CO(h20)6 2+ + 4Cl- <=> CoCl4 2- + 6H20
What would AgNO3 do when added to this?
What is the equilibrium expression?
See above.
Because AgNO3 has nitrate in it, and nitrate is ALWAYS soluable, the AgNO3 dissociates 100%, which means that in the solution there are Ag+ and NO3- ions.
When added to this equation, the Ag+ ions and Cl- ions will react using up some of the Cl- ions in the reactants side, thus the shift will be to the left to make up for any used Cl- ions that reacted.
The equilibrium expression is always the concentration of products divided by concentration of reactants.
Thus Kc=[CoCl4][H2O]/[Co(H2O)6+2][Cl-]
When AgNO3 is added to the reaction, it would form a precipitate with the chloride ions (Cl-) present in the reaction. The silver ions (Ag+) would react with the chloride ions (Cl-) to form silver chloride (AgCl), which is insoluble and would precipitate out of the solution.
The equilibrium expression for the given reaction is:
[CoCl4 2-][H2O]^6 / [Co(H2O)6 2+][Cl-]^4
To determine what AgNO3 would do when added to the given equation, we need to identify if it reacts with any of the compounds present in the equation.
From the equation, we can see that there are chloride ions (Cl-) present as a reactant. AgNO3 is silver nitrate, which contains Ag+ ions. Silver ions have a strong affinity for chloride ions, leading to the formation of a white precipitate called silver chloride (AgCl).
When AgNO3 is added to the equation, it will react with the chloride ions (Cl-) present and form AgCl precipitate. So, the overall reaction would be:
Ag+ + Cl- -> AgCl (s)
Now, let's move on to the equilibrium expression:
The equilibrium expression is a mathematical representation of the ratio of the concentrations of products and reactants at a given point of equilibrium. It is usually written using the concentrations of species raised to the power of their respective stoichiometric coefficients.
In the given equation:
CO(H2O)6 2+ + 4Cl- <=> CoCl4 2- + 6H2O
The equilibrium expression would be:
K = [CoCl4 2-] / [CO(H2O)6 2+] * [H2O]^6 / [Cl-]^4
Where:
- K represents the equilibrium constant for the reaction.
- [CoCl4 2-] represents the concentration of CoCl4 2- ions.
- [CO(H2O)6 2+] represents the concentration of CO(H2O)6 2+ ions.
- [H2O] represents the concentration of H2O molecules.
- [Cl-] represents the concentration of chloride ions.
Note that the concentrations are written in square brackets to indicate their molar concentration.
Calculating the equilibrium constant (K) using the given concentrations of the species would allow you to determine the extent of the reaction and the position of equilibrium.