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Investigating titrations

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Investigating distillation methods

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Extracting metals and equilibria

The reactivity series of metals

Extracting metals

Biological methods of metal extraction - Higher

Reducing the use of resources

Life cycle assessments

Reversible reactions and equilibria

Position of equilibrium - Higher

Chemical changes

Acids, bases and pH

Strong and weak acids - Higher

Reactions of acids

Electrolysis

States of matter and mixtures

Changes of state

Substance types and determining purity

Filtration and crystallisation

Chromatography: phases and calculations

Potable water, treatment and purification

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Chemical equations

Ionic equations and half equations - Higher

Hazards, risks and precautions

The history of the atom

The atom and isotopes

Calculating relative masses

Calculating relative atomic mass - Higher

The history of the periodic table

Electronic configuration

Ions and their formation

Ionic bonding: properties of compounds and naming

Covalent bonding

Giant covalent substances

Metallic bonding and alloys

Conservation of mass

Molecular and empirical formulae

Mole calculations and Avogadro's constant - Higher

Concentrations of solutions

Limiting reactants and masses - Higher

Practical skills

Measuring techniques

Safety and ethics

Designing experiments

Methods of heating substances

Working with electronics

Random sampling and sampling methods

Comparing results using percentage change

Working scientifically

The scientific method

Science communication and ethics

Evaluating risks and hazards

Collecting data

Processing and presenting data

Units and equations

Structuring a scientific report and drawing conclusions

Uncertainties and evaluations

Explainer Video

Tutor: Alexander

Summary

Investigating titrations

In a nutshell

This practical involves using the required apparatus to carry out a titration using accurate measurements and the correct technique. Using the results of a titration you can calculate the concentration of the unknown solution.

Equations

This equation forms the basis of this experiment:

word equation	Symbol equation
$hydrochloric\ acid\ +\ sodium\ hydroxide\ \rightarrow\ sodium\ chloride\ +\ water$	$HCl(aq)\ +\ NaOH(aq)\ \rightarrow\ NaCl(aq)\ +\ H_2O(l)$

These equations will be used as part of this experiment:

$Titre\ (cm^3)\ = \ end\ volume\ (cm^3)\ -\ start\ volume\ (cm^3)$

$\dfrac{titre\ 1\ +\ titre\ 2}{number\ of\ titres}\ =\ average\ titre$

Equipment list

The following equipment list is used to carry out a titration.

Equipment	Use
Burette	Used to dispense acid into the conical flask
Funnel	Placed in the burette to help pour the acid into the burette
Pipette	Measures a specific volume of alkali $(25\,cm^3)$ to be dispensed into a conical flask
Pipette filler	Used to fill the pipette
Conical flask	Where the titration occurs
Boss	Used to support the burette
Clamp	Used to support the burette
Stand	Used to support the burette
White tile	Placed under a conical flask to help observe a colour change from the indicator
Goggles	Protect eyes from safety hazards
Gloves	Protect hands / skin from safety hazards
Acid (hydrochloric, sulfuric or nitric), unknown concentration	Dispensed into alkali to calculate the concentration of acid
Sodium hydroxide, known concentration	Used to neutralise the acid
Indicator (methyl orange, phenolphthalein)	Gives a visual response of when the pH of a solution changes

Experiment: Determination of reacting volumes using a strong alkali and a strong acid via a titration

Experimental variables

The independent variable is the one you change. The dependent variable is the one which depends on what has been changed, therefore it is the one you measure. The control variable is the one which is kept constant.

Independent variable	$Volume\ of\ acid$
Dependent variable	$pH$
Control variable	$Volume\ of\ alkali$

Safety precautions

When performing experiments, it is very important you consider safety precautions. This is so you and others do not get hurt.

Hazard	Risk	Safety measure
Sodium hydroxide solution	Skin and eye irritation	Wear gloves and eye protection
Acid solution (hydrochloric, sulfuric, nitric)	Skin and eye irritation	Wear gloves and eye protection, fill burette slowly using a funnel

Method

Follow the steps below for the practical.

Chemistry; Chemistry practicals; KS4 Year 10; Investigating titrations

1.	Burette filled with acid (hydrochloric acid)
2.	Boss, clamp and stand
3.	Conical flask containing solution

1.	Use the pipette and pipette filler to add $25 \, cm^3$ of the alkali into a clean conical flask.
2.	Add a few drops of the selected indicator to the flask and place the flask on a white tile.
3.	Fill the burette with acid using a funnel. Make sure to remove the funnel to not skew the readings and note the starting volume.
4.	Add the acid slowly from the burette to the alkali in the conical flask. Make sure to swirl the solution before adding further acid and check for a colour change.
5.	Stop adding the acid when the end-point is reached (when the indicator gives a positive result). Note down the final volume reading of the burette. To ensure that more accurate results are obtained add in the acid drop wise near the end-point.
6.	Repeat steps 1 to 5 until you get concordant titres (see analysis for concordant titre definition).

Analysis

Record the results in a table as shown:

Repeat	Start volume $(cm^3)$	End volume $(cm^3)$	Titre $(cm^3)$
Rough	$12.80$	$0.00$	$12.80$
$1$	$20.05$	$7.60$	$12.45\ \checkmark$
$2$	$22.70$	$10.05$	$12.65$
$3$	$22.25$	$9.75$	$12.50\ \checkmark$

To calculate the titre use the following equation:

$Titre\ (cm^3)\ =\ end\ volume\ (cm^3)\ -\ start\ volume\ (cm^3)$

$\frac{titre\ 1\ + \ titre\ 2}{number\ of\ titres}\ =\ mean\ titre\ (cm^3)$

$mean\ titre\ = \frac{12.45\ +\ 12.50}{2}\ =\ 12.475 \, cm^3$

Readings should be to two decimal points, ending in zero or five (where liquid level is between graduations on the burette).

Make sure to mark your concordant results. Concordant titres are within $0.20 \, cm^3$ or less of each other. Calculate the mean titre by summing the titres and then dividing by the total number of titres.

Conclusion

Using the obtained measurements from the experiment you could calculate the concentration in $(mol/dm^3)$ of the acid.

Evaluation

What actions were taken to ensure accurate measurements? What improvements could be made to the method? Was the practical carried out safely?

Learn with Basics

Length:

Unit 1

Physical and chemical properties

Unit 2

The pH scale and indicators

Jump Ahead

Optional

Unit 3

Investigating titrations

Final Test

Create an account to complete the exercises

FAQs - Frequently Asked Questions

Why should I remove the funnel from the burette?

You should remove the funnel to ensure that no residue drops into the burette. This would change the volume present in the burette and skew the results.

When do I stop a titration?

You stop the titration practical after you have concordant titres. Titres which are within 0.20 cm^3 of each other.

What is the purpose of a titration?

The purpose of a titration is to find out the concentration of an acid or alkali.

Home

Chemistry

Chemistry practicals

Investigating titrations

Videos

Summary

Exercises

Select Lesson

Exam Board

Select an option

Chemistry practicals

Investigating distillation methods

Investigating the composition of inks

Investigating acids and alkalis

Preparing soluble and insoluble salts

Investigating electrolysis

Investigating rates of reaction

Fuels and Earth science

Hydrocarbons and crude oil

Combustion and pollution

Cracking

Evolution of the Earth's atmosphere

Greenhouse gases and climate change

Rates of reaction and energy changes

Calculating rates of reactions

Catalysts

Endothermic and exothermic reactions

Energy changes in reactions

Bond energy calculations - Higher

Groups in the periodic table

Group 1: properties and reactivity

Group 7: properties and reactions

Group 0: properties and reactivity

Extracting metals and equilibria

The reactivity series of metals

Extracting metals

Biological methods of metal extraction - Higher

Reducing the use of resources

Life cycle assessments

Reversible reactions and equilibria

Position of equilibrium - Higher

Chemical changes

Acids, bases and pH

Strong and weak acids - Higher

Reactions of acids

Electrolysis

States of matter and mixtures

Changes of state

Substance types and determining purity

Filtration and crystallisation

Chromatography: phases and calculations

Potable water, treatment and purification

Key concepts

Chemical equations

Ionic equations and half equations - Higher

Hazards, risks and precautions

The history of the atom

The atom and isotopes

Calculating relative masses

Calculating relative atomic mass - Higher

The history of the periodic table

Electronic configuration

Ions and their formation

Ionic bonding: properties of compounds and naming

Covalent bonding

Giant covalent substances

Metallic bonding and alloys

Conservation of mass

Molecular and empirical formulae

Mole calculations and Avogadro's constant - Higher

Concentrations of solutions

Limiting reactants and masses - Higher

Practical skills

Measuring techniques

Safety and ethics

Designing experiments

Methods of heating substances

Working with electronics

Random sampling and sampling methods

Comparing results using percentage change

Working scientifically

The scientific method

Science communication and ethics

Evaluating risks and hazards

Collecting data

Processing and presenting data

Units and equations

Structuring a scientific report and drawing conclusions

Uncertainties and evaluations

Explainer Video

Tutor: Alexander

Summary

Investigating titrations

In a nutshell

Equations

This equation forms the basis of this experiment:

word equation	Symbol equation
$hydrochloric\ acid\ +\ sodium\ hydroxide\ \rightarrow\ sodium\ chloride\ +\ water$	$HCl(aq)\ +\ NaOH(aq)\ \rightarrow\ NaCl(aq)\ +\ H_2O(l)$

These equations will be used as part of this experiment:

$Titre\ (cm^3)\ = \ end\ volume\ (cm^3)\ -\ start\ volume\ (cm^3)$

$\dfrac{titre\ 1\ +\ titre\ 2}{number\ of\ titres}\ =\ average\ titre$

Equipment list

The following equipment list is used to carry out a titration.

Equipment	Use
Burette	Used to dispense acid into the conical flask
Funnel	Placed in the burette to help pour the acid into the burette
Pipette	Measures a specific volume of alkali $(25\,cm^3)$ to be dispensed into a conical flask
Pipette filler	Used to fill the pipette
Conical flask	Where the titration occurs
Boss	Used to support the burette
Clamp	Used to support the burette
Stand	Used to support the burette
White tile	Placed under a conical flask to help observe a colour change from the indicator
Goggles	Protect eyes from safety hazards
Gloves	Protect hands / skin from safety hazards
Acid (hydrochloric, sulfuric or nitric), unknown concentration	Dispensed into alkali to calculate the concentration of acid
Sodium hydroxide, known concentration	Used to neutralise the acid
Indicator (methyl orange, phenolphthalein)	Gives a visual response of when the pH of a solution changes

Experiment: Determination of reacting volumes using a strong alkali and a strong acid via a titration

Experimental variables

Independent variable	$Volume\ of\ acid$
Dependent variable	$pH$
Control variable	$Volume\ of\ alkali$

Safety precautions

When performing experiments, it is very important you consider safety precautions. This is so you and others do not get hurt.

Hazard	Risk	Safety measure
Sodium hydroxide solution	Skin and eye irritation	Wear gloves and eye protection
Acid solution (hydrochloric, sulfuric, nitric)	Skin and eye irritation	Wear gloves and eye protection, fill burette slowly using a funnel

Method

Follow the steps below for the practical.

1.	Burette filled with acid (hydrochloric acid)
2.	Boss, clamp and stand
3.	Conical flask containing solution

1.	Use the pipette and pipette filler to add $25 \, cm^3$ of the alkali into a clean conical flask.
2.	Add a few drops of the selected indicator to the flask and place the flask on a white tile.
3.	Fill the burette with acid using a funnel. Make sure to remove the funnel to not skew the readings and note the starting volume.
4.	Add the acid slowly from the burette to the alkali in the conical flask. Make sure to swirl the solution before adding further acid and check for a colour change.
5.	Stop adding the acid when the end-point is reached (when the indicator gives a positive result). Note down the final volume reading of the burette. To ensure that more accurate results are obtained add in the acid drop wise near the end-point.
6.	Repeat steps 1 to 5 until you get concordant titres (see analysis for concordant titre definition).

Analysis

Record the results in a table as shown:

Repeat	Start volume $(cm^3)$	End volume $(cm^3)$	Titre $(cm^3)$
Rough	$12.80$	$0.00$	$12.80$
$1$	$20.05$	$7.60$	$12.45\ \checkmark$
$2$	$22.70$	$10.05$	$12.65$
$3$	$22.25$	$9.75$	$12.50\ \checkmark$

To calculate the titre use the following equation:

$Titre\ (cm^3)\ =\ end\ volume\ (cm^3)\ -\ start\ volume\ (cm^3)$

$\frac{titre\ 1\ + \ titre\ 2}{number\ of\ titres}\ =\ mean\ titre\ (cm^3)$

$mean\ titre\ = \frac{12.45\ +\ 12.50}{2}\ =\ 12.475 \, cm^3$

Readings should be to two decimal points, ending in zero or five (where liquid level is between graduations on the burette).

Conclusion

Using the obtained measurements from the experiment you could calculate the concentration in $(mol/dm^3)$ of the acid.

Evaluation

What actions were taken to ensure accurate measurements? What improvements could be made to the method? Was the practical carried out safely?

Learn with Basics

Length:

Unit 1

Physical and chemical properties

Unit 2

The pH scale and indicators

Jump Ahead

Optional

Unit 3

Investigating titrations

Final Test

Create an account to complete the exercises

FAQs - Frequently Asked Questions

Why should I remove the funnel from the burette?

You should remove the funnel to ensure that no residue drops into the burette. This would change the volume present in the burette and skew the results.

When do I stop a titration?

You stop the titration practical after you have concordant titres. Titres which are within 0.20 cm^3 of each other.

What is the purpose of a titration?

The purpose of a titration is to find out the concentration of an acid or alkali.

Investigating titrations

Videos

Summary

Exercises

Select Lesson

Exam Board

Chemistry practicals

Fuels and Earth science

Rates of reaction and energy changes

Groups in the periodic table

Extracting metals and equilibria

Chemical changes

States of matter and mixtures

Key concepts

Practical skills

Working scientifically

Explainer Video

Summary

Investigating titrations

​​In a nutshell​​

Equations

​​word equation

Symbol equation

Equipment list

Equipment

Use

Experiment: Determination of reacting volumes using a strong alkali and a strong acid via a titration

Experimental variables

Safety precautions

Hazard

Risk

Safety measure

Method

Analysis

Repeat

Start volume (cm3)(cm^3)(cm3)​​

End volume (cm3)(cm^3)(cm3)​​

Titre (cm3)(cm^3)(cm3)​​

Conclusion

Evaluation

Learn with Basics

Unit 1

Physical and chemical properties

Unit 2

The pH scale and indicators

Jump Ahead

Unit 3

Investigating titrations

Final Test

FAQs - Frequently Asked Questions

Why should I remove the funnel from the burette?

When do I stop a titration?

What is the purpose of a titration?

Investigating titrations

Videos

Summary

Exercises

Select Lesson

Exam Board

Chemistry practicals

Fuels and Earth science

Rates of reaction and energy changes

Groups in the periodic table

Extracting metals and equilibria

Chemical changes

States of matter and mixtures

Key concepts

Practical skills

Working scientifically

Explainer Video

Summary

Investigating titrations

​​In a nutshell​​

Equations

​​word equation

Symbol equation

Equipment list

Equipment

Use

Experiment: Determination of reacting volumes using a strong alkali and a strong acid via a titration

In a nutshell

word equation

Start volume $(cm^3)$

End volume $(cm^3)$

Titre $(cm^3)$

In a nutshell

word equation

Start volume $(cm^3)$

End volume $(cm^3)$

Titre $(cm^3)$