---
title: "Pure Substances and Mixtures"
book: "School Chemistry — Grades 1 to 12"
subject: chemistry
language: en
chapter: 8
exercises: 12
source: https://one-course.com/books/chemistry/1/en/chapter/8-pure-substances-and-mixtures
license: CC-BY-NC-SA-4.0
credit: "One Chemistry Book, One Course (one-course.com)"
---

# Chapter 8 — Pure Substances and Mixtures

A bottle of mineral water lists on its label a dozen dissolved substances, with their amounts in milligrams per litre. The water that comes out of a laboratory’s purifier lists none. Both are clear and colourless, both quench thirst — yet only one of them is what a chemist calls pure. This chapter gives the word “pure” its exact meaning, and shows how to tell a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) from a [mixture](#def-g6-pure-substances-and-mixtures-mixture) without tasting anything.

**You already know.**

To [mix](https://one-course.com/books/chemistry/1/en/chapter/2-mixing-and-dissolving#def-g2-mixing-and-dissolving-mix) is to put different things together; a solid that [dissolves](https://one-course.com/books/chemistry/1/en/chapter/2-mixing-and-dissolving#def-g2-mixing-and-dissolving-dissolve) in water leaves the liquid clear, and the clear liquid is a solution ([Chapter 2](https://one-course.com/books/chemistry/1/en/chapter/2-mixing-and-dissolving#ch-g2-mixing-and-dissolving)). [Mixes](https://one-course.com/books/chemistry/1/en/chapter/2-mixing-and-dissolving#def-g2-mixing-and-dissolving-mix) can be taken apart by [sieving](https://one-course.com/books/chemistry/1/en/chapter/3-separating-mixtures#def-g3-separating-mixtures-sieve), [decanting](https://one-course.com/books/chemistry/1/en/chapter/3-separating-mixtures#def-g3-separating-mixtures-decant), [filtering](https://one-course.com/books/chemistry/1/en/chapter/3-separating-mixtures#def-g3-separating-mixtures-filter) and [evaporating](https://one-course.com/books/chemistry/1/en/chapter/3-separating-mixtures#def-g3-separating-mixtures-evaporate) ([Chapter 3](https://one-course.com/books/chemistry/1/en/chapter/3-separating-mixtures#ch-g3-separating-mixtures)). Every material has properties that can be tested: hard or soft, transparent or not, floats or sinks ([Chapter 1](https://one-course.com/books/chemistry/1/en/chapter/1-what-things-are-made-of#ch-g1-materials-around-us)).

## 8.1 Chemical species and pure substances

**Definition 8.1 (Chemical species).**

A *chemical species* is one particular kind of substance, with its own name and its own properties: water, sugar, salt, oxygen, ethanol (the alcohol of wine), iron.

**Definition 8.2 (Pure substance).**

A *pure substance* is made of one single [chemical species](#def-g6-pure-substances-and-mixtures-species) and nothing else: distilled water, a crystal of sugar, a gold ring of pure gold.

**Definition 8.3 (Mixture).**

A *mixture* contains several [chemical species](#def-g6-pure-substances-and-mixtures-species). [Air](https://one-course.com/books/chemistry/1/en/chapter/4-air-a-mixture-of-gases#def-g4-air-a-mixture-of-gases-air), sea water, mineral water, milk, granite and orange juice are mixtures.

**Remark 8.4 (Pure in everyday language).**

A carton of “pure orange juice” means that nothing has been added to the juice. To a chemist the juice is still a [mixture](#def-g6-pure-substances-and-mixtures-mixture): water, sugars, acids, vitamins, colours and flavours, many [chemical species](#def-g6-pure-substances-and-mixtures-species). “Pure mountain water” is a [mixture](#def-g6-pure-substances-and-mixtures-mixture) too: water with dissolved salts.

![Sorting matter. The bottom boxes give examples of each kind.](https://one-course.com/images/onecourse/chapters/chemistry-1/g6-pure-substances-and-mixtures/fig-616d6b574cfb.svg)

*Sorting matter. The bottom boxes give examples of each kind.*

## 8.2 Homogeneous and heterogeneous mixtures

**Definition 8.5 (Homogeneous and heterogeneous mixtures).**

A [mixture](#def-g6-pure-substances-and-mixtures-mixture) is a *homogeneous mixture* when its different parts cannot be told apart by eye, even with a magnifying glass: it looks the same everywhere. It is a *heterogeneous mixture* when at least two different parts can be seen.

**Example 8.6 (Four mixtures).**

Salty water and [air](https://one-course.com/books/chemistry/1/en/chapter/4-air-a-mixture-of-gases#def-g4-air-a-mixture-of-gases-air) are homogeneous: their parts cannot be seen. Oil on water is heterogeneous: two layers. Muddy water is heterogeneous: grains float in it and settle. Orange juice with pulp is heterogeneous: the bits of pulp can be seen.

![One homogeneous and three heterogeneous mixtures.](https://one-course.com/images/onecourse/chapters/chemistry-1/g6-pure-substances-and-mixtures/fig-ecf70e28af36.svg)

*One homogeneous and three [heterogeneous mixtures](#def-g6-pure-substances-and-mixtures-homogeneous).*

![](https://one-course.com/images/onecourse/chapters/chemistry-1/g6-pure-substances-and-mixtures/img-011e5b442ea8.jpg)

![](https://one-course.com/images/onecourse/chapters/chemistry-1/g6-pure-substances-and-mixtures/img-469e92876ef5.jpg)

*Granite: grains of three or four different minerals can be seen. A heterogeneous solid. Photo: Eurico Zimbres, CC BY-SA 2.0 br.*

*Orange juice with pulp: a [heterogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous).*

**Remark 8.7 (Homogeneous does not mean pure).**

Salty water looks exactly like pure water. Looking is not enough to tell a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) from a [homogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous): we must measure something.

## 8.3 Identifying a pure substance by its constants

**Proposition 8.8 (A pure substance has its own constants).**

Each [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) melts at its own fixed temperature, boils at its own fixed temperature (at normal pressure), and has its own mass for a given volume, its density. These numbers are its constants; the physics book explains what they measure. For a few [pure substances](#def-g6-pure-substances-and-mixtures-pure-substance):

| [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) | melts at | boils at | mass of $1\,\mathrm{cm}^{3}$ |
| --- | --- | --- | --- |
| water | $0\,{}^{\circ}\mathrm{C}$ | $100\,{}^{\circ}\mathrm{C}$ | about $1.0\,\mathrm{g}$ |
| ethanol | $-114\,{}^{\circ}\mathrm{C}$ | $78\,{}^{\circ}\mathrm{C}$ | $0.79\,\mathrm{g}$ |
| propanone (acetone) | — | $56\,{}^{\circ}\mathrm{C}$ | $0.78\,\mathrm{g}$ |
| salt (sodium chloride) | $801\,{}^{\circ}\mathrm{C}$ | — | $2.17\,\mathrm{g}$ |
| iron | $1538\,{}^{\circ}\mathrm{C}$ | — | $7.87\,\mathrm{g}$ |

**Proposition 8.9 (A mixture has no fixed boiling temperature).**

A [mixture](#def-g6-pure-substances-and-mixtures-mixture) does not boil at one fixed temperature: salty water starts to boil a little above $100\,{}^{\circ}\mathrm{C}$, and its temperature keeps rising while it boils, as the water leaves and the salt that stays behind gets more concentrated.

**Method 8.10 (Is this liquid pure? Which one is it?).**

1. Heat it, in the laboratory, and read its temperature while it boils.
2. If the temperature stays fixed, the liquid is probably a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) : compare that temperature with a table of constants.
3. If the temperature keeps rising, it is a [mixture](#def-g6-pure-substances-and-mixtures-mixture) .
4. Confirm with a second constant, for instance the mass of a known volume.

**In the lab — Boiling salty water.**

The teacher heats pure water and salty water side by side, each with a thermometer in it. The pure water boils at $100\,{}^{\circ}\mathrm{C}$ and stays there as long as it boils. The salty water starts boiling a little above $100\,{}^{\circ}\mathrm{C}$, and the thermometer creeps upwards minute after minute.

## 8.4 Water, pure and not

**Example 8.11 (Four waters).**

- **Distilled water** , made in a laboratory, is very nearly a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) : water and nothing else.
- **Tap water** is a [homogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous) : water with small amounts of dissolved substances (a drop dried on a dark plate leaves a white ring).
- **Mineral water** is a [homogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous) whose label gives the dissolved substances, in milligrams per litre.
- **Sea water** is a [homogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous) holding about $35\,\mathrm{g}$ of salts in each kilogram.

![A bottle of mineral water: clear and colourless, and still a mixture.](https://one-course.com/images/onecourse/chapters/chemistry-1/g6-pure-substances-and-mixtures/img-5834939be922.jpg)

*A bottle of mineral water: clear and colourless, and still a [mixture](#def-g6-pure-substances-and-mixtures-mixture).*

**Example 8.12 (Reading a mineral-water label).**

A label reads: calcium $78\,\mathrm{mg}/\mathrm{L}$, magnesium $24\,\mathrm{mg}/\mathrm{L}$, sodium $5\,\mathrm{mg}/\mathrm{L}$, hydrogencarbonate $357\,\mathrm{mg}/\mathrm{L}$, sulfate $10\,\mathrm{mg}/\mathrm{L}$, chloride $4\,\mathrm{mg}/\mathrm{L}$. (These figures are an example.) In one litre there are $78 + 24 + 5 + 357 + 10 + 4 = 478$ mg of dissolved substances, about half a gram: tiny beside the $1000\,\mathrm{g}$ of water, but enough to make it a [mixture](#def-g6-pure-substances-and-mixtures-mixture).

## 8.5 Exercises

**Exercise 8.1 ★.**

[Pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) or [mixture](#def-g6-pure-substances-and-mixtures-mixture)? Distilled water, [air](https://one-course.com/books/chemistry/1/en/chapter/4-air-a-mixture-of-gases#def-g4-air-a-mixture-of-gases-air), sea water, a block of pure iron, milk, a sugar crystal.

**Solution of Exercise 8.1.**

[Pure substances](#def-g6-pure-substances-and-mixtures-pure-substance): distilled water, the block of pure iron, the sugar crystal. [Mixtures](#def-g6-pure-substances-and-mixtures-mixture): [air](https://one-course.com/books/chemistry/1/en/chapter/4-air-a-mixture-of-gases#def-g4-air-a-mixture-of-gases-air), sea water, milk.

**Exercise 8.2 ★.**

Homogeneous or heterogeneous? Salty water, granite, oil on water, tap water, muesli.

**Solution of Exercise 8.2.**

Homogeneous: salty water, tap water. Heterogeneous: granite, oil on water, muesli.

**Exercise 8.3 ★.**

What is a [chemical species](#def-g6-pure-substances-and-mixtures-species)? Give three examples.

**Solution of Exercise 8.3.**

One particular kind of substance, with its own name and properties: for instance water, salt, ethanol (also sugar, oxygen, iron).

**Exercise 8.4 ★.**

A liquid boils at $78\,{}^{\circ}\mathrm{C}$, and its temperature stays at $78\,{}^{\circ}\mathrm{C}$ while it boils. Use the table of constants to suggest what it is.

**Solution of Exercise 8.4.**

A fixed boiling temperature suggests a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance); $78\,{}^{\circ}\mathrm{C}$ is the boiling temperature of ethanol.

**Exercise 8.5 ★.**

Why is “pure orange juice” not a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) for a chemist?

**Solution of Exercise 8.5.**

It contains many [chemical species](#def-g6-pure-substances-and-mixtures-species) (water, sugars, acids, vitamins, flavours): it is a [mixture](#def-g6-pure-substances-and-mixtures-mixture). “Pure” on the carton only means that nothing was added.

**Exercise 8.6 ★★.**

A liquid starts to boil at $100.5\,{}^{\circ}\mathrm{C}$ and its temperature rises while it boils. Is it a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance)? What could it be?

**Solution of Exercise 8.6.**

No: a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) boils at a fixed temperature. It is a [mixture](#def-g6-pure-substances-and-mixtures-mixture), probably water with something dissolved in it, such as salty water.

**Exercise 8.7 ★★.**

Look at the figure of the four beakers. In which beaker could a filter separate the parts of the [mixture](#def-g6-pure-substances-and-mixtures-mixture)? In which beaker could it not?

**Solution of Exercise 8.7.**

A filter could separate the muddy water (the grains stay on the paper) and the juice with pulp (the pulp stays). It cannot separate salty water (the salt is dissolved) nor oil from water (both liquids pass through; they are separated by pouring off the top layer).

**Exercise 8.8 ★★.**

A metal cube of volume $10\,\mathrm{cm}^{3}$ has a mass of $78.7\,\mathrm{g}$. What is the mass of $1\,\mathrm{cm}^{3}$? Which metal of the table could it be?

**Solution of Exercise 8.8.**

$78.7 \div 10 = 7.87\,\mathrm{g}$ for $1\,\mathrm{cm}^{3}$: iron.

**Exercise 8.9 ★★.**

Using the mineral-water label of the example, what percentage of the dissolved mass is hydrogencarbonate? Round to the nearest whole number.

**Solution of Exercise 8.9.**

$\frac{357}{478} \approx 0.747$: about $75\,\%$.

**Exercise 8.10 ★★.**

Sea water holds about $35\,\mathrm{g}$ of salts per kilogram. What mass of salts is there in a $2\,\mathrm{kg}$ bucket of sea water? What percentage of the mass of sea water is salt?

**Solution of Exercise 8.10.**

$2 \times 35 = 70\,\mathrm{g}$ of salts. Percentage: $\frac{35}{1000} =
3.5\,\%$.

**Exercise 8.11 ★★★.**

Two clear, colourless liquids look identical. Describe two measurements, made in a laboratory, that would show whether they are the same [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance).

**Solution of Exercise 8.11.**

Measure their boiling temperatures (each must stay fixed while boiling, and the two must be equal), and weigh the same volume of each (equal masses). Two equal constants, both fixed, point to the same [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance).

**Exercise 8.12 ★★★.**

A [mixture](#def-g6-pure-substances-and-mixtures-mixture) is made of $90\,\mathrm{g}$ of water and $10\,\mathrm{g}$ of ethanol. What percentage of its mass is ethanol? Can it be identified with the table of constants? Explain.

**Solution of Exercise 8.12.**

$\frac{10}{90 + 10} = 10\,\%$ ethanol. It is a [mixture](#def-g6-pure-substances-and-mixtures-mixture): it has no fixed boiling temperature and appears nowhere in the table, which lists only [pure substances](#def-g6-pure-substances-and-mixtures-pure-substance).

## 8.6 Problem: Three Colourless Liquids

**Problem 8.1.**

Weekend problem — three unlabelled flasks of clear, colourless liquid, and the measurements that tell them apart

A laboratory assistant finds three flasks, A, B and C, whose labels have fallen off. All three hold a clear, colourless liquid. The laboratory uses only three such liquids: distilled water, ethanol and sea water brought back from a field trip. The assistant makes three kinds of measurements, in the laboratory.

**Part I — Looking.**

1. The three liquids look exactly alike. Can the assistant tell, by looking, which ones are [pure substances](#def-g6-pure-substances-and-mixtures-pure-substance) ? Explain.
2. If one of them is a [mixture](#def-g6-pure-substances-and-mixtures-mixture) , is it homogeneous or heterogeneous?
3. Which kind of measurement can show that a liquid is a [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) ?

**Part II — Measuring.** Each liquid is heated until it boils. Liquid A boils at $100\,{}^{\circ}\mathrm{C}$ and its temperature stays there. Liquid B boils at $78\,{}^{\circ}\mathrm{C}$ and stays there. Liquid C starts to boil at $100.6\,{}^{\circ}\mathrm{C}$, and its temperature keeps rising slowly. Then $50.0\,\mathrm{mL}$ of each liquid is weighed: A $49.8\,\mathrm{g}$, B $39.5\,\mathrm{g}$, C $51.2\,\mathrm{g}$.

4. Which liquids are [pure substances](#def-g6-pure-substances-and-mixtures-pure-substance) ? Which is a [mixture](#def-g6-pure-substances-and-mixtures-mixture) ?
5. Using the table of constants of this chapter, name liquids A and B.
6. Compute the mass of $1\,\mathrm{mL}$ (that is, $1\,\mathrm{cm}^{3}$ ) of each liquid.
7. Do these masses agree with your answer to question 5?
8. Why does the temperature of liquid C keep rising while it boils?

**Part III — What is in liquid C?** $100\,\mathrm{mL}$ of liquid C are left to dry in a dish. When all the water has gone, $3.5\,\mathrm{g}$ of white crystals remain.

9. What does this residue show about liquid C?
10. Using the mass of $1\,\mathrm{mL}$ of C found in question 6, find the mass of $100\,\mathrm{mL}$ of C, then the percentage of its mass that is salt (to one decimal place).
11. Sea water holds about $35\,\mathrm{g}$ of salts in each kilogram. What percentage is that? Compare with question 10.
12. Conclude: how many grams of salt does each litre of liquid C hold, and is liquid C the sea water?

**Solution of Problem 8.1.**

**1.** No. A [pure substance](#def-g6-pure-substances-and-mixtures-pure-substance) and a [homogeneous mixture](#def-g6-pure-substances-and-mixtures-homogeneous) can look exactly alike: something must be measured.

**2.** Homogeneous: it is clear and its parts cannot be seen.

**3.** A constant: a boiling temperature that stays fixed while the liquid boils (or the mass of a known volume, compared with a table).

**4.** A and B, whose boiling temperatures stay fixed, are [pure substances](#def-g6-pure-substances-and-mixtures-pure-substance). C is a [mixture](#def-g6-pure-substances-and-mixtures-mixture).

**5.** A boils at $100\,{}^{\circ}\mathrm{C}$: water. B boils at $78\,{}^{\circ}\mathrm{C}$: ethanol.

**6.** A: $49.8 \div 50.0 = 0.996\,\mathrm{g}$. B: $39.5 \div 50.0 =
0.790\,\mathrm{g}$. C: $51.2 \div 50.0 = 1.024\,\mathrm{g}$.

**7.** Yes: about $1.0\,\mathrm{g}$ for water, $0.79\,\mathrm{g}$ for ethanol.

**8.** As the water boils away, the salt stays behind, so the liquid that remains holds more and more salt; it then boils at a higher temperature.

**9.** Liquid C holds a dissolved solid: it is a solution, a [mixture](#def-g6-pure-substances-and-mixtures-mixture), as its boiling already showed.

**10.** $100 \times 1.024 = 102.4\,\mathrm{g}$; $\frac{3.5}{102.4}
\approx 0.034$: about $3.4\,\%$ of the mass is salt.

**11.** $\frac{35}{1000} = 3.5\,\%$: very close to question 10.

**12.** $3.5\,\mathrm{g}$ in $100\,\mathrm{mL}$, so $3.5 \times 10 =
35\,\mathrm{g}$ of salt per litre. With its saltiness and its boiling behaviour, C is the sea water; A is distilled water and B ethanol.