NH4CL , ZNCL2 , KAL(SO4)2
FIND THE FOLLOWING
NET IONIC EQUATION FOR HYDROLYSIS
EXPRESSION FOR EQUILIBRIUM CONSTANT (KA OR KB)
VALUE
THANK YOU SO MUCH!!!
Here is how you do these.
........NH4^+ + H2O ==>H3O^+ + NH3
Ka = (H3O^+)(NH3)/(NH4^+)
Ka for NH4^+ = (Kw/Kb for NH3)= ?
To find the net ionic equation for hydrolysis, we need to determine which ions from the given compounds will react with water to form ions that can participate in a chemical reaction.
1. NH4Cl:
When NH4Cl is dissolved in water, it dissociates into NH4+ and Cl- ions. The NH4+ ion does not undergo hydrolysis, but the Cl- ion reacts with water to form HCl(aq) and OH-.
The net ionic equation for the hydrolysis of NH4Cl can be written as:
Cl- + H2O -> HCl + OH-
2. ZnCl2:
When ZnCl2 is dissolved in water, it dissociates completely into Zn2+ and Cl- ions. The Zn2+ ion does not undergo hydrolysis, but the Cl- ion reacts with water to form HCl(aq) and OH-.
The net ionic equation for the hydrolysis of ZnCl2 can be written as:
2Cl- + 2H2O -> 2HCl + 2OH-
3. KAl(SO4)2:
When KAl(SO4)2 is dissolved in water, it dissociates into K+, Al3+, and (SO4)2- ions. Neither K+ nor Al3+ undergo hydrolysis, but the (SO4)2- ion reacts with water to form H2SO4(aq) and OH-.
The net ionic equation for the hydrolysis of KAl(SO4)2 can be written as:
(SO4)2- + 2H2O -> H2SO4 + 2OH-
Now, moving on to the expression for the equilibrium constant (Ka or Kb), we can determine the value by examining the balanced chemical equation for the hydrolysis reaction.
The expression for the equilibrium constant for the net ionic equation can be written as:
Kw = [H+][OH-]
Since Kw (the equilibrium constant for water) is equal to 1.0 x 10^-14 at 25°C, we can substitute it into the expression:
1.0 x 10^-14 = [H+][OH-]
Finally, to find the value of either [H+] or [OH-], we need additional information about the system or conditions of the reaction.
Note: The values or specific calculations for the equilibrium constant will depend on the concentration or activity of the ions in the solution and any other relevant factors in the specific context of the experiment or problem.
To find the net ionic equation for hydrolysis, we need to first identify the ions that are involved in the hydrolysis of each compound.
1. NH4Cl:
The compound NH4Cl dissociates in water to form NH4+ and Cl- ions. The hydrolysis of NH4+ can be represented by the following equation:
NH4+ + H2O ⇌ NH3 + H3O+
2. ZnCl2:
Similarly, ZnCl2 dissociates in water to form Zn2+ and 2Cl- ions. However, neither of these ions undergoes significant hydrolysis. Therefore, we can conclude that the hydrolysis of ZnCl2 does not contribute to the net ionic equation.
3. KAl(SO4)2:
The compound KAl(SO4)2 dissociates in water to form K+, Al3+, and 2(SO4)2- ions. The hydrolysis of Al3+ can be represented by the following equation:
Al3+ + 3H2O ⇌ Al(OH)3 + 3H+
Now, let's write the net ionic equation by excluding the spectator ions (ions that are present on both sides of the equation and do not participate in the reaction):
NH4+ + H2O ⇌ NH3 + H3O+
Al3+ + 3H2O ⇌ Al(OH)3 + 3H+
Regarding the expression for the equilibrium constant (Ka or Kb), we need to determine whether the hydrolysis is acidic or basic.
1. NH4Cl:
The hydrolysis of NH4+ results in the formation of H3O+ ions, indicating an acidic hydrolysis reaction. The equilibrium constant expression (Ka) can be written as:
Ka = [NH3][H3O+]/[NH4+]
2. ZnCl2:
As mentioned earlier, ZnCl2 does not undergo significant hydrolysis. Therefore, there is no equilibrium constant expression for this compound.
3. KAl(SO4)2:
The hydrolysis of Al3+ results in the formation of OH- ions, indicating a basic hydrolysis reaction. The equilibrium constant expression (Kb) can be written as:
Kb = [Al(OH)3][OH-]/[Al3+]
I apologize, but I cannot provide you with the specific values of the equilibrium constants (Ka or Kb) without additional information or access to a database.
I hope this helps! Let me know if you have any further questions.