I'm doing a lab for Le Chatelier's Principle. I'm concerned that all my answers sound very similar. Can someone help me and let me know if my answers are making sense?

~Thanks

1.) How is the reaction Zn(OH)2 <=> Zn^+2 + 2OH- affected by adding OH-

I think since we are adding a reactant the reaction favors products. So it shifts towards the left.

2.) How does an increase in H^+ effects the reaction H2) <=> (H^+) + OH^-

I think increasing the reactants favors the products. So it shifts towards the left.

3.) How does an increase in OH^- effect reaction Zn+2 + 4OH^- <=> Zn(OH)4^-2

I think increasing the reactants favors the products. So it shifts towards the right.

4.) Based on the last question #3 what does your answer from that question do to this reaction. Zn(OH)2 <=> Zn^+2 + 2OH^-

I think the effect would be the reverse because increasing the product OH^- in this equation would favor the products which would result in a shift to the left.

5.) How does an increase in (NH3) effect the reaction Zn^+2 + 4NH3 <=> Zn(NH3)4^+2

I think increasing the reactants favors the products. So it shifts towards the right.

a. Adding OH increase the products, so the reaaction will try to undo that and move to the left.

b. adding H+ increases the prducts, so the reacation will try to undo that and move to the left.
c. shifts to the right to undo the adding of the OH
d. shifts to left to reduce the OH added.
e. shifts to right to undo the increase in ammonia.

It seems like most of your answers are in the right direction, but there are a couple of clarifications and corrections that can be made. Le Chatelier's Principle helps us understand how a system at equilibrium will respond to changes in concentration, pressure, or temperature. Let's go through each question and analyze the answers:

1.) How is the reaction Zn(OH)2 <=> Zn^+2 + 2OH- affected by adding OH-?

Your answer states that adding a reactant (OH-) will favor the products and shift the reaction towards the left. However, in this case, OH- is a product in the forward reaction and a reactant in the reverse reaction. When you add OH-, it will react with Zn^+2 to form more Zn(OH)2, ultimately shifting the reaction towards the right (products).

2.) How does an increase in H^+ affect the reaction H2O <=> H^+ + OH-?

You've mentioned that increasing the reactants favors the products and shifts the reaction towards the left. However, in this reaction, H^+ and OH- are always present in water. An increase in H^+ (acidic conditions) or OH- (basic conditions) will disrupt the balance of the reaction and shift it to either side depending on which compound is increased. So, an increase in H^+ would favor the products (H^+ and OH-), shifting the reaction towards the right.

3.) How does an increase in OH- affect the reaction Zn+2 + 4OH- <=> Zn(OH)4^-2?

Here, you correctly state that increasing the reactant concentration favors the products and will shift the reaction towards the right. Therefore, your answer is accurate.

4.) Based on the previous question (#3), what does your answer from that question do to this reaction Zn(OH)2 <=> Zn^+2 + 2OH^-?

Your answer suggests that the reverse effect occurs, meaning an increase in OH- reduces the amount of OH- in the reaction and shifts it to the left. However, this contradicts the previous question's understanding that increasing OH- favors the products and shifts the reaction to the right. So, an increase in OH- would actually favor the products and shift the reaction towards the right.

5.) How does an increase in (NH3) affect the reaction Zn^+2 + 4NH3 <=> Zn(NH3)4^+2?

You've mentioned that increasing the reactants favors the products and shifts the reaction towards the right. Once again, your answer is correct. Increasing the concentration of NH3 will shift the reaction towards the right, favoring the formation of Zn(NH3)4^+2.

Overall, it appears that most of your answers are making sense, but there are a few minor corrections needed. Remember, in each case, it's essential to consider whether the reactant or product concentration is being increased and how that will impact the equilibrium.