Difference of OH- in Strong vs Weak Bases

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SUMMARY

The discussion clarifies the differences in hydroxide ion (OH-) behavior between strong and weak bases. It establishes that while all OH- ions are chemically identical, their effects in reactions can differ based on the strength of the accompanying acid or base. The reaction of acetic acid (CH3COOH) with OH- is noted to proceed to completion, despite acetic acid being a weak acid, due to the nature of the reaction dynamics and approximations in chemical behavior. Additionally, the dissociation of sodium acetate (CH3COONa) is highlighted as complete, emphasizing the role of strong bases in driving reactions to completion.

PREREQUISITES
  • Understanding of acid-base chemistry, specifically the concepts of strong and weak acids and bases.
  • Familiarity with chemical reaction dynamics and equilibrium.
  • Knowledge of dissociation and hydrolysis in aqueous solutions.
  • Ability to correctly write and interpret chemical formulas.
NEXT STEPS
  • Research the principles of acid-base equilibrium and how they apply to weak acids like acetic acid.
  • Learn about the concept of hydrolysis and its effects on weak acids in solution.
  • Study the dissociation constants (Ka and Kb) for various acids and bases to understand their strengths.
  • Examine the role of ionic compounds in solution, particularly focusing on sodium ions (Na+) and their interactions.
USEFUL FOR

Chemistry students, educators, and professionals interested in acid-base reactions, particularly those studying organic chemistry and reaction mechanisms.

clavin
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is there any difference in oh- from a strong base than from a weak base apart from concentration?
second
lets say we have this reaction
ch3cooh + oh- => ch3coo- + h2o
in this reaction my book says the reaction will go to completion
but isn't acetic acid a weak acid. so shouldn't the disassociation should be partial
therefore why does the reaction go to completion?
also one more example
ch3cooNa=> ch3coo- + Na+
here again the disassociation is full
as Na+ comes from a strong acid
so why the dissociation extent of Na affect that of ch3coo-
 
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All OH- are identcial, and indistinguishable.

No such thing as ch3cooh - please write formulas correctly.

Neutralized acetic acid slightly hydrolizes, so stating that the reaction goes to completion is an aproximation - but a good one.

Na+ doesn't come from an acid. I have no idea what you are asking about.

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