The Amazing World of Solutes, Solvents, and Solutions

Mouthwash often contains a small amount of peppermint oil dissolved in alcohol and water. Peppermint oil is an example of a:

If you mix a packet of instant coffee powder into a mug of hot water, the coffee powder is the:

In a solution of 'milk of magnesia', small particles are dispersed but if we consider a clear solution of Epsom salt in water, the salt is the:

When we dissolve some solid naphthalene in benzene, the naphthalene acts as the:

A student adds a spoonful of honey to a cup of hot tea. After stirring, the honey is no longer visible as a separate layer. In this solution, honey is the:

Sea water contains various dissolved salts and gases. What acts as the solvent in sea water?

In a solution of $0.9\%$ Sodium Chloride (Normal Saline), identify the solvent.

When you dissolve $50$ g of sucrose (cane sugar) in $100$ ml of water at high temperature, it forms a thick syrup. In this case, what is the solvent?

In 'Rose Metal', a low-melting alloy of $50\%$ Bismuth, $25\%$ Lead, and $25\%$ Tin, which metal acts as the solvent?

An experiment uses a solution of $5$ ml of bromine liquid in $100$ ml of chloroform. Identify the solute and the solvent.

A solution of iodine in alcohol is known as:

Why can a true solution pass through a filter paper without leaving any residue?

If $50 \text{ g}$ of sugar is present in $250 \text{ g}$ of a sugar solution, what is the concentration in terms of mass percentage?

Stainless steel is an alloy of iron, carbon, and metals like chromium and nickel. It is considered a:

If the concentration of a solution is $10\%$ by mass and the mass of the solution is $150 g$, calculate the mass of the solvent.

A solution that contains less than the maximum possible amount of solute at a given temperature is called:

Which of these is a heterogeneous mixture that might be mistaken for a solution but eventually settles?

A student performs the experiment illustrated in the flowchart below. They start with $500$ g of a sugar solution with a concentration of $20\%$ by mass. From this container, $100$ g of the solution is removed and then replaced by $100$ g of pure distilled water. After thorough stirring to ensure homogeneity, what is the final concentration (mass by mass percentage) of the sugar in solution 'X'?

Which component acts as the solvent in a solution of 'Air'?

If you have $250$ g of a $12\%$ sugar solution, how much sugar is left in the container if all the water is evaporated?

Sea water is a complex solution. Which of the following is a primary solute in it?

If you have an unsaturated solution of sugar, you can make it saturated by:

Which state of matter can act as a solvent?

In a solution of Iodine in Alcohol, which component is present in a larger amount?

A student adds a solid solute to $100$ mL of water at $20^{\circ}C$ in sequential steps as shown in the flowchart. Based on the observations, which statement correctly describes the solution at Stage C?

Which of the following describes the ratio of components in a solution?

In the context of solutions, what does 'diffusion' refer to?

Identify which of the following is an example of a 'gas in liquid' solution.

If the solubility of a salt is $30g$ at $20^\circ C$ and $50g$ at $60^\circ C$, what is the concentration of a saturated solution at $60^\circ C$ in terms of mass percentage?

The mass of a solution is $540g$ and it contains $40g$ of solute. What is the mass of the solvent?

What is the name for a mixture that is the same throughout (uniform)?

If you want to dissolve a solid in a liquid very slowly, you should:

Vinegar is a solution of acetic acid in water. What is the solute in vinegar?

Which of these is NOT a factor that affects how fast a solid dissolves in a liquid?

Identify the factors that contribute to the 'Speed of Dissolving' based on the following summary diagram.

How does increasing the pressure affect the rate and solubility of a solid solute in a liquid solvent?

What is the primary difference between a saturated and an unsaturated solution at a given temperature?

In which of the following cases would the rate of dissolution be highest?

Why is it harder to dissolve a second spoonful of sugar in a glass of water than the first spoonful?

How does the 'Lattice Energy' of a solid crystal compare to the 'Solvation Energy' during a fast dissolution process?

A student prepares a solution by dissolving $15g$ of glucose in enough water to make the total volume of the solution $100mL$. Based on the diagram, what is the concentration of this solution expressed as a mass by volume percentage?

Two liquids that mix completely with each other to form a solution are said to be:

If $40g$ of sugar is dissolved in $160g$ of water, what is the mass by mass percentage of the solution?

Which of the following increases the solubility of a gas in a liquid?

If the mass of the solute is $w$ and the mass of the solvent is $W$, the mass percentage of the solution is given by:

Which of the following can be separated from its solvent by the process of evaporation?

In a solution of vinegar (acetic acid in water), water is the:

A solution has a mass/mass percentage of $25\%$. If the mass of the solvent is $300$ g, find the mass of the solute.

If the mass of a saturated solution is $150$ g and it contains $30$ g of solute, what is the solubility of the solute?

If a solution is $5\% (m/m)$, how much solution will contain $2.5$ g of solute?

Which of these is NOT a characteristic of a solution?

A solution of iodine in alcohol is known as:

The component of a solution that is present in the largest amount is the:

Which of these mixtures is homogeneous?

Bronze is a solid solution (alloy) often used to make medals and statues. Based on the composition shown in the diagram, which of the following correctly identifies the solute and solvent in this solution?

When a gas (Substance X) is dissolved in a liquid (Substance Y) to form a liquid solution (Z), as shown in the diagram, which statement correctly identifies the role of the components?

Solubility of a substance is typically defined as the maximum amount of solute that can be dissolved in:

When salt is dissolved in water, the salt particles occupy:

In a $20\%$ (m/m) solution of common salt in water, what is the ratio of the mass of solute to the mass of solvent?

Which factor primarily determines the physical state (solid, liquid, or gas) of a solution?

Which of the following is NOT a property of a solution?

To prepare a saturated solution of sugar, you should keep adding sugar to water until:

A clear, transparent mixture where the solute does not settle is a:

Solubility of gases in liquids generally ________ with an increase in temperature.

A student is given four beakers, each containing 100g of water at $25^{\circ}C$. The student adds exactly 20g of a different substance (P, Q, R, or S) to each beaker and stirs well. Based on the solubility data provided in the flowchart, which substance forms an unsaturated solution that requires the least amount of additional solute to reach its saturation point?

Which of the following represents the correct sequence in the formation of a saturated solution?

Solubility of a substance 'A' is 20g at $25^{\circ}C$ and 35g at $50^{\circ}C$. If a saturated solution at $50^{\circ}C$ (containing 100g water) is cooled to $25^{\circ}C$, how much 'A' will precipitate?

In a saturated solution of a gas in a liquid, if the temperature is lowered while keeping the pressure constant, what happens?

A solution contains $30\text{ g}$ of Sugar in $170\text{ g}$ of water. What is its concentration?

Calculate the mass of Potassium Sulphate required to prepare its saturated solution in $50\text{ g}$ of water at $40^{\circ}\text{C}$, given its solubility is $15\text{ g}/100\text{ g}$ water at that temperature.

What is the effect of crushing a solid solute before adding it to a liquid?

When a solid dissolves in a liquid, the solid is the ________ phase.

Solubility of a substance is usually given at ________ temperature.

Which temperature would likely have the highest solubility for sugar in water?

What happens to the solubility of most solids in water when the temperature is lowered to $0^\circ C$?

If a solution is transparent and does not settle over time, it is most likely a:

Why is solubility data often plotted on a graph against temperature?

A student dissolves $100\text{ g}$ of a salt in $100\text{ g}$ of water at $100^{\circ}C$. Upon cooling to $20^{\circ}C$, the solubility is $20\text{ g}/100\text{ g}$ water. If $80\text{ g}$ of salt precipitates, what was the initial state at $100^{\circ}C$?

What is the relationship between the 'solubility' of most solid solutes and the 'thermal energy' of the solvent?

Why does a saturated solution of Calcium Hydroxide ($Ca(OH)_2$) become cloudy when heated?

What happens when you pump air into a bicycle tire (relating to gas behavior)?

What is the solvent in the Earth's oceans?

If you increase the temperature of a soda, the $CO_{2}$ gas molecules move:

Which of these is a homogeneous mixture?

An experimenter uses a sealed chamber to study how different conditions affect the amount of oxygen ($O_{2}$) that can dissolve in water. If the experimenter performs the two steps shown in the diagram, what will be the overall result regarding the solubility of the gas?

How does increasing the surface area of a liquid (e.g., by spreading it out) affect the rate at which a dissolved gas escapes?

Why is the solubility of oxygen in blood higher than its solubility in pure water?

What would be the effect of increasing the 'purity' of a solvent (removing all ions and impurities) on the solubility of a non-polar gas?

Which law states that the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases, which is crucial for calculating individual gas solubilities?

During an experiment, a student notices that as she adds sugar to a carbonated drink, it fizzes violently. This is because:

What is the main reason why a person floats more easily in the ocean than in a lake?

Solubility of gases in liquids ________ with an increase in temperature.

If an object has a density of $1 \text{ g/cm}^3$, how will it behave in water?

If you take a saturated solution of salt at $60^{\circ}C$ and cool it to $20^{\circ}C$, what will happen?

A scientist records the maximum amount (in grams) of three different solutes—X, Y, and Z—that can dissolve in $100\ g$ of water at $25^{\circ}C$. The data is shown in the diagram below. If $35\ g$ of each solute is stirred into separate beakers containing $100\ g$ of water at $25^{\circ}C$, which beaker(s) will contain a saturated solution with some solid remaining undissolved?

In a soda water solution, identify the components.

If an object is weighed in air and then weighed while submerged in water, the weight in water will be:

What happens to the density of a solution when more solute is dissolved in a fixed volume of solvent?

If an object is floating in a liquid, the buoyant force acting on it is:

Which of the following has the highest density?

An object has a mass of $10g$ and a volume of $20cm^3$. Will it float or sink in water ($1g/cm^3$)?

When we say a solution is 'unsaturated', it means:

Which of the following is the solvent in the air we breathe?

A stone of mass $30g$ is put into a cylinder containing water. The level rises from $20mL$ to $30mL$. What is the density of the stone?

A specialized cleaning solution has a known density of $1.2\ g/mL$. If a laboratory technician measures out $500\ mL$ of this solution, what is the total mass of the sample?

The diagram below provides the mass and volume of four different liquid samples. Which liquid has the highest density?

A student determines the density of an unknown solid object using the displacement method. Based on the measurements shown in the diagram, if the object has a mass of $120\ g$, what is its density?

If you have 250 g of a 20% salt solution, how much more salt must be added to make it a 25% solution?

Which of the following statements is FALSE about solutions?

A block of material with a density of 0.6 $g/cm^3$ is floating in a liquid with a density of 0.8 $g/cm^3$. What fraction of the block's volume is above the liquid surface?

In the lab, if you want to find the volume of $50 ml$ of water, which tool would you use?

Which of the following will have the highest density?

To find the density of a liquid, we need to know its mass and its:

Solubility of gases in liquids generally ______ with an increase in temperature.

To calculate the density of a liquid, one must first find its mass. This is done by:

Relative density has no units because:

A substance with a density of $2.5\text{ g/cm}^3$ is placed in a liquid with a density of $3.0\text{ g/cm}^3$. The substance will:

A $100\text{ cm}^3$ block of aluminum (density $2.7\text{ g/cm}^3$) is submerged in a sugar solution of density $1.2\text{ g/cm}^3$. What is the buoyant force acting on the block? (Take $g = 9.8\text{ m/s}^2$)

If the density of a solution is higher than the density of the solvent, the solute must be:

When a solute is dissolved in a solvent, the mass of the solution is always equal to the sum of the masses of the solute and solvent. This follows which law?

Which will be more dense: 100ml of water with 10g of salt, or 100ml of water with 20g of salt?

Density is considered a:

If you dissolve sugar in water, the mass of the solution is:

Which of these statements is TRUE about heating a liquid solution?

Which of these factors does NOT directly affect the density of a liquid solution?

If density is $D$, mass is $M$, and volume is $V$, what happens to $D$ if $V$ is halved by cooling (assuming $M$ is constant)?

The rise of warm air and the fall of cool air is an example of a density current. This is most similar to which liquid process?

If you heat a solution and its density remains exactly the same, what must be happening simultaneously?

Which of these experimental errors would most likely lead to an incorrect conclusion about the effect of temperature on density?

Imagine a vertical tube filled with a solution, heated at the top and cooled at the bottom. Will a convection current form?

If the density of an object is less than the density of the liquid it is placed in, it will...

When pressure is applied to a fluid, the change in density is most noticeable in:

A solution is prepared by dissolving $10g$ of salt in $100g$ of water. The mass of the solution is:

In most solids, the effect of pressure on density is:

What is the general conclusion about the effect of pressure on the density of matter?

Using the data from the previous question (mass $10g$, new volume $1L$), what is the new density?

If a gas has a mass of $10g$ and occupies $5L$ at $1\ atm$, and then pressure is increased to $5\ atm$ at constant temperature, what is the new volume?

In a hypothetical world where liquids were as compressible as gases, what would happen to a cup of water if the atmospheric pressure doubled?

A syringe is filled with a solution of sugar and water. The tip is sealed and the plunger is pushed hard. Does the concentration (mass of solute per volume of solution) change?

What is the effect on the density of a solvent if a non-volatile solute is added and then the system is compressed?