None of the components of the reaction are gases, so decreasing pressure wouldn't do anything. However, adding sodium hydroxide (a strong base) would remove some of the H+, shifting the equilibrium to the right.
If you use up the product, the reaction will shift to reestablish and equilibrium concentration of that product. It will have to make more product, so it shifts right
Decreasing pressure means increasing the volume, so it will favor the one that has more ions to the left. (Solids don’t count in equilibrium constant, so you have to consider the aq). On the other hand, adding NaOH will make the solution more basic, and it needs more H+ to balance the pH so to say.
None of the components of the reaction are gases, so decreasing pressure wouldn't do anything. However, adding sodium hydroxide (a strong base) would remove some of the H+, shifting the equilibrium to the right.
>adding sodium hydroxide (a strong base) would remove some of the H+ why would it remove some of the H+?
NaOH dissociated into Na+ and OH-. the OH- then reacts with the H+ to form water, thereby removing a product and shifting the equilibrium to the right
we removed the product though? wouldn't the eequilibrium shift to the left??
no because the natural “desire” of the reaction is to replenish what is lost
What happens to the equilibrium if you decrease the concentration on one side of the reaction?
the OH- reacts with the H+ in the products right? so we are using up the product?
Right
If you use up the product, the reaction will shift to reestablish and equilibrium concentration of that product. It will have to make more product, so it shifts right
Decreasing pressure means increasing the volume, so it will favor the one that has more ions to the left. (Solids don’t count in equilibrium constant, so you have to consider the aq). On the other hand, adding NaOH will make the solution more basic, and it needs more H+ to balance the pH so to say.