KHC4H4O6(s)<-> K+ (aq)+ HC4H4O6-(aq)

Question

1) If the above reversible were started with only solid potassium hygrpden tartrate, which reaction would proceed faster, the "forward" or "reverse"?
I said forward
2) If the reactions were started with only the separated ions present, which would proceed faster?
I said reverse
3) if the reaction were equilibrium and a large amount K+ ion was added which reaction would proceed faster? As a result, what would happen to the amount of HC4H4O6-(aq) in solution ?
I said reverse and the result of HC4H4O6-(aq) will increase since K ion increase.

Answer 1

I agree with 1 and 2.

For 3, I agree with reverse, but a decrease in the....(aq) because it has to combine with the K to go in reverse.

Answer 2

Oh ok gotcha. Thank you again!!

Answer 3

You !welcome

Answer 4

This is kinda relate to this and I am trying to figure this out but I am stuck.
In procedure B2, you will titrate a saturated solution to find out how much of the anion dissolved. Assume you we're able to dissolve about 0.12g of potassium hydrogen tartrate in 25.0 mL of water. For the titration, you will use 10.00mL of this sample. How many mL of 0.0500M NaOH would required to bring the titration to its end point? Show your work.
I am not sure where to start