KHC4H4O6(s)<-> K+ (aq)+ HC4H4O6-(aq)
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.
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.
Oh ok gotcha. Thank you again!!
You !welcome
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
1) If the reaction is started with only solid potassium hydrogen tartrate (KHC4H4O6), the forward reaction would proceed faster. This is because there are more reactant particles (solid) available for the forward reaction, compared to the reverse reaction involving ions in solution. The forward reaction requires the solid potassium hydrogen tartrate to dissolve and produce ions in solution, which may take some time.
2) If the reactions were started with only the separated ions (K+ and HC4H4O6-) present, the reverse reaction would proceed faster. When the ions are already separated in solution, they can come into contact more easily and quickly react with each other. The reverse reaction involves the recombination of the separated ions to form the solid potassium hydrogen tartrate.
3) If the reaction is at equilibrium and a large amount of K+ ion is added, the reverse reaction would proceed faster. Adding more K+ ions as a product of the forward reaction disturbs the equilibrium balance. According to Le Chatelier's principle, the system will try to counteract this disturbance by shifting the equilibrium in the direction that reduces the concentration of K+ ions. As a result of the reverse reaction being favored, the amount of HC4H4O6-(aq) in solution would increase because it is being converted into solid potassium hydrogen tartrate.