Solutions

A solution where the solvent is in the solid state and the solute is in the gaseous state is exemplified by:

In a binary solution, if component A is $30\%$ and component B is $70\%$, B is typically called the:

Identify the 'gas-in-liquid' solution from the options below:

Which of the following components of 22-carat gold is the solute?

Which of the following correctly pairs the solution with its type?

A solution of ethylene glycol in water (antifreeze) is which type of solution?

When two or more gases are mixed together, the resulting solution is always:

In the 'Types of Solutions', where would you classify 'Dust particles in the air'?

Which of the following characterizes a 'Liquid in Liquid' solution that forms a maximum boiling azeotrope?

How is a 'Gas in Gas' solution different from other solution types in terms of miscibility?

When a gas is in equilibrium with its solution, the rate of gas molecules entering the liquid is ________ the rate of gas molecules leaving the liquid.

The constant $K_H$ in Henry's Law is often expressed in kilobars. $1$ bar is approximately equal to:

If a gas follows Henry's Law, what will happen to its solubility if the temperature is decreased?

What is the consequence of high partial pressure of $O_2$ in the lungs?

Two gases, $A$ and $B$, are dissolved in a solvent at $298$ K. The mole fractions of these gases in the solution at a partial pressure of $1$ bar are provided in the diagram. Which of the following correctly identifies their Henry's law constants ($K_H$) and the relative slopes of their partial pressure ($p$) versus mole fraction ($x$) plots?

Which of the following describes the effect of increasing the partial pressure of a gas above a liquid at equilibrium?

At $298$ K, the Henry's Law constant for $N_2$ is $8.42 \times 10^{-7}$ $M/mmHg$. What is the molarity of $N_2$ in water saturated with air at $760$ mmHg? (Assume air is $78\%$ $N_2$).

If the Henry's Law constant for $N_2$ is $1.0 \times 10^5 \text{ atm}$ and the mole fraction of $N_2$ in air is $0.8$, calculate the number of moles of $N_2$ dissolved in $10 \text{ moles}$ of water at a total pressure of $5 \text{ atm}$.

Why is the solubility of $O_2$ in blood much higher than its solubility in water at the same partial pressure?

The $K_H$ of $CO_2$ in water at $298 \text{ K}$ is $1.67 \text{ kbar}$. Find the molality of $CO_2$ in water at $298 \text{ K}$ and $P_{CO2} = 1 \text{ bar}$.

The total vapour pressure of an ideal solution is a linear function of:

What is the vapour pressure of a solution of glucose in water at $100^\circ C$ compared to pure water?

Relative lowering of vapour pressure is a property that depends on:

For a binary solution, if the vapour pressure of the solution is lower than expected by Raoult's law, the boiling point will be:

If we double the mole fraction of a non-volatile solute in a very dilute ideal solution, the relative lowering of vapour pressure will:

A solution is made by mixing $32\text{ g}$ of methanol ($M=32$) and $46\text{ g}$ of ethanol ($M=46$). If $p_{meth}^0 = 90\text{ mmHg}$ and $p_{eth}^0 = 50\text{ mmHg}$, what is the total pressure?

In a mixture of $A$ and $B$, if the $A-B$ forces are stronger than $A-A$ and $B-B$ forces, what happens to the vapour pressure?

In the graph of $P_{total}$ vs $x_A$ for a solution showing positive deviation, the curve:

A solution is prepared by mixing 2 moles of liquid $A$ and 3 moles of liquid $B$. If $P_A^o = 100$ and $P_B^o = 150$, what is the total vapour pressure and the mole fraction of $A$ in the vapour?

If two liquids $A$ and $B$ form an ideal solution, the total pressure is $P$. The mole fraction of $A$ in the vapour phase ($y_A$) is given by:

For a non-ideal solution, the Raoult's Law vapor pressure curve is:

When ethyl alcohol is added to cyclohexane, the hydrogen bonds between alcohol molecules are broken. This leads to:

A $95\%$ ethanol-water mixture is a common example of:

Which of the following represents the correct order of forces in a solution showing positive deviation?

In the formation of a binary liquid solution of components $A$ and $B$, the enthalpy change for breaking $A-A$ and $B-B$ interactions (cohesive forces) is represented by Step 1, and the enthalpy change for forming $A-B$ interactions (adhesive forces) is represented by Step 2. If the magnitude of energy released in Step 2 is significantly greater than the energy consumed in Step 1, which of the following set of properties will the resulting solution exhibit?

Which of the following statements about maximum boiling azeotropes is correct?

The vapor pressure of a solution of $X$ and $Y$ follows the line $P = P_X^0 x_X + P_Y^0 x_Y$ throughout the entire concentration range. This solution is:

When volatile liquids $A$ and $B$ are mixed to form a non-ideal solution, the temperature of the mixture is observed to decrease relative to the initial temperatures of the pure components. This behavior is modeled using the activity coefficient relationship $\ln \gamma_A = \alpha x_B^2$, where $x_B$ is the mole fraction of component $B$ and $\alpha$ is a constant. Which of the following statements correctly identifies the sign of $\alpha$ and the type of azeotrope formed by this system?

Which of the following conditions is common to both ideal solutions and solutions with positive/negative deviations?

If the molar enthalpy of vaporization of pure liquid A is $\Delta H_{vap,A}$ and for pure liquid B is $\Delta H_{vap,B}$, and the solution shows negative deviation, the enthalpy of vaporization of the azeotrope will be:

The primary objective of studying colligative properties in high school chemistry is to determine the:

What is the van't Hoff factor ($i$) for an aqueous solution of glucose?

When Acetic acid is dissolved in benzene, it undergoes dimerization. What is the value of the van't Hoff factor ($i$) for this process assuming complete dimerization?

Which of the following is a common unit used to measure osmotic pressure?

Identify the relationship between molar mass ($M$) and the depression in freezing point ($\Delta T_f$).

Assuming complete dissociation, which of the following has the highest boiling point?

A $1\%$ (mass/vol) solution of $KCl$ was found to possess an osmotic pressure of $5.73\ atm$ at $300\ K$. Calculate the Van't Hoff factor for $KCl$ at this concentration. ($R = 0.0821\ L\ atm\ K^{-1}\ mol^{-1}$, Molar mass of $KCl = 74.5$)

Two solutions $X$ and $Y$ are prepared. $X$ contains $10\ g$ urea in $100\ mL$ and $Y$ contains $10\ g$ glucose in $100\ mL$. Which of the following is correct?

In the relation $\Delta T_f = i K_f m$, what does 'm' represent?

Which constant is dependent only on the nature of the solvent and not the solute?

What happens to the colligative property if a solute dissociates?

In a case of 100% dissociation, if $i=5$, the salt could be:

If $i = 1 + \\alpha$, the solute must be of the type:

Which solute will have a van't Hoff factor of 1?

If the van't Hoff factor for a $0.05 \text{ M}$ solution of an electrolyte is $2.0$, and the electrolyte is $AB_2$, the degree of dissociation is:

The molar mass of acetic acid is $60 \text{ g/mol}$. In benzene, it forms dimers and its observed molar mass is $110 \text{ g/mol}$. The degree of association is approximately:

For a solute which undergoes tetramerization, the van't Hoff factor for complete association is:

An aqueous solution of $FeCl_3$ shows a van't Hoff factor of $3.2$. What is its degree of dissociation?

The osmotic pressure of a solution of $MgCl_2$ is $5.0\text{ atm}$ at $300\text{ K}$. If the concentration is $0.1\text{ M}$, calculate the van't Hoff factor.

The van't Hoff factor for $BaCl_2$ at $0.01\text{ M}$ concentration is $2.50$. What is the percentage of dissociation?

What is the sum of the mole fractions of components A, B, and C in a ternary solution?

For a solution where the density is $1\text{ g/mL}$, which of the following is true?

What is the mass of glucose ($\text{C}_6\text{H}_{12}\text{O}_6$) required to prepare $100\text{ g}$ of a $5\% (w/w)$ solution?

Molality is preferred over molarity in experimental chemistry because:

What is the molarity of a solution when 4 g of $NaOH$ is dissolved in enough water to make 100 mL of solution?

A solution contains 25% water, 25% ethanol and 50% acetic acid by mass. Calculate the mole fraction of water.

Molarity (M) is defined as:

What is the mass of $Na_2S_2O_3 \cdot 5H_2O$ (molar mass $= 248$) needed to prepare $500\ mL$ of $0.125\ M$ solution?

Calculate the molality of $1\ L$ of $93\%$ $H_2SO_4$ ($w/v$) if the density of the solution is $1.84\ g/mL$.

A $40\%$ by weight solution of $H_2SO_4$ has a density of $1.30\ g/mL$. Its molarity is: