kPa$ and the mole fraction of $CO_2$ in the gas phase is $0.5$, calculate the mole fraction of $CO_2$ in the liquid phase.

How does the value of Henry's constant $K_H$ relate to the intermolecular forces between the gas and the solvent?

At $298\ K$, the Henry's law constant for $H_2S$ in water is $0.1\ mol\cdot kg^{-1}\cdot bar^{-1}$. If $H_2S$ is used for the qualitative analysis of metal ions and its solubility is $0.185\ m$, what is the pressure of $H_2S$ applied?

Vapor pressure is a:

A solution of two volatile liquids A and B has $P_A^\circ = 200$ and $P_B^\circ = 300$. If the mole fraction of A is $0.4$, what is the partial pressure of B?

An ideal solution is formed when its components have:

If the intermolecular forces between molecules A and B are stronger than those between A-A or B-B, the solution will show:

Two aqueous solutions are prepared using the same non-volatile solute and pure water. Solution A contains $1\text{ mole}$ of solute dissolved in $10\text{ moles}$ of water, while Solution B contains $2\text{ moles}$ of the same solute dissolved in $10\text{ moles}$ of water. If $P^\circ$ is the vapor pressure of pure water, and $P_A$ and $P_B$ are the vapor pressures of solutions A and B respectively at the same temperature, which of the following relationships is correct?

At a constant temperature, a liquid mixture of two volatile components, X ($P_X^\circ = 200\text{ mm Hg}$) and Y ($P_Y^\circ = 50\text{ mm Hg}$), is prepared with equal number of moles of each component. This mixture is in equilibrium with its vapor. According to Raoult's Law and Dalton's Law, what is the ratio of the mole fractions of X to Y in the vapor phase ($y_X : y_Y$)?

Benzene and toluene form an nearly ideal solution. At $313\text{ K}$, the vapor pressure of pure benzene is $160\text{ mm Hg}$ and pure toluene is $60\text{ mm Hg}$. What is the total vapor pressure of a mixture containing equal masses of benzene and toluene? (Molar masses: Benzene = $78$, Toluene = $92$)

What is the mole fraction of a non-volatile solute in a solvent if the vapor pressure of the solution is $0.5\text{ atm}$ and the pure solvent vapor pressure is $0.8\text{ atm}$?

In a dilute solution of a non-volatile solute, the mole fraction of the solute is $0.02$. What is the ratio of the vapor pressure of the solution to that of the pure solvent?

The total vapor pressure of a mixture of $1\text{ mole}$ of A ($P_A^\circ = 150\text{ torr}$) and $2\text{ moles}$ of B ($P_B^\circ = 240\text{ torr}$) is $200\text{ torr}$. In this mixture:

When comparing two solutions, if Solution 1 is ideal and Solution 2 shows negative deviation, which will have a higher boiling point if their pure components are the same?

Binary mixtures having the same composition in liquid and vapor phase and boiling at a constant temperature are called ___.

At the composition of a maximum boiling azeotrope, the vapor pressure of the solution is at its:

Which of these is a characteristic of a solution showing negative deviation?

At the azeotropic point of a binary mixture, the mole fraction of component $A$ in the liquid phase ($X_A$) and the mole fraction of $A$ in the vapor phase ($Y_A$) are related as:

For two liquids $A$ and $B$, if $P_A^0 = 200$ mm Hg and $P_B^0 = 100$ mm Hg, the mole fraction of $A$ in a solution that has a total vapor pressure of $150$ mm Hg (assuming ideality) is:

Which of the following is not true for a solution showing positive deviation?

When Ethanol and Acetone are mixed, the $A-B$ interactions are weaker than $A-A$ or $B-B$ interactions. What is the expected sign of the derivative of the total pressure with respect to mole fraction ($dP/dx_A$) at the point of azeotropy?

In the context of non-ideal solutions, what does the 'Lever Rule' help determine on a pressure-composition phase diagram?

A solution contains components $A$ and $B$. If the partial vapor pressure of $A$ is $P_A$ and it is found that $P_A/x_A > P_A^o$, what can you conclude about the intermolecular forces?

The osmotic pressure of a solution increases if:

Which of the following is equal to the depression in freezing point for a 1 molal solution?

Sea water is desalinated using which of the following processes?

The abnormal molar mass of a solute is observed when there is:

Relative lowering of vapor pressure is a colligative property because it depends on:

Which of the following aqueous solutions has the highest freezing point?

For a dilute solution containing a non-volatile solute, the molar mass of the solute ($M_2$) can be calculated using relative lowering of vapor pressure as:

Two elements $A$ and $B$ form compounds $AB_2$ and $AB_4$. When dissolved in $20\ g$ of benzene, $1\ g$ of $AB_2$ lowers the freezing point by $2.3\ K$ and $1\ g$ of $AB_4$ lowers it by $1.3\ K$. The atomic masses of $A$ and $B$ are ($K_f$ for benzene = $5.1$):

The ratio of the elevation in boiling point for $0.1\ m\ NaCl$ and $0.1\ m\ Na_2SO_4$ (assuming $100\%$ dissociation) is:

A $0.01\ m$ aqueous solution of $AlCl_3$ freezes at $-0.068^{\circ}C$. The van't Hoff factor is ($K_f = 1.86$):

Which of the following describes a solution with an osmotic pressure lower than that of another solution?

For a very dilute solution, the osmotic pressure is proportional to the number of ________ of the solute in a given volume.

Which constant is numerically the same as the Ideal Gas Constant '$R$' used in the Van't Hoff equation?

The process of 'pickling' vegetables involves high salt concentrations to prevent bacterial growth through which mechanism?

Two solutions $X$ and $Y$ are separated by a semi-permeable membrane. If the osmotic pressure of $X$ is greater than that of $Y$, then:

If the osmotic pressure of a dilute solution is $8.21\text{ atm}$ at $300\text{ K}$, what is the concentration in moles per litre? ($R = 0.0821$)

The molarity ($M$) of a solution is related to osmotic pressure ($\pi$) by the relation $\pi = MRT$. If $\pi$ is in atm and $T$ in K, the units of $R$ are:

A $1.17\% (w/v)$ $NaCl$ solution is isotonic with a $7.2\% (w/v)$ solution of a non-electrolyte. The molar mass of the non-electrolyte is:

Calculate the osmotic pressure of a $0.1\text{ M}$ solution of $Na_2SO_4$ that is $70\%$ dissociated at $27^{\circ}\text{C}$.

Which of the following will have the same osmotic pressure as a $0.1\text{ M} NaCl$ solution (assume 100% dissociation)?

Which salt will show the same Van't Hoff factor as $Mg(NO_3)_2$ for 100% dissociation?

A solute has a Van't Hoff factor of 0.75. This indicates that the solute:

When $NaCl$ is added to water, the observed osmotic pressure is higher than the calculated one because:

If a solute undergoes trimerization, the value of '$n$' in the association formula ($i = 1 + (1/n - 1)\alpha$) is:

What is the apparent molecular weight of $NaCl$ (theoretical $58.5$) in water if it is 90% dissociated?

If a substance $X$ is 100% associated into dimers, its Van't Hoff factor is:

The depression in freezing point for $1 \text{ m}$ urea, $1 \text{ m}$ $NaCl$, and $1 \text{ m}$ $CaCl_2$ solutions are in the ratio:

What is the degree of dissociation of a weak electrolyte $A_2B_3$ if the Van't Hoff factor is $3.4$?

Which of the following will show a Van't Hoff factor of 1.0?

A solution of $1.25\ g$ of an unknown solute in $20\ g$ of benzene freezes at $4.5^{\circ}C$. Pure benzene freezes at $5.5^{\circ}C$. If the solute is known to be $100\%$ dimerized and $K_f = 5.12$, find the actual molar mass of the solute.

If a salt $XY_{2}$ dissociates as $XY_{2} \\rightarrow X^{2+} + 2Y^{-}$, and the degree of dissociation is $\\alpha$, then $i$ is:

The Van't Hoff factor ($i$) for an aqueous solution of Ethylene glycol is:

What is the Van't Hoff factor ($i$) for $K_{3}[Fe(CN)_{6}]$ assuming $100\%$ dissociation?

For a solute that neither associates nor dissociates, the ratio of observed to calculated osmotic pressure is:

An aqueous solution of $FeCl_{3}$ has a Van't Hoff factor of $3.1$. What is its degree of dissociation?

Which of the following values of $i$ is impossible for a solute that can only associate or stay as a monomer?

Two solutions $0.1\,M$ $NaCl$ and $0.1\,M$ $Na_{2}SO_{4}$ are compared. The ratio of their boiling point elevations ($\Delta T_{b1} / \Delta T_{b2}$) assuming complete ionization is:

If the osmotic pressure of a $0.1\,M$ solution of $CuSO_4$ is $3.5\,atm$ at $27^{\circ}C$, the degree of dissociation is:

The Van't Hoff factor of a $0.1\,m$ $La(NO_3)_3$ solution is $3.42$. What is the percentage dissociation?

What is the Van't Hoff factor for a $0.01\,m$ solution of $CH_3COOH$ if its $K_a = 1.8 \times 10^{-5}$?