Acid-Base solutions and their effectiveness for deprotonation of NH4+

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SUMMARY

The discussion centers on the effectiveness of various acid-base solutions for the deprotonation of NH4+. The solutions analyzed include 0.1 M A (pH 6.85), 0.1 M B (pH 7.22), 0.1 M C (pH 8.34), and 0.1 M D (pH 11.88). It is concluded that solution D, with the highest pH, is the most effective for deprotonating NH4+ due to its status as the strongest base among the options provided. Participants clarified that NH4+ is a weak acid, and the reaction's effectiveness is determined by the strength of the base used.

PREREQUISITES
  • Understanding of acid-base chemistry, specifically the concepts of pH and pKa.
  • Knowledge of the dissociation of weak acids and their conjugate bases.
  • Familiarity with the relationship between pH and basicity in aqueous solutions.
  • Basic principles of equilibrium constants (K) in acid-base reactions.
NEXT STEPS
  • Study the concept of pKa and its relevance to acid-base strength.
  • Learn about the dissociation constants of common weak acids and their conjugate bases.
  • Research the role of pH in determining the effectiveness of acid-base reactions.
  • Explore the relationship between strong acids and strong bases in chemical reactions.
USEFUL FOR

Chemistry students, educators, and professionals in fields related to chemical analysis and reaction mechanisms will benefit from this discussion, particularly those focused on acid-base equilibria and deprotonation processes.

ada0713
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Consider the following solutions and their respective pH values. Which substance would be effective(K>1) for the deprotonation of NH4+ ?
0.1 M A, pH = 6.85
0.1 M B, pH = 7.22
0.1 M C, pH = 8.34
0.1 M D, pH = 11.88

1) A
2) B
3) C
4) D
5) none are effective

If the reaction to be effective
doesn't Strong acid have to react with strong base?
since NH4+ is strong acid, I thought it should react with the strongest
base among the four substances,
so i chose D, which has the highest pH value.

Is it right, or am I doing something wrong here?
 
Last edited:
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oh.. NH4+ is not a strong acid..
how do I approach this problem then?

If K>1, net direction is right,
then shouldn't the reactants be stonger acid and stronger base?
 
Last edited:
anyone?
 
Dissociation of ammonium as an acid is weak; I would guess the choice D is the strongest base allowed for you and that would be most effective in deprotonating the ammonium ion. I say it is the strongest base there because all of your choices are 0.1 Molar; and D has the highest pH (therefore most alkaline).
 
i thought NH4+ would be a strong acid. NH3 is a weak base, it's conjugate acid, NH4+ should then be strong.

but you still need the strongest base... therefore D
 
ada0713 said:
Consider the following solutions and their respective pH values. Which substance would be effective(K>1) for the deprotonation of NH4+ ?
0.1 M A, pH = 6.85
0.1 M B, pH = 7.22
0.1 M C, pH = 8.34
0.1 M D, pH = 11.88

1) A
2) B
3) C
4) D
5) none are effective

If the reaction to be effective
doesn't Strong acid have to react with strong base?
since NH4+ is strong acid, I thought it should react with the strongest
base among the four substances,
so i chose D, which has the highest pH value.

Is it right, or am I doing something wrong here?

Why do you think you were given the pH at a particular concentration? Have you studied the concept of pKa? What 'K' was referred to in the question "...(K>1)..."?
 

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