A reaction of hydrolysis of Ba(NO) in a net ionic form?
To write the net ionic equation for the hydrolysis of Barium Nitrate (Ba(NO3)2), we need to know whether it is taking place in an acidic or basic solution. Since you did not specify, I'll assume it is taking place in water.
Step 1: Write the balanced molecular equation.
The chemical formula for Barium Nitrate is Ba(NO3)2. When it reacts with water, it can be represented as follows:
Ba(NO3)2 + H2O → Ba(OH)2 + HNO3
Step 2: Separate the soluble ionic compounds into their constituent ions.
Barium Nitrate dissociates into Ba2+ and NO3- ions in water, while water itself is not an ion.
Ba(NO3)2 → Ba2+ + 2NO3-
H2O → H+ + OH-
Step 3: Write the net ionic equation.
Only those ions that participate in the reaction are written in the net ionic equation. Since the Nitrate ions (NO3-) and Hydroxide ions (OH-) do not change during the reaction, they are not included in the net ionic equation.
Ba2+ + 2H2O → Ba(OH)2 + 2H+
Therefore, the net ionic equation for the hydrolysis of Ba(NO3)2 in water is:
Ba2+ + 2H2O → Ba(OH)2 + 2H+
To determine the net ionic form of the hydrolysis reaction of Ba(NO)2, we first need to write the balanced molecular equation, and then break it down into its ionic components.
Step 1: Write the balanced molecular equation:
Ba(NO)2 + H2O → Ba(OH)2 + HNO3
Step 2: Separate the soluble compounds into ions:
Ba(NO)2 → Ba^2+ + 2NO3^-
H2O → H+ + OH-
Ba(OH)2 → Ba^2+ + 2OH^-
HNO3 → H+ + NO3^-
Step 3: Form the net ionic equation by canceling out spectator ions:
Ba^2+ + 2OH^- + 2H+ + 2NO3^- → Ba^2+ + 2OH^- + 2H+ + 2NO3^-
In this case, the net ionic equation is the same as the molecular equation because there are no spectator ions. Therefore, the net ionic form of the hydrolysis of Ba(NO)2 is:
Ba(NO)2 + H2O → Ba(OH)2 + HNO3