I’ve been to my chemistry lecture and I wasn’t able to understand these key poin
ID: 711666 • Letter: I
Question
I’ve been to my chemistry lecture and I wasn’t able to understand these key points. Could anyone answer this set of questions explain their answer in their own words?
Please remember Chegg's 5 subsets per question policy, which means that you must go over all of these problems instead of answering only one. I’ve been to my chemistry lecture and I wasn’t able to understand these key points. Could anyone answer this set of questions explain their answer in their own words?
Please remember Chegg's 5 subsets per question policy, which means that you must go over all of these problems instead of answering only one. 6.) Give the equation for a supersaturated solution in comparing Q with Ksp. A) Q> Ksp C) Q = Ksp E) none 7.) Which of the following solutions is a good buffer system? A) A solution that is 0.10 M HC2H302 and 0.10 M LiC2H302 B) A solution that is 0.10 M HBr and 0.10 M KC2H302 C) A solution that is 0.10 M HI and 0.10 M NH4+ D) A solution that is 0.10 M NaOH and 0.10 M KOH E) None of the above are buffer systems.
Explanation / Answer
6)To find out the correct relation,we must understand the concept of ionic product Q.The ionic product (Q) of a salt is the product of the concentrations of the ions in solution raised to the same powers as in the solubility product expression.It is analogous to the reaction quotient (Q) used in Gas equilibrium Whereas Ksp describes equilibrium concentrations, the ion product describes concentrations that are not necessarily equilibrium concentrations.Now there are three possibilities possible are given below-
1)Q < Ksp. The solution is unsaturated, and more of the ionic solid, if available, will dissolve.
2)Q = Ksp. The solution is saturated and at equilibrium.
3)Q > Ksp. The solution is supersaturated, and ionic solid will precipitate.
From these above condition it is clear that option A is the right choice.
7) To act like a buffer solution,it must contain either an acid and its conjugate base OR a base with its conjugate acid.So,
A)Solution of 0.1M HC2H3O3 and 0.1 M NaC2H3O3=It will act like a buffer solution with HC2H3O3 being the acid and NaC2H3O3 being the conjugate base.
B)Solution of 0.1M HBr and 0.1M of KC2H3O3=No.It will not act like a buffer as there is no conjuagte base for HBr.
C)Solution of 0.1M HI and 0.1M NH4+=Again no.As there is no conjugate base for NH44+.(i.e; NH3)
D)Solution of 0.1M NaOH and 0.1M KOH=There is no question of it being a buffer solution as both are strong bases with OH-.There is no chance of forming a conjugate acid at all.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.