⚡ Topic Learning Kit

Chemistry Solutions: Types, Concentration & Colligative Properties

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💡 Key Idea

What Makes a Solution: Solute + Solvent

Two parts, one uniform phase.

↳ A solution is homogeneous at the particle level — solute and solvent cannot be distinguished or filtered apart.

⚖️ Comparison

Types of Solutions by Physical State

Nine combinations, one concept.

↳ Any of the three states can act as solute or solvent — the physical state of the solution is that of the solvent.

➗ Formula

Concentration: Mass %, ppm, Mole Fraction

Four ways to say 'how much'.

↳ Mass % and ppm are mass-based; mole fraction is mole-based and dimensionless.

➗ Formula

Molarity vs Molality

M vs m — one letter, big difference.

↳ Use molality for colligative properties because it does not change with temperature.

➗ Formula

Normality and Equivalent Concept

Equivalents, not moles.

↳ Normality depends on the reaction — the same solution can have different N in different reactions.

📖 Definition

Solubility: Saturated, Unsaturated, Supersaturated

How much can dissolve?

↳ Temperature and pressure shift solubility in opposite ways for solids vs gases.

➗ Formula

Henry's Law: Gas Solubility vs Pressure

More pressure, more fizz.

↳ Higher pressure above a liquid → more gas dissolves; lower pressure → gas escapes.

➗ Formula

Raoult's Law for Ideal Solutions

Vapour pressure follows mole fraction.

↳ Raoult's law is the foundation for all colligative property calculations.

⚖️ Comparison

Ideal vs Non-Ideal Solutions

Positive or negative deviation?

↳ Deviation direction tells you whether A–B forces are weaker or stronger than pure-component forces.

💡 Key Idea

Colligative Properties: Depend on Count, Not Identity

Number of particles rules.

Colligative properties depend only on the number of solute particles, not on their chemical nature.

↳ All four colligative properties scale with the number of dissolved particles.

➗ Formula

Relative Lowering of Vapour Pressure

Solute lowers the vapour pressure.

↳ Relative lowering equals the mole fraction of the solute — a direct link between vapour pressure and composition.

➗ Formula

Boiling Point Elevation & Freezing Point Depression

Two shifts, one constant.

↳ K_b and K_f are solvent-specific constants — molality is the only variable you change.

➗ Formula

Osmotic Pressure and van't Hoff Equation

Pressure that stops osmosis.

↳ Osmotic pressure is the best method for measuring molar mass of macromolecules because it is measurable at low concentrations.

💡 Key Idea

van't Hoff Factor: Counting Ions

One formula unit, many particles.

↳ For electrolytes, multiply the expected colligative effect by i to account for dissociation.

⚠️ Common Mistake

Molarity vs Molality Mix-Up

Don't swap M and m.

↳ Colligative formulas use molality, not molarity — remember the lowercase m.

🌍 Real World

Solutions in Everyday Life

Chemistry you can taste.

↳ Colligative properties are the physics behind antifreeze, saline, soda, and desalination.

🎯 Exam Tip

Exam Tip: Units and Constants

Units win marks.

↳ Matching R to the pressure unit is the most common source of lost marks in solution problems.

Smart notes

What you'll study, topic by topic

Chemistry Solutions: Types, Concentration & Colligative Properties

18 min

A solution is a homogeneous mixture of solute and solvent whose properties depend on composition and concentration. This kit covers types of solutions, ways of expressing concentration, solubility, Raoult's law, and coll…

A solution is a homogeneous mixture of two or more substances.
The solute is the substance that dissolves; the solvent is the substance that does the dissolving.
In a solution, particles are dispersed at the molecular or ionic level (typically

Full explanation, worked examples & memory tricks in the app

Leveled MCQ practice

Try the smart MCQs from this kit

All 18 questions, laddered from warm-up to topper-level, each with its answer and the reasoning behind it.

Warm-up · 6 questions

Q1. Which statement best defines a solution?

Beginner

A A heterogeneous mixture with visible particles

B A homogeneous mixture of two or more substances

C A pure substance with fixed composition

D A suspension that settles on standing

Show the answer

B · A homogeneous mixture of two or more substances

A solution is a homogeneous mixture where solute and solvent are uniformly mixed at the particle level.

Q2. In salt water, which substance is the solvent?

Beginner

A Water

B Neither; it is a suspension

C Salt

D Both salt and water equally

Show the answer

A · Water

Water is the solvent because it does the dissolving and is present in the greater amount.

Q3. A solution is transparent and does not settle on standing because:

Beginner

A The solvent is always water

B Particles are large enough to scatter light

C The solute evaporates quickly

D Particles are at the molecular or ionic level, typically <1 nm

Show the answer

D · Particles are at the molecular or ionic level, typically <1 nm

Solutions have particles smaller than 1 nm, so they do not scatter light significantly or settle.

Q4. Which rule predicts whether a solute will dissolve in a solvent?

Beginner

A Opposites always attract

B Like dissolves like

C All solutes dissolve in all solvents

D Heavier substances dissolve first

Show the answer

B · Like dissolves like

The general rule is 'like dissolves like': polar solvents dissolve polar/ionic solutes, nonpolar dissolve nonpolar.

Q5. Which of the following is a gaseous solution?

Beginner

A Seawater

B Air

C Sugar water

D Brass

Show the answer

B · Air

Air is a solution of gases, mainly nitrogen and oxygen.

Q6. A solution is a homogeneous mixture where solute particles are dispersed at the molecular or ionic level, typically smaller than 1 nanometer.

Beginner

A True

B False

Show the answer

A · True

A solution is a homogeneous mixture where solute particles are dispersed at the molecular or ionic level, typically smaller than 1 nanometer.

Building up · 7 questions

Q7. A solution that contains the maximum amount of solute that can dissolve at a given temperature is called:

Intermediate

A Saturated

B Supersaturated

C Dilute

D Unsaturated

Show the answer

A · Saturated

A saturated solution has dissolved as much solute as possible at that temperature; excess solute will not dissolve.

Q8. What happens to the solubility of most solids when temperature increases?

Intermediate

A It decreases

B It first increases then decreases

C It remains exactly the same

D It increases

Show the answer

D · It increases

For most solids, solubility increases with temperature.

Q9. Why does warm soda go flat faster than cold soda?

Intermediate

A Warm soda has more solute

B Cold soda has higher pressure

C Gas solubility increases as temperature increases

D Gas solubility decreases as temperature increases

Show the answer

D · Gas solubility decreases as temperature increases

The solubility of gases decreases with increasing temperature, so carbon dioxide escapes faster from warm soda.

Q10. Which formula represents molarity (M)?

Intermediate

A $M = \frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$

B $M = \frac{\text{moles of solute}}{\text{kilograms of solvent}}$

C $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

D $M = \frac{\text{mass of solute}}{\text{mass of solution}} \times 100\%$

Show the answer

C · $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

Molarity is defined as moles of solute per liter of solution.

Q11. A solution contains 5 g of NaCl in 100 g of solution. What is the mass percent of NaCl?

Intermediate

A 5%

B 50%

C 0.5%

D 10%

Show the answer

A · 5%

Mass percent = (5 g / 100 g) × 100% = 5%.

Q12. Which of the following best explains why oil and water do not mix?

Intermediate

A Oil is denser than water and sinks

B Oil dissolves only in acidic solutions

C Oil is nonpolar and water is polar, so they cannot form favorable interactions

D Water molecules are too large to surround oil molecules

Show the answer

C · Oil is nonpolar and water is polar, so they cannot form favorable interactions

Oil is nonpolar and water is polar; the mismatch means oil molecules cluster together rather than mix with water.

Q13. When sugar dissolves in water, the sugar molecules are:

Intermediate

A Settled at the bottom

B Chemically converted into water

C Surrounded by water molecules through hydrogen bonding

D Melted into liquid sugar

Show the answer

C · Surrounded by water molecules through hydrogen bonding

Molecular solutes like sugar separate and become surrounded by water molecules via hydrogen bonding; dissolving is not melting.

Topper level · 5 questions

Q14. A solution that contains more dissolved solute than normally possible at a given temperature is:

Advanced

A Supersaturated and unstable

B Concentrated but saturated

C Unsaturated and dilute

D Saturated and stable

Show the answer

A · Supersaturated and unstable

A supersaturated solution contains excess solute and is unstable; it can crystallize suddenly if disturbed.

Q15. In a mixture of 10 mL ethanol and 90 mL water, which is the solvent and why?

Advanced

A Water, because it is present in the greater amount

B Ethanol, because it is less polar

C Ethanol, because it dissolves first

D Neither; they form a suspension

Show the answer

A · Water, because it is present in the greater amount

The solvent is usually the component present in the greater amount; here water is 90 mL vs ethanol 10 mL.

Q16. Which statement correctly distinguishes dissolving from melting?

Advanced

A Melting involves a solvent; dissolving does not

B Dissolving is dispersal of solute particles in a solvent; melting is a change of state due to heat

C Dissolving and melting are the same process

D Dissolving changes the chemical identity of the solute

Show the answer

B · Dissolving is dispersal of solute particles in a solvent; melting is a change of state due to heat

Dissolving disperses solute particles into a solvent without changing state; melting is a solid-to-liquid phase change caused by heat.

Q17. A chemist prepares a solution by dissolving 10 g of KCl in enough water to make 500 mL of solution. What is the molarity of the KCl solution? (Molar mass of KCl = 74.55 g/mol)

Advanced

A 1.35 M

B 0.67 M

C 0.27 M

D 1.00 M

Show the answer

B · 0.67 M

To find the molarity (M), use the formula: $$M = \frac{\text{moles of solute}}{\text{liters of solution}}$$. First, calculate moles of KCl: $$\text{moles} = \frac{10 \text{ g}}{74.55 \text{ g/mol}} \approx 0.134 \text{ mol}$$. Convert 500 mL to liters:…

Q18. A solution is prepared by dissolving 20 g of sugar (C₁₂H₂₂O₁₁) in 200 g of water. Calculate the mass percent of sugar in the solution. (Assume the density of the solution is approximately equal to that of water.)

Advanced

A 30%

B 20%

C 25%

D 10%

Show the answer

B · 20%

To find the mass percent, use the formula: $$\text{mass percent} = \left( \frac{\text{mass of solute}}{\text{mass of solution}} \right) \times 100\%$$. The mass of the solution is $$20 \text{ g (sugar)} + 200 \text{ g (water)} = 220 \text{ g}$$. Thus,…

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