ICE Table and pH Calculations

The video tutorial explains the use of the ICE table to calculate the pH of weak acids and bases. It covers the concept of initial concentration, change, and equilibrium, and demonstrates the process with examples of citric acid and ammonia. The tutorial highlights the assumptions made for weak acids and bases and how to use the Ka and Kb expressions to find the pH.

What does the 'I' in the ICE table stand for?

• Inert substance

• Intermediate state

• Ionization constant

• Initial concentration

Why do we use the ICE table for weak acids and bases?

• They fully ionize in water

• They do not ionize at all

• They only partially ionize in water

• They are strong electrolytes

In the ICE table for citric acid, what is the initial concentration of the dissociated ions?

• 1 mole per dm³

• 0 mole per dm³

• 0.1 mole per dm³

• 0.22 mole per dm³

What assumption is made about 'x' when calculating the pH of a weak acid like citric acid?

• x is large compared to initial concentration

• x is twice the initial concentration

• x is negligible compared to initial concentration

• x is equal to the initial concentration

What is the pH of citric acid when the concentration of hydrogen ions is 0.012759 mole per dm³?

• 7.00

• 14.00

• 1.89

• 3.00

What is the initial concentration of ammonia in the ICE table example?

• 0.22 mole per dm³

• 0.100 mole per dm³

• 1.00 mole per dm³

• 0.012 mole per dm³

Why is water not included in the ICE table for ammonia?

• It is a strong base

• It does not participate in the reaction

• It is a strong acid

• It is already ionized

What is the pOH of ammonia when the concentration of hydroxide ions is 1.3191 x 10^-3 mole per dm³?

• 14.00

• 7.00

• 11.12

• 2.88

How do you convert pOH to pH?

• Add 7 to pOH

• Divide pOH by 2

• Multiply pOH by 2

• Subtract pOH from 14

What is the final pH of ammonia in the example provided?

• 7.00

• 11.1

• 1.89

• 2.88