Class 11 chemistry · linked to Mole, formula, and concentration · Basic laboratory techniques
Source: CBSE Class 11 chemistry practical syllabus · use your school laboratory manual (NCERT Lab Manual where your school uses it).
Preparing a molar solution (Class 11 chemistry practical)
You practise making a solution of known molarity from a solid solute in a volumetric flask.
The mass, molar mass, and target molarity come from your laboratory manual — not from this page.
Published practice page. Concentrations, masses, and numerical answers come from your school laboratory manual and your own readings — not invented here. Not yet reviewed by a named chemistry reviewer. Version 1.0.0, updated 2026-10-03.
Safety — read before you start
Safety warning. Practise here. Perform the real experiment only in your school lab, with your teacher present.
- Some solutes are irritant or toxic — read the label your teacher provides.
- Broken volumetric glassware cuts; handle carefully.
Wear: Lab coat, Splash goggles, Gloves, as your teacher directs.
Follow your teacher’s disposal instructions. Do not pour leftovers down a household drain.
Loads only after you tap. Use the lab hands to pick up and use equipment (pointer hidden in the scene). Falls back to a flat diagram if WebGL is unavailable.
Aim
To prepare a standard aqueous solution of a given molarity by dissolving a calculated mass of solute in a volumetric flask, using the values in your laboratory manual.
Methods and quantities can differ between schools. Follow your teacher's instructions.
Apparatus and chemicals
| Item | Note |
|---|---|
| Volumetric flask | Capacity as per your manual. |
| Analytical / school balance | Use the precision your teacher requires. |
| Beaker and glass rod | For dissolving before transfer. |
| Funnel and wash bottle | Distilled water only for make-up. |
| Watch glass | For weighing the solid. |
| Assigned solute (solute) | Name, grade, and mass are not printed here until checked against your manual. |
| Distilled water (H2O) | Solvent for make-up to the mark. |
Theory and reaction
Open
Molarity M = moles of solute / litres of solution.
moles = mass / molar mass. Solve for mass once M and V are fixed by the manual.
The meniscus sits on the calibration mark after the solid is fully dissolved and the solution is mixed.
Molarity = moles / litres. moles = mass / molar mass.
Procedure
- Read the target molarity, flask volume, and solute name from your manual. Calculate the mass you need.
- Weigh that mass on a clean watch glass using the balance procedure your teacher shows.
- Dissolve the solid in a beaker with less than the flask’s full volume of distilled water. Stir until clear (or as the manual describes for that solute).
- Transfer quantitatively into the volumetric flask. Rinse the beaker and rod into the flask.
- Add distilled water carefully until the meniscus sits on the mark. Stopper and invert to mix.
- Label the flask with solute, molarity, date, and your name.
Observation table
Enter the readings from your school lab in the practical file below. This page does not fill them in for you.
Calculation
mass = M × V(L) × molar mass. Use only the M, V, and molar mass from your manual. No worked number is shown here until review.
Result
Write the molarity you prepared and the mass you actually weighed, with units. Leave blank if your teacher collects a different record format.
Precautions
- Never make up to the mark before the solid has dissolved.
- Read the meniscus at eye level.
- Do not heat a volumetric flask unless your teacher explicitly allows a different vessel for dissolving.
Viva questions
Answer one question at a time. The full answers stay closed until you open them.
Question 1 of 3
Molarity is moles of solute per…
Pick an answer first.
Show all questions and answers
Molarity is moles of solute per…
Answer: litre of solution. Reason: M uses solution volume in litres.
Why finish at the calibration mark after dissolving?
Answer: So the solution volume matches the flask’s stated volume. Reason: Molarity needs a known solution volume.
Molality differs from molarity because molality uses…
Answer: kg of solvent. Reason: Molality = moles / kg solvent.
Common mistakes
- Using the beaker volume as if it were the volumetric flask.
- Forgetting to rinse solute stuck on the watch glass or funnel into the flask.
- Copying a mass from a friend’s notebook instead of calculating from your manual.
Frequently asked questions
- Can I do this at home?
- No. Use this page to practise the order of ideas and steps. Do the real experiment only in your school laboratory, with your teacher present.
Your practical file
Name, school, and roll number are optional and are not sent anywhere.
The practical file opens on this device.
Review
Not yet reviewed by a named chemistry reviewer. Published for practice only — follow your teacher and laboratory manual for quantities and safety.
Related notes
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