Asked by Trixie
Calculate the initial molarity of KNH2 and the molarities of K+, NH3, OH-, and H3O+ in an aqueous solution that contains 0.75 g of KNH2 in 0.255 L of solution. You may ignore the reaction of NH3 with water.
I already found the initial molarity, but I am not sure how to find each species concentration with the information given. Please explain how to solve rather than give me only answers--they are helpful to compare but I want to learn how to do this. Thanks!
I already found the initial molarity, but I am not sure how to find each species concentration with the information given. Please explain how to solve rather than give me only answers--they are helpful to compare but I want to learn how to do this. Thanks!
Answers
Answered by
DrBob222
NH2^- + HOH ==> NH3 + OH^-
Set up ICE chart with NH3 = x and OH^- = x so NH2^- = your molarity -x
Solve for x.
Kb = (Kw/Ka) = (NH3)(OH^-)/(NH2^-)
That gives you NH3, OH, you have NH2^- and K^+ is same as NH2^-.
Set up ICE chart with NH3 = x and OH^- = x so NH2^- = your molarity -x
Solve for x.
Kb = (Kw/Ka) = (NH3)(OH^-)/(NH2^-)
That gives you NH3, OH, you have NH2^- and K^+ is same as NH2^-.
Answered by
Blake
This could be a dumb question but how do you find Kb here in order to solve for x?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.