A 1.00 liter solution contains 0.40 M ammonia and 0.52 M ammonium iodide . If 0.
ID: 522172 • Letter: A
Question
A 1.00 liter solution contains 0.40 M ammonia and 0.52 M ammonium iodide.
If 0.260 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false.
(Assume that the volume does not change upon the addition of potassium hydroxide.)
_______TrueFalse A. The number of moles of NH3 will remain the same.
_______TrueFalse B. The number of moles of NH4+ will remain the same.
_______TrueFalse C. The equilibrium concentration of H3O+ will decrease.
_______TrueFalse D. The pH will increase.
_______TrueFalse E. The ratio of [NH3] / [NH4+] will remain the same.
Explanation / Answer
Answer:-
Volume of the buffer = 1.00 L
[NH3] = 0.40 M , [NH4I] = 0.52 M
0.260 moles of KOH are added.
After addition of the KOH the following reaction will take place,
NH4+ + OH- ---------> NH3 + H2O
So, from the equation it is evident that the number of moles of NH3 will increase and the number of moles of NH4I will decrease. KOH is a strong base , so the pH of the buffer will increase and the concentration of H3O+ will decrease.
So.
False A. The number of moles of NH3 will remain the same.
False B. The number of moles of NH4+ will remain the same.
True C. The equilibrium concentration of H3O+ will decrease.
True D. The pH will increase.
False E. The ratio of [NH3] / [NH4+] will remain the same.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.