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Module 1: Practical chemistry for exams›PAG 2.3 - Identification of an unknown carbonate

PAG 2.3 - Identification of an unknown carbonate

An overview of PAG 2.3 - Identification of an unknown carbonate

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In OCR Chemistry Required Practical 2 (PAG 2.3), titration is used to identify an unknown metal carbonate with the formula .

By making up a solution of known gravimetric concentration of the carbonate and using titration to find the molar concentration, mass and moles are obtained.

This allows for the subsequent calculation of , which is used to identify the metal X.

In OCR PAG 2.3: Identification of an unknown carbonate, there are several important safety requirements to be aware of (beyond normal lab practice such as wearing goggles).

Use a pipette filler – never pipette by mouth.
Immediately clean up any spills of acid or alkali.

Experimental method for OCR Chemistry Required Practical 2 (PAG 2.3)

Part 1: Making the standard solution

A step-by-step guide for an experimental method involving the weighing and dissolving of sodium carbonate (X2CO3) in distilled water, transferring the solution to a volumetric flask, and ensuring the final volume is exactly 250 cm³. The guide includes illustrations of the equipment used, such as a balance, beaker, stirring rod, funnel, and volumetric flask.

Experimental method for OCR Chemistry Required Practical 2 (PAG 2.3)

Part 2: Performing the titration

An instructional infographic detailing the experimental method for a titration procedure, including steps for measuring a carbonate solution, adding an indicator, filling a burette with hydrochloric acid, conducting rough and accurate titrations, and recording results in a table.

The precision of the balance used is critical for ensuring the accuracy of mass measurements and subsequent calculations.

A digital laboratory scale with a circular weighing platform and a blue control panel displaying a reading of 0.00.

Do

Measure solids and liquids precisely. Ensures accurate mole calculations and enthalpy values. A balance with a resolution of at least two decimal places should be used.

A digital weighing scale with a round platform and a red control panel displaying '0.0' on a green screen.

Don't

Use a balance with a resolution of 1 decimal place or lower.

Avoid unintentional dilution of solutions.

A laboratory pipette with a graduated scale on the side, positioned next to a container labeled NaOH, indicating the presence of sodium hydroxide.

Do

Rinse all glassware used for accurately measuring solution volumes with the solution itself.

A pipette is shown with a container above it labeled 'Distilled water'.

Don't

Rinse precision glassware with water immediately before use – leftover water will dilute the solution.

Prevent parallax errors when reading volumes.

An illustration showing a measuring cylinder with a scale marked from 20 to 25 ml. An eye is depicted on the left side, and a green arrow points to the measurement of 22.14 ml.

Do

Read the burette at eye level and record to

A measurement scale showing values from 20 to 25 ml. Two eyes are illustrated, one pointing to 22.26 ml and the other to 22.02 ml, with red arrows indicating the measurements.

Don't

Read from above or below – this leads to incorrect readings due to parallax error.

Use only the minimum amount of indicator needed in acid base titration.

A laboratory scene featuring a flask with pink liquid and a dropper above it. Next to the flask is a bottle labeled 'Phenolphthalein' containing blue liquid.

Do

Add just 2–3 drops of phenolphthalein to the flask.

A laboratory scene showing a bottle labeled 'phenolphthalein' pouring a blue liquid into a flask containing a pink solution.

Don't

Add too much indicator – Indicators are weak acids. Excess indicator can affect the pH and affect the titration end point.

Keep the titration mixture well mixed.

A hand holding a conical flask containing a pink liquid, with arrows indicating swirling motion, and a dropper above the flask.

Do

Swirl the conical flask gently and consistently during titration to ensure complete contact between reactants.

A laboratory setup featuring a conical flask with a pink liquid inside, topped with a pipette holder and a blue pipette.

Don't

Leave the flask still during titration – without swirling, the acid and alkali will not mix properly, leading to an inaccurate endpoint.

Control the addition of acid as you approach the endpoint.

Two hands are holding a flask with a pink liquid inside. One hand is using a dropper to add a drop of liquid into the flask.

Do

Add the sodium hydrogensulfate drop by drop near the end point.

A laboratory setup featuring a conical flask with red liquid at the bottom and a blue pipette dispensing a clear liquid into the flask.

Don't

Add too quickly – it is easy to miss the exact endpoint and overshoot the titre.

Ensure your standard solution is fully mixed.

Hands holding a stopper flask, with the instruction 'Stopper flask and invert several times to mix' displayed beside it.

Do

Invert the volumetric flask several times after filling to the graduation mark.

A volumetric flask filled with blue liquid, labeled 'Volumetric flask: still and not inverted.'

Don't

Use the standard solution without inversion – The top of the solution may be less concentrated than the bottom. Even small concentration differences can affect the accuracy of your results.

Ensure the burette is free from air bubbles.

A laboratory apparatus showing a graduated pipette filled with liquid, indicating 'No air bubbles' next to the pipette.

Do

Check the burette for air bubbles and remove them by running some solution through the tap before starting the titration.

A diagram of a pipette filled with blue liquid, showing air bubbles at the tip. The pipette has measurement markings on the side and is connected to a gray stopcock.

Don't

Start titrating with air bubbles in the burette – The volume occupied by the bubble will be taken into your volume reading. Less solution will actually be transferred than is recorded.

Use concordant titres (within 0.1 cm³) to calculate the mean titre. Calculate the moles of using:

Then use the balanced equation to calculate the moles of in the aliquot and then in the full solution. Calculate the molar mass:

Subtract the mass contribution from to determine and identify