sodium carbonate and hydrochloric acid experiment

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Titration of Sodium Carbonate With Hydrochloric Acid

How to Reduce Potassium Permanganate

You can use the technique of titration to determine the concentration of a sodium carbonate solution using a solution with a known concentration of hydrochloric acid, or vice versa. HCl gradually reduces the alkalinity of the solution until the pH is 7. Because the reaction between sodium carbonate and hydrochloric acid proceeds in two stages, you can use more than one indicator. Phenolphthalein is suitable for the first stage, and methyl orange is best for the second.

TL;DR (Too Long; Didn't Read)

Use phenolphthalein for the first titration of sodium carbonate with hydrochloric acid, then check your results by doing a second titration with methyl orange.

A Two-Stage Reaction

When you add a hydrochloric acid (HCl) solution to a solution of sodium carbonate (Na 2 CO 3 ), the hydrogen ion in HCl switches places with one of the sodium ions in Na 2 CO 3 to produce sodium hydrogencarbonate, also known as sodium bicarbonate (baking soda), and sodium chloride (salt).

Na 2 CO 3 (aq) + HCl(aq) → NaHCO 3 (aq) + NaCl(aq)

Sodium hydrogencarbonate is basic, and it reacts with the HCl still in solution to produce sodium chloride, carbon dioxide and water.

NaHCO 3 (aq) + HCl(aq) → NaCl(aq) + CO 2 (g) + H 2 O(l)

Phenolphthalein is a good indicator for the first reaction because it responds to the pH change caused by the formation of sodium hydrogencarbonate. It is pink in basic solutions and turns colorless as soon as the solution becomes acidic. Methyl orange, on the other hand, responds to pH changes associated with the formation of NaCl, changing from yellow to red as the solution becomes more acidic. At neutrality, it is a distinct orange color.

Basic Procedure

Titrations generally call for accurately graduated beakers and pipettes for transferring solution from one beaker to another. Wear goggles and gloves for protection from corrosive chemicals.

Measure out a suitable amount of a sodium carbonate solution of unknown concentration and a hydrochloric acid solution of known concentration in separate graduated beakers.

Put a few drops of phenolphthalein in the sodium carbonate solution. The indicator will turn pink.

Carefully add HCl to sodium carbonate solution until the solution becomes colorless. Record the volume of HCl solution you added.

Calculate the number of moles of HCl in the original solution and derive from this the number of moles of Na 2 CO 3 in the target solution, keeping in mind that 1 mole of HCl reacts with 1 mole of Na 2 CO 3 . Determine the concentration of the Na 2 CO 3 solution using a volumetric analysis.

In this part of the titration, HCl is reacting with NaHCO 3 , but the proportion is still one mole to one mole. After molarity calculations and a volumetric analysis, the results should be identical to those using phenolphthalein.

Related Articles

Purpose of titration, common acid base indicators, how to make a bromothymol blue solution, why does phenolphthalein change color, how to test for sodium bicarbonate, how to test for calcium hydroxide, methods on how to determine ph in ph paper, methods for testing ph of liquids, how to find an equivalence point titration, how to calculate the k value on a titration graph, how to standardize a ph meter, how-to science experiments for kids with iodine and..., how to turn a glass of water with red dye back into..., how to dissolve calcium oxalate, sulfuric acid & chlorine bleach reaction, how to determine if salts are acidic or basic, how to do titration calculations, potassium permanganate experiments.

• Purdue University: What Is Titration?

About the Author

Chris Deziel holds a Bachelor's degree in physics and a Master's degree in Humanities, He has taught science, math and English at the university level, both in his native Canada and in Japan. He began writing online in 2010, offering information in scientific, cultural and practical topics. His writing covers science, math and home improvement and design, as well as religion and the oriental healing arts.

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Practical videos | 14–16 years

• 1 Access free videos to support your teaching
• 2 Paper chromatography
• 3 Rates of reaction
• 4 Simple distillation
• 5 Enthalpy change of combustion
• 6 Conservation of mass
• 7 Electrolysis of aqueous solutions
• 8 Halogen displacement reactions
• 9 Identifying ions
• 10 Preparing a soluble salt
• 11 Reactivity series of metals
• 12 Simple titration
• 13 Temperature change (neutralisation)
• 14 Potable water

Simple titration

2020-07-07T11:42:00+01:00

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Simple acid-base titration can be used to find out the concentration of a solution

Running a titration experiment

This video by the Royal Society of Chemistry explains the steps involved in running a titration experiment. Fran demonstrates how to rinse and prepare the burette to ensure accurate results. The acid-base titration uses a standard solution of Na 2 CO 3 to find the exact concentration of HCl by identifying the end-point of the neutralisation reaction. The video includes both a rough titration and recording data from a subsequent accurate titration. Calculations of the concentration of HCl are not included, so students could follow up with data analysis to assess their understanding of the content. 

Results analysis

Students can be given typical results such as these (taken from the AQA AS and A Level  Required Practical Handbook ), and asked to manipulate and analyse them. Students do not need to be provided with a complete table as they could be expected to calculate the titre from the final and initial readings. They should also be able to identify concordant results and discard anomalous results before continuing with their analysis.

AQA required practical specification

Mrs Peers-Dent from Malmesbury Education carries out the titration in this video, following the AQA required practical specification. It demonstrates how the titration procedure can be used to find the concentration of H 2 SO 4 using a known concentration of NaOH. Mrs Peers-Dent measures the acid to the nearest 0.1cm 3 , whereas in the Royal Society of Chemistry video above Fran measures to the nearest 0.05cm 3 . The titration screen experiment below also measures to the nearest 0.05cm 3 . You may decide which is the most appropriate based on the ability of the group you are working with or you could use this as an opportunity to discuss key terminology such as precision, accuracy and reliability .

Learners can practise their skills using Royal Society of Chemistry’s  titration screen experiment . We recommend that 14–16 students complete Level 1 of the screen experiment, while older students can progress to Levels 2, 3 and 4. The screen experiments frame the titration procedure with a real-world scenario to foster an interest in chemistry careers and contextualise their learning.

 Also check out

• Online titration quiz  – further videos and access to five online quizzes.
• A microscale acid-based titration  – outline of a class practical to carry out titration on a small scale.
• Measuring the amount of vitamin C in fruit drinks  – another class practical using microscale titration.

Additional information

We have collated these videos of key practical experiments to support remote teaching as part of our response to Covid-19. Teachers requested resources to help them deliver practical content without access to laboratories or equipment. We are developing further resources and welcome feedback to help us produce those you most need. Please email us or use the comment section below.

Access free videos to support your teaching

Paper chromatography

Rates of reaction

Simple distillation

Enthalpy change of combustion

Conservation of mass

Electrolysis of aqueous solutions

Halogen displacement reactions

Identifying ions

Preparing a soluble salt

Reactivity series of metals

Temperature change (neutralisation)

Potable water

• 14-16 years
• 16-18 years

Specification

• AT d: Use laboratory apparatus for a variety of experimental techniques including: titration, using burette and pipette, distillation and heating under reflux, including setting up glassware using retort stand and clamps, qualitative tests for ions and…
• RP 1: Make up a volumetric solution and carry out a simple acid–base titration.
• 4. use laboratory apparatus for a variety of experimental techniques, including:
• titration, using burette and pipette
• di) use of laboratory apparatus for a variety of experimental techniques including: i) titration, using burette and pipette
• 2a Determination of the reacting volumes of solutions of a strong acid and a strong alkali by titration.
• 2b Determination of the concentration of one of the solutions in mol/dm³ and g/dm³ from the reacting volumes and the known concentration of the other solution.
• Students should be able to: describe how to carry out titrations using strong acids and strong alkalis only (sulfuric, hydrochloric and nitric acids only) to find the reacting volumes accurately
• 5.9C Carry out an accurate acid-alkali titration, using burette, pipette and a suitable indicator
• 3.16 Explain why, if soluble salts are prepared from an acid and a soluble reactant: titration must be used; the acid and the soluble reactant are then mixed in the correct proportions; the solution remaining, after reaction, is only salt and water
• 3.18 Describe how to carry out an acid-alkali titration, using burette, pipette and a suitable indicator, to prepare a pure, dry salt
• 6 Titration of a strong acid and strong alkali to find the concentration of the acid using an appropriate pH indicator
• C5.4.7 describe and explain the procedure for a titration to give precise, accurate, valid and repeatable results
• C5.3.6 describe and explain the procedure for a titration to give precise, accurate, valid and repeatable results
• C5.1b describe the technique of titration
• PAG 6 Titration of a strong acid and strong alkali to find the concentration of the acid using an appropriate pH indicator
• Use of appropriate qualitative reagents and techniques to analyse and identify unknown samples or products including gas tests, flame tests, precipitation reactions, and the determination of concentrations of strong acids and strong alkalis
• methyl orange
• Examples of primary standards include: sodium carbonate, Na₂CO₃, oxalic acid, H₂C₂O₄.2H₂O, potassium hydrogen phthalate, KH(C₈H₄O₄), silver nitrate, AgNO₃, potassium iodate, KIO₃, potassium dichromate, K₂Cr₂O₇
• Learners should also be aware that, where practicable, titrations should be repeated until concordant results are obtained.
• volumetric analysis: the volume markings on beakers provide only a rough indication of volume
• measuring cylinders generally provide sufficient accuracy for preparative work, but for analytical work, burettes, pipettes and volumetric flasks are more appropriate
• titration is used to accurately determine the volumes of solution required to reach the end-point of a chemical reaction.
• preparation of a standard solution
• Volumetric analysis involves using a solution of accurately known concentration in a quantitative reaction to determine the concentration of another substance.
• Titration is used to determine, accurately, the volumes of solution required to reach the end-point of a chemical reaction. An indicator is normally used to show when the end-point is reached. Titre volumes within 0.2 cm³ are considered concordant.
• Solutions of accurately known concentration are known as standard solutions.
• Redox titrations are based on redox reactions. In titrations using acidified permanganate, an indicator is not required, as purple permanganate solution turns colourless when reduced.
• Given a balanced equation for the reaction occurring in any titration, the: concentration of one reactant can be calculated given the concentration of the other reactant and the volumes of both solutions
• volume of one reactant can be calculated given the volume of the other reactant and the concentrations of both solutions.
• pipette with safety filler
• Titration is used to determine, accurately, the volumes of solution required to reach the end-point of a chemical reaction.
• An indicator is normally used to show when the end-point is reached.
• Titre volumes within 0.2 cm³ are considered concordant
• For solutions, the mass of solute (grams or g), the number of moles of solute (moles or mol), the volume of solution (litres or l) or the concentration of the solution (moles per litre or mol l⁻¹) can be calculated from data provided
• Titration can be used to produce a soluble salt. Once the volumes of acid and alkali have been noted, the reaction can be repeated without the indicator to produce an uncontaminated salt solution. The solution can then be evaporated to dryness.
• In an acid-base titration, the concentration of the acid or base is determined by accurately measuring the volumes used in the neutralisation reaction. An indicator can be added to show the end-point of the reaction
• Given a balanced equation for the reaction occurring in any titration: the concentration of one reactant can be calculated given the concentration of the other reactant and the volumes of both solutions
• the volume of one reactant can be calculated given the volume of the other reactant and the concentrations of both solutions
• use laboratory apparatus for a variety of experimental techniques including: titration, using burette and pipette
• use acid-base indicators in titrations of weak/strong acids with weak/strong alkalis
• (f) acid-base titrations
• PRACTICAL: Standardisation of an acid solution
• (j) titration as a method to prepare solutions of soluble salts and to determine relative and actual concentrations of solutions of acids/alkalis
• (k) the concentration of a solution in mol dm⁻³
• (l) calculations involving neutralisation reactions in solution, using a balanced chemical equation
• PRACTICAL: Titration of a strong acid against a strong base using an indicator
• 2.6.3 demonstrate knowledge and understanding that the volumes of acid and alkali solutions that react together can be measured by titration using phenolphthalein or methyl orange;
• 2.6.4 carry out acid–base titrations using an indicator and record results to one decimal place, repeating for reliability and calculating the average titre from accurate titrations (details of the practical procedure and apparatus preparation are…
• 2.6.5 collect data from primary and secondary sources for acid–base titration and use this data to calculate the concentrations of solutions in mol/dm³ and g/dm³.
• 2.6.6 calculate concentrations of solutions and solution volumes in an acid–base titration, identify unknown compounds and determine the degree of hydration;
• Prescribed Practical C8: determine the reacting volumes of solutions of acid and alkali by titration and determine the concentration of solutions of acid and alkali by titration;
• Use of: titration apparatus including at least class B bulb pipettes and burettes (volume), burette holder/clamp and white tile;
• carry out experiments with the appropriate manipulation of apparatus, taking accurate measurements and considering health and safety;
• 1.8.10 describe neutralisation as the reaction between the hydrogen ions in an acid and the hydroxide ions in an alkali to produce water and recall the ionic equation as: H⁺(aq) + OH⁻(aq) → H₂O(l)
• 1.8.12 recall that a base is a metal oxide or hydroxide which neutralises an acid to produce a salt and water and that an alkali is a soluble base;
• 1.8.9 describe neutralisation as the reaction between the hydrogen ions in an acid and the hydroxide ions in an alkali to produce water and recall the ionic equation as: H⁺(aq) + OH⁻(aq) → H₂O(l)
• 1.8.11 recall that a base is a metal oxide or hydroxide which neutralises an acid to produce a salt and water and that an alkali is a soluble base;
• 8. Investigate reactions between acids and bases; use indicators and the pH scale
• Apparatus used in volumetric analysis.
• Correct titrimetric procedure.
• Acid-base titrations.
• Solving volumetric problems from first principles, where the formula method is not applicable. (Either method may be used when both methods are applicable.)
• Mandatory experiment 4.2 - Standardisation of a hydrochloric acid solution using a standard solution of sodium carbonate.
• Mandatory eexperiment 4.2A - A hydrochloric acid/sodium hydroxide titration, and the use of this titration in making the sodium salt.

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• Titration Of Hydrochloric Acid Against Standard Sodium Carbonate

Titration of Hydrochloric Acid against Standard Sodium Carbonate

Acid-base titration methods based on the dissolution of a sample in excess of standard acid, followed by back titration with a standard base. The hydrochloric acid solutions were standardized against pure sodium carbonate using bromophenol blue as an indicator.

Table of Contents

Materials required, observations, calculations, results and discussion, precautions.

• Frequently Asked Questions

Determination of strength of a given solution of dilute Hydrochloric acid by titrating it against standard solution of Sodium Carbonate solution (M/10).

Hydrochloric acid solution may be titrated against sodium carbonate solution using methyl orange indicator. When weak base is titrated with a strong acid, solution will be slightly acidic at end point. If a weak acid is titrated with a strong base the solution is slightly basic because the salt formed will be hydrolysed to a certain extent.

The chemical reactions involved in this titration are given below.

Na 2 CO 3 (aq) + 2HCl(aq) → 2NaCl(aq) + CO 2 (g) + H 2 O(l)

CO 3 2- (aq) + 2H + (aq) → CO 2 (g) + H 2 O(l)

In acid base titrations at the end point the amount of the acid becomes chemically equivalent to the amount of base present. In case of a strong acid and a strong base titration at the end point of solution the solution becomes neutral.

• Conical flask
• Burette stand
• White glazed tile
• Measuring flask
• Hydrochloric acid
• Sodium carbonate
• Methyl orange
• Watch glass

(a) Preparation of standard solution of sodium carbonate

• Molecular weight of sodium carbonate = 106
• Amount of sodium carbonate required to prepare solution of 250ml = 1.325g
• Dissolve 1.325g of sodium carbonate in distilled water and prepare the standard solution in 250ml of measuring flask by adding the required amount of water.

(b) Titration of hydrochloric acid and sodium carbonate solution

• Wash, rinse and fill the burette with M/10 Na 2 CO 3 solution. Note the initial reading.
• Take 10cm 3 of HCl solution with the help of a pipette and transfer it into a clean washed titration flask.
• Add 2 drops of methyl orange into the titration flask.
• Add M/10 sodium carbonate solution to the titration flask till the colour changes to the light pink.
• Note the final reading and find out the volume of sodium carbonate solution used to neutralize HCl solution.
• Repeat the experiment till you get concordant readings.

Volume of HCl solution = 10cm 3

Volume of sodium carbonate solution used = V cm 3

(Sodium carbonate) a 1 M 1 V 1 = (HCl) a 2 M 2 V 2

The strength of hydrochloric acid solution is ________ g/L.

• While weighing do not spill the substance on balance pan.
• Rotate the knob of balance gently.
• Keep the weights in weights box at proper places after weighing
• Wash the watch glass carefully so that even a single crystal is not left on the watch glass.
• Bring the watch glass close to funnel while transferring weighed substance and transfer it gently. Wash it repeatedly with distilled water.
• Wash the burette with water after titration is over.
• Last few drops should be added using pipette to avoid extra addition of distilled water above the mark on the neck of the measuring cylinder.

Frequently Asked Questions on Titration of Hydrochloric Acid against Standard Sodium Carbonate

What is normality .

Normality is defined as number of gram equivalents dissolved per litre of solution. \(\begin{array}{l}N = \frac{Strength\ of\ solution\ in\ g/L}{Equivalent\ weight\ of\ solute\ in\ grams}\end{array} \)

What is the burette used for ?

Burette is a glass apparatus used for titration. It is used for delivering out any volume of a liquid under controlled conditions between a certain range.

What is the end point ?

The stage during titration at which the reaction is just complete is known as end point. At the end point the chemical reaction is said to be completed. Indicators are used to find out the end point accurately.

Why is it necessary to rinse the burette or pipette with the liquid it is filled ?

It is to be washed with water and then with distilled water only and it is not to be rinsed.

Name few common indicators.

Phenolphthalein, methyl orange, starch etc are some common indicators used to find out the endpoint in volumetric analysis.

Put your understanding of this concept to test by answering a few MCQs. Click ‘Start Quiz’ to begin!

Select the correct answer and click on the “Finish” button Check your score and answers at the end of the quiz

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• Titration of Hydrochloric Acid against Standard Sodium Carbonate

Titration of Na₂CO₃ with HCl

Methods of acid-base titration based on a sample dissolution exceeding normal acid, followed by back titration with a standard base is characterised in this experiment. Using bromophenol blue as an indicator, hydrochloric acid solutions were standardised against pure sodium carbonate. Here, we will study the titration of HCl and sodium carbonate in detail.

Determination of the strength of the diluted hydrochloric acid solution by titrating it against the normal sodium carbonate solution (M/10).

The hydrochloric acid solution can be titrated using a methyl orange indicator against the sodium carbonate solution. If a slightly acidic solution is titrated with a weak base, the endpoint is slightly acidic. The solution is slightly basic if a weak acid is titrated with a strong base since the salt produced is to a certain degree hydrolyzed. The reaction of sodium carbonate with HCl is given below.

Na 2 CO 3 (aq) + 2HCl(aq) → 2NaCl(aq) + CO 2 (g) + H 2 O(l)

CO 3 2- (aq) + 2H+(aq) → CO 2 (g) + H 2 O(l)

These are the hydrochloric acid and sodium carbonate equations.

In acid-base titrations, the amount of the acid becomes chemically equivalent to the amount of base present. The solution becomes neutral in the event of a strong acid and a strong base titration of the solution.

Materials Required

Conical flask

Burette stand

White glazed tile

Measuring flask

Hydrochloric acid

Sodium carbonate

Methyl orange

Watch glass

Procedure for Titration of HCl and Sodium Carbonate

A. Preparation of a Sodium Carbonate Standard Solution

Sodium carbonate has a molecular weight of 106.

The amount of sodium carbonate needed to make a 250mL solution is 1.325g.

Prepare the standard solution by dissolving 1.325g of sodium carbonate in distilled water and adding the required amount of water to a 250ml measuring flask.

B. Titration of Hydrochloric Acid and Sodium Carbonate Solution

Wash, rinse, and fill the burette with M/10 Na 2 CO 3 solution. Note the initial reading.

Take 10cm 3 of HCl solution with the help of a pipette and transfer it into a clean washed titration flask.

Add 2 drops of methyl orange into the titration flask.

Add M/10 sodium carbonate solution to the titration flask till the colour changes to light pink.

Note the final reading and find out the volume of sodium carbonate solution used to neutralise the HCl solution.

Repeat the experiment till you get concordant readings.

Observation

Volume of HCl solution = 10cm 3 .

The volume of sodium carbonate solution used = V cm 3 .

Calculation

(Sodium carbonate) a 1 M 1 V 1 = (HCl) a 2 M 2 V 2 .

2 × 1/10 × V = 1 × x × 10 x = V/5 Strength in g/L = molarity × molar mass = V5 × 36.5.

The strength of the hydrochloric acid solution is ________ g/L.

Precautions

Do not spill the material on the balance pan while measuring.

Gently turn the balance knob.

After weighing, put the weights in the weights box in the correct positions.

Wash the watch glass thoroughly to ensure that not a single crystal remains on it.

When moving the weighted substance, bring the watch glass close to the funnel and gently move it. It should be washed multiple times with distilled water.

After the titration, wash the burette with water.

To prevent applying distilled water above the mark on the neck of the measuring cylinder, the last few drops should be applied with a pipette.

Did You Know?

Hydrochloric acid, also known as muriatic acid, is a hydrogen chloride aqueous solution. It's a colourless liquid with a strong, pungent odour. It's considered a strong acid. In the digestive systems of most animal species, including humans, it is a component of gastric acid. Hydrochloric acid is a common laboratory reagent as well as a common industrial chemical.

The boiling and melting points, density, and pH of hydrochloric acid are all influenced by the concentration or molarity of HCl in the aqueous solution. They range from values for water at very low concentrations near 0 percent HCl to over 40 per cent HCl for fuming hydrochloric acid.

Hydrochloric acid is produced by dissolving hydrogen chloride in water in an industrial environment. Hydrogen chloride can be produced in a number of ways, but there are some precursors to hydrochloric acid. In the chlor alkali process, which produces hydroxide, hydrogen, and chlorine, the latter of which can be combined to produce HCl, large-scale production of hydrochloric acid is almost always incorporated with industrial-scale production of other chemicals.

This study material must have given you an overview of the topic titration of HCl and sodium carbonate. You must have got an insight into the topic and given your brain one more concept to store. 

Chemistry is often considered to be a challenging subject for most students. But, once given the right attention and effort, it can be more of an experimental subject. 

Let us starlight jump on to learn some of the proven tricks and techniques that will make chemistry simpler and also increase your ability to learn it. 

Review the study material and then attend the lecture 

The best technique to ace in chemistry is to do reading of the study material beforehand and then when you attend the class, you get to understand but while understanding you may find some points relatable which your mind will catch faster and store into it. Another good thing about it is that you already have read it, so you might have questions that will be solved then and there. From this technique, the class time is utilized more efficiently and also each lecture gives you more understanding that finally, leads to better results. 

Take good notes

Attending classes regularly and taking all the notes is vital. Notes can help you in the last days of preparation and also are very handy. You can only take good notes if you pay attention to the class and avoid distractions. Make sure that whatever notes you take, should be organized as it will help you to review the class that you have attended, whenever you want to. Also, another important advantage is that it forces you to write all the points which will, in turn, help you to remember the concepts easily. 

Focus on your work not grade

Chemistry is a subject that needs complete concentration. If you will shift your focus from learning and understanding the concepts of chemistry to score better grades, it would take away all the concentration which would surely affect your final results. Hence, students are advised to always focus on learning and understand that the grades would always follow. 

Use study groups

Using study groups is a very good way to manage the learning of any challenging subject. Chemistry is indeed a challenging subject that is full of formulas and symbols and vocabulary. Using a study group will help you to share insights with others and also hear out to them. You can also have a look at the notes they have, clear doubts, and exchange many ideas. However, creating a large group might also result in so much confusion and hence, students are advised to make a small group and make the most out of it. Your study sessions should not be very long, only till the time that you find it productive, and later, you should make time for self-study. 

Take advantage of lab time

There is no better way to learn chemistry than hands-on experience. Chemistry labs can be very helpful if you try to make the best use of them. Students shall never be missing any chance of being in a lab. This will help you strengthen your knowledge of chemistry and also enhance your understanding of the concepts

To conclude, based on your observations and understanding, you may come across a lot of study tips, tricks, techniques and suggestions but you may only pick up the ones that you think would suit you the best. 

There may be times when you might think that some strategy is working so well for your partner and you would also get the same results, but then, it doesn't work that way. 

Students are advised to work based on their study habits and patterns and not under the influence of others. 

Success might not always come easy but if you choose not to give up and keep moving ahead despite the challenges, it will come to you, sooner or later. This is what we shall be waiting for and let its vision fuel as continuously.

FAQs on Titration of Hydrochloric Acid against Standard Sodium Carbonate

1. What is the Best Way to Titrate a Solution of Na 2 CO 3 and NaHCO 3 Against HCl?

Na 2 CO 3 and NaHCO 3  estimation in a mixture: Prepare a solution of distilled water in a 250 ml regular flask by correctly measuring around 2.0 g of the mixture. Using phenolphthalein as an indicator, slowly titrate 25 mL of this solution against regular hydrochloric acid. To concordance, repeat the process (V p ml).

2. Why is Hydrochloric Acid not Used as a Primary Standard?

Primary Standards for Acid-Base Titrations:

Since both hydrochloric acid, HCl, and sulfuric acid, H 2 SO 4 , are readily available as condensed solutions that can be easily diluted, the concentration of the "concentrated" solution is not precisely determined, they are not suitable for use as primary criteria.

3. How do You Prepare and Standardize 0.1 N HCl?

Preparation and Standardization of 0.1 M Hydrochloric acid (HCl).

In a 1000 mL volumetric flask that has been washed and dried, pour about 100 mL of water.

Add approximately 8.5 mL of Conc.

Mix in another 700 mL of water and set aside to cool to room temperature.

Fill the jar with 1000 mL of water.

Give at least one hour for the solution to settle before continuing with the standardization.

4. How can I become a chemist? 

The course for a chemist is one of the most interesting courses. This includes some specialized subjects like organic chemistry, analytical chemistry, physical chemistry, instrumental analysis, calculus, physics and computer science. And if you wish to know more about chemistry as a career option, you can check out the online website of Vedantu where you get all the knowledge about the same. 

5. What are the job opportunities in chemistry? 

If you desire to keep the subject of chemistry as your career field, you have many doors open in front of you. There are a lot of career options in the field of chemistry, some of them are chemical engineers, analytical chemists, biochemists and much more. If you want to know about all of them,  you can check the online website of Vedantu which offers you all the related information.