2. What physical/chemical properties allowed you to separate and confirm Lead (I

Question

2. What physical/chemical properties allowed you to separate and confirm Lead (II), Mercury (I), and Silver)? Explain your answer in terms of Ksp SP. 3. What is the common ion effect? How does Le Chatelier's principle explat Where did you observe this phenomenon in this lab? 4. Explain your expected results if you had made the following errors during the lab: a) 6 M NH, is accidentally added instead of hot water in the step used to separate PbCl, from AgCl and Hg,Cl. b) You did not wash the filter paper with hot water before filtering in the step used to separate PbCl2 from AgCl.and Hg,C

Explanation / Answer

3) We know that weak acids and weak bases slightly ionize in water and equilibrium is established in their solutions. The phenomenon of suppression of the degree of dissociation of a weak acid or a weak base by the addition of a strong electrolyte containing a common ion is known as common ion effect.

For example: let us consider the ionization of a weak base ammonium hydroxide i.e. NH4OH as:
NH4OH (aq) NH4+ (aq) + OH– (aq).

The common-ion effect is used to describe the effect on an equilibrium involving a substance that adds an ion that is a part of the equilibrium. Adding a common ion prevents the weak acid or weak base from ionizing as much as it would without the added common ion. LeChatelier's Principle states that if an equilibrium gets out of balance it will shift to restore the balance. If a common ion is added to a weak acid or weak base equilibrium, then the equilibrium will shift towards the reactants, in this case the weak acid or base.

For Example :

The Common ion effect of OH- on the ionization of Ammonia(NH3)

Whwn a strong base supplies the common ion OH- the equilibrium shift to form more NH3

NH3+H2O (Reversible reaction symbol) NH4+OH- (Added ion) In this case Equilibrium shift to form more NH3

Thefore, adding the common ion of hydroxide, shifts the reaction towards the left to decrease the stress (Le Chatelier's Principle), forming more reactants. This decreases the reaction quotient, for the reaction is being pushed towards the left to reach equilibrium

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