# Difference of OH- in Strong vs Weak Bases

• clavin
In summary, the conversation discusses the difference in dissociation between a strong base and a weak base, specifically in the reactions of ch3cooh + oh- and ch3cooNa. The speaker's book states that the reactions will go to completion, but the speaker questions this due to the weak acid nature of acetic acid. The expert summarizes that all OH- are identical and that Na+ does not come from an acid, and therefore the dissociation of Na+ should not affect that of ch3coo-.
clavin
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-

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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## 1. What is the difference between a strong base and a weak base?

A strong base is a substance that completely dissociates in water, releasing a high concentration of hydroxide ions (OH-). A weak base, on the other hand, only partially dissociates in water, resulting in a lower concentration of hydroxide ions.

## 2. How do strong bases and weak bases affect the pH of a solution?

Strong bases have a higher concentration of hydroxide ions, which can neutralize a higher amount of hydrogen ions (H+) in a solution. This results in a higher pH, making the solution more basic. Weak bases, with their lower concentration of hydroxide ions, have a smaller effect on the pH of a solution.

## 3. Can you give examples of strong bases and weak bases?

Some common examples of strong bases include sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)2). Examples of weak bases include ammonia (NH3), ammonium hydroxide (NH4OH), and acetate (CH3COO-).

## 4. How do the chemical structures of strong and weak bases differ?

Strong bases typically have larger, more complex chemical structures compared to weak bases. This is because strong bases have a higher affinity for hydroxide ions, which requires a stronger bond between the base and the hydroxide ion.

## 5. What are the implications of using strong vs weak bases in different experiments or applications?

Strong bases are often used in experiments or applications where a high pH or basic environment is desired. This could include processes such as soapmaking or water treatment. Weak bases, with their milder effects on pH, may be used in applications where a more subtle or controlled change in pH is needed, such as in some types of chemical reactions or as a buffering agent in solutions.

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