Mole Calculation Mastery Workskop

Hi Students,

2 months to GCE O Level, Have you scored the marks you truly deserved?

Is Mole Calculations your #1 Killer Topic?

Click here to find out more



Over the years, this topic is often voted the “Hot Favorite” on students’ challenging topics. Some have

- problems understanding what the question is asking for,
- do not know where to start,
- totally blank when they read the question,
- too confused with the formulaes to use…WHY?

Click here to find out more

Let’s check out a typical exam question on Mole Calculations:

Question:

The following equation represents the precipitation reaction between lead (II) nitrate solution and potassium iodide solution.

aPb(NO3)2(aq) + bKI(aq) –> cPbI2(s) + dKNO3(aq)

In an experiment, 20.0g of lead(II) nitrate and 20.0g of potassium iodide were dissolved separately to form 250cm3 of lead (II) nitrate solution and 250cm3 of potassium iodide solution.

(a) Determine a, b, c and d. (2 marks)

(b) Using suitable calculation, identify the limiting reactant. (2 marks)

(c) What is the maximum mass of lead (II) iodide (PbI2) that can be obtained from the experiment? (2 marks)

(d) What is the concentration of potassium nitrate in the reaction mixture when the reaction is completed? Give your answers in mol/dm3. (2 marks)

(e) Write an Ionic Equation for the above reaction and identify the spectator ion. (2 marks)

Here is the answers:

a) a = 1 , b = 2, c = 1 and d = 2

b) KI is the Limiting Reactant.

c) Maximum mass of PbI2 that can be obtained = 27.8g (to 3 sf)

d) Concentration of KNO3 = 0.241 mol/dm3

e) Ionic Equation: Pb2+(aq) + 2I-(aq) à PbI2(s). Spectator Ions: NO3-(aq) and K+(aq)

PS: If you cant solve those questions comfortably, i strongly encourage to join us at the Mole Calculations Mastery WOrkshop on 16th Aug, where you know everything that you need for Mole Concepts, before your nearing Exams.

Click here to find out more