What are the different types of JC Chemistry tuition classes available at your centre?

We have 3 modes of learning for students to choose from: weekly physical classes at Bishan; weekly online lessons via Zoom; and on-demand video lessons.

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Please be rest assured that I conduct all my classes personally and I do not engage other tutors to teach at my centre.

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Most of my students showed improvements by at least 3 grades and more than 80% have attained distinction for A Levels. The earlier the students join my classes, the more confident I am in improving their grades.

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Usually the class size is around 10 to 12 students. Max class size is 16 pax.

Is there makeup lesson if I miss a class?

Yes makeup lesson is available in the same week subject to availability. If makeup class is not possible, the student can view the recorded video lessons at Google Classroom.

Do you have trial lesson available? How much is it?

Yes we do. Fees for trial lesson are for Bishan class and for Zoom online class.

Does your centre offer O Level chemistry tuition? Do you teach IB / IP chemistry tuition? How about H1 Chemistry?

Chemistry Guru specialises in H2 Chemistry for JC1 and JC2 or IP Year 5 and IP Year 6 students only. Find out all the information about A Level H2 Chemistry and the detailed comparison between H1 and H2 Chemistry. We do not conduct lessons for H1 Chemistry, O Level Chemistry, IB Chemistry or IP Chemistry at IP Year 3 and IP Year 4.

Common Ion Effect

In this JC2 webinar let's discuss common ion effect and how it suppresses solubility of sparingly soluble salts.

Let's consider the scenario where we have a solution of silver nitrate (AgNO₃) and silver chloride (AgCl).

common ion effect mixture of AgCl and AgNO3

Silver nitrate is soluble so will be fully dissociated in solution to form Ag⁺ and NO₃^- ions.

Silver chloride is sparingly soluble so will only be partially dissociated to form some Ag⁺ and Cl^- ions.

common ion effect dissociation of salts

Notice both salts give Ag⁺ ions.

Since this ion is dissociated from both salts, we call this the common ion.

The presence of common ion from AgNO₃ will increase the total Ag⁺ concentration in solution.

This will affect the position of equilibrium for AgCl dissociation.

According to Le Chatelier's Principle, an increase in concentration of product will shift the position of equilibrium towards the left to reduce the concentration of product.

Check out the following video lesson for a detailed discussion on Le Chatelier's Principle.

common ion effect shift in position of equilibrium

This means that more AgCl solid will be formed, and less of the salt dissolves, ie decrease or suppression of solubility.

In general the presence of a common ion will suppress the solubility of a sparingly soluble salt.

Topic: Solubility Product, Physical Chemistry, A Level Chemistry, Singapore

Back to other previous Physical Chemistry Video Lessons.

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Common Ion Effect

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