Question

CAN SOMEONE PLEASE HELP ME WITH A LAB !!!! I WILL FAN, FOLLOW, MEDAL, AND EVERYTHING !!!! I PROMISE

Answer 1

@nincompoop @adilalvi @study100 @satellite73

Answer 2

@aaronq

Answer 3

@Preetha @mayankdevnani

Answer 4

please????

Answer 5

let me break it down how do i do this?
Background
Cobalt(II) does not exist in aqueous solution as a free ion, such as Co2+, but forms a complex ion where 6 water molecules attach to it. This results in the pink complex ion Co(H2O)6+2. In the presence of Cl- ions, a different complex forms, the blue CoCl4-2 complex ion. We can use their different colors to indicate the equilibrium concentrations for the following reaction:

In this simulation you not only observe the equilibrium concentrations through their colors, but also directly read their concentrations (in the Solution Info panel on the right).

Predictions /4
You will make a number of predictions before doing the investigation yourself. At the end we will revisit the predictions to see if you (and Le Chatelier!) were correct. Highlight or underline your answer, either Reactants or Products.
1.) Which direction will the system shift if HCl is added? Reactants or Products
2.) Which direction will the system shift if the solution is diluted? Reactants or Products
3.) Which direction will the system shift if AgNO3 is added? Reactants or Products
Hint: You may need to consult your Table of Solubilities.
4.) Will the Keq value change as a result of the above changes?

Answer 6

this is the reaction Co(H2O)6+2(aq) + 4Cl-(aq) CoCl4-2 (aq) + 6H2O(l)
pink blue

Answer 7

1.) Which direction will the system shift if HCl is added? Products
2.) Which direction will the system shift if the solution is diluted? no change pure liquids or solids are not included in the equilibrium
3.) Which direction will the system shift if AgNO3 is added? Reactants
Hint: You may need to consult your Table of Solubilities.
Will precipitate AgCl
4.) Will the Keq value change as a result of the above changes? NO

Answer 8

@cuanchi is right but i think his answer to question #2 is incorrect. i think system shift to reactants when solution diluted.

Answer 9

am i right @nincompoop ?

Answer 10

@Luigi0210 what do you think?

Answer 11

@chmvijay what do you think?

Answer 12

I agree, water is on the right side (products) of the equation. adding more water will shift it to the reactant's side.

Answer 13

I am sorry, I think that the question is not correctly formulated since doesn't give the option of the reaction don't move in either direction. Besides that it is a common mistake in the students to include solids X(s) o pure liquids X(l) in the expression of the equilibrium constant. If we talk about concentrations of reactants or products I will totally agree that is going to change, but the reaction is not going to produce more moles of reactants when you add more water. Notice that in the formula the water has an (l) that means pure water and its concentration doesn't change if you add more water. The other three components of the reaction as a (aq) that indicates that the reaction is in aqueous media. It is the same reason that you don't include the water concentration when you describe the Kw = [H+][OH-]. I attached a page of the book where Nivaldo Tro explain why pure solids and liquids are not include in the equilibrium constant expression.
In turn if the reaction were in an alcoholic media and the water is a product of the reaction in the alcoholic solution in that case the water will be consider a product of the reaction and the concentration will change if we add more water (because the solvent of the reaction is alcohol) and you will be adding water.
Co(H2O)6+2(aq) + 4Cl-(aq) CoCl4-2 (aq) + 6H2O(l)

When we talk about what direction the reaction is moving we refer at the change of the total amount (mass) of reactant or products not to the change in the concentration, but as in the general model most the reactions that we consider for study we mention that we increase the amount of one of the reactants or product without changing the volume of the solution we implicitly do the correlation of change of mass as a change of concentration (that in this case is correct because there is not change in volume).
When you latter study the shift of equilibrium in a buffer system you will see that the pH of the buffer is not changing when you add water but it change lightly if you add acid or base.