Mg(OH)2=Mg2 + 2OH-
a) which species would react with if an acid H+ is added to the mixture? my answer is the equation will shift to the right (product)
b) would this cause a deficit or excess? my answer is excess
c) what would you predict would be observed by adding the acid? i don't know with this one pls help?
d)in c above use lechatelier's principle to explain the observation.
pls i need help this is one of the postlab questions which is not related to the experiment were having.
I think you have not answered a correctly. The question doesn't ask in a which direction the reaction shifts; it asks which ion will react with H^+ if an acid is added. The answer is it will react with the OH^-.
b. Will this cause a deficit or excess OF WHAT? If they mean OH, it will cause a deficit since you will be using OH to react with the H^+.
c. More Mg(OH)2 solid will dissolve.
d. Le Chatlier's Principle, in simple words, says that a system in equilibrium will try to undo what we do to it. So if we add H^+, that reacts with OH decreasing the OH^-, the reaction will shift to the right to replace the OH^- we've removed, and that means more solid Mg(OH)2 will dissolve.
a) If an acid, H+, is added to the mixture, it would react with the hydroxide ions (OH-) present in Mg(OH)2. The equation would proceed towards the right (product side) to form water (H2O).
b) The addition of the acid, H+, would cause an excess of H+ ions. This is because by adding the acid, you are increasing the concentration of H+ ions in the mixture.
c) If acid is added to the mixture, you would observe that the solution becomes more acidic. There would be an increase in the concentration of H+ ions, leading to a decrease in the pH value of the solution.
d) Le Chatelier's principle can help explain the observation. According to this principle, if a stress (in this case, the addition of an acid) is applied to a system at equilibrium, the system will respond by shifting its equilibrium position in a way that minimizes the effect of the stress. In this case, the addition of acid causes an increase in the concentration of H+ ions. To counterbalance this increase and minimize the effect of the added acid, the equilibrium position of the reaction will shift to the right, resulting in more water formation. This shift would help lower the concentration of H+ ions and restore equilibrium. As a result, the solution becomes more acidic.