The presence of ammonia in a solution of AgCl will decrease the solubility of AgCl.
True Or False
Absolutely false. It will increase the solubility BECAUSE of the formation of the complex Ag(NH3)2Cl
AgCl + 2NH3 ==> Ag(NH3)Cl
The standard enthalpy of fusion of iodobenzene is 9.75 kJ/mol at its melting point, 241.8 K. What is the standard change in entropy for the melting of iodobenzene at its melting point?
A) –9.75 J/(mol • K)
B) –311 J/(mol • K)
C) 0.0403 J/(mol • K)
D) 40.3 J/(mol • K)
E) 0.0189 J/(mol • K)
True.
The presence of ammonia in a solution of AgCl (silver chloride) will decrease the solubility of AgCl. Ammonia forms a complex with silver ions, Ag+, to create the complex ion [Ag(NH3)2]+. This complex ion is less soluble than AgCl, causing a shift in equilibrium and reducing the solubility of AgCl.
True. The presence of ammonia (NH3) in a solution of AgCl (silver chloride) will decrease the solubility of AgCl. This is due to the formation of a complex ion known as Ag(NH3)2+, which reduces the concentration of Ag+ ions in the solution. The decreased concentration of Ag+ ions shifts the equilibrium of the dissolution reaction towards the direction of less dissolution, resulting in decreased solubility of AgCl.
To understand this concept, we can refer to the solubility product (Ksp) expression for AgCl, which is given as follows:
AgCl ⇌ Ag+ + Cl-
The equilibrium expression for this reaction can be written as:
Ksp = [Ag+][Cl-]
When ammonia is added to the solution, it can react with Ag+ ions to form Ag(NH3)2+ complex ions according to the equation:
Ag+ + 2NH3 ⇌ Ag(NH3)2+
As a result, the concentration of Ag+ ions in the solution decreases, leading to a decrease in the solubility of AgCl. Therefore, the statement that the presence of ammonia in a solution of AgCl decreases its solubility is true.