The hydroxide ion reacts with the H2PO2 ion according to the following equation:
OH^- + H2PO2^- > HPO2^-2 + H2
The rate law for this reaction rate is R=k[OH^-]^2[H2PO^-2]. What will be the change in the reaction rate if the H2PO2 ion concentration is doubled. What will the effect if the hydroxide ion concentration tripled?
If H2PO2 doubled, more HPO2 and H2 are made. It would be the same if hydroxides tripled as well.
I think you have given a "qualitative" answer. I think the questions wants a "quantitative" answer.
Look at the rate equation of
rate = k[OH^-]^2*[(H2PO2)^2-]
if OH is doubled then rate quadrupled because OH is squared.
If H2PO2^2- is tripled, rate is tripled because H2PO2^2- is to the first power.
If it was a qualitative question, how would the question above be reformatted to fit it?
Also, if H2PO2 is tripled, how does that correspond to H2PO, since they're both different compounds? I understand how doubling OH will quadruple it in the rate, I just don't understand how the other go hand in hand.
I would think something like this.
"The hydroxide ion reacts with the H2PO2 ion according to the following equation:
OH^- + H2PO2^- > HPO2^-2 + H2
What will be the change in the reaction rate if the H2PO2 ion concentration is increased. What will the effect if the hydroxide ion concentration is increased?"
All I've done is remove the rate equation completely and changed doubled and tripled to increased.