Stock solutionFeCl Stock Solution KSCN Stock Solution AgNO KSCN s Stock Solution
ID: 549225 • Letter: S
Question
Stock solutionFeCl Stock Solution KSCN Stock Solution AgNO KSCN s Stock Solution AgNOs FeCls p 1. What is e the evidence for a shift in equilibrium when iron(ll) chloride is added to the stock solution? for a shift in equilibrium when potassium thiocyanate is added What is the evidence to the stock solution? 2. 3. What is the evidence for a shift in equilibrium when silver nitrate is added to the stock solution? (The formation of a precipitate is not the evidence since the precipitate is not one of the substances in the equilibrium) a. The change in concentration of which ion in the equilibrium caused this equilibrium shift? b. Write a net ionic equation to illustrate how this concentration change occurred .Explanation / Answer
Answer:
1. The equilibrium moves to the right side. The intensity of the blood red color increases.
2. The equilibrium moves to the right side. The intensity of the blood red color increases.
3.a. Because it reacts with chlorides ions and forms FeCl3. It will not disturb the ions in the equilibrium reaction
b. Actually the equilibrium moves towards the left and decreases the color of the blood red color and forms silver thiocyanate
4. The net ionic equation: Ag^+1 (aq) + SCN^-1 (aq) <<<>>>AgSCN (s) white precipitate