Comparing Strengths of Bases: OH- vs. Forming OH- in Water

  • Thread starter Thread starter HelloMotto
  • Start date Start date
  • Tags Tags
    Base
Click For Summary
SUMMARY

The discussion compares the strengths of two groups of bases: those that contain hydroxide ions (OH-) like sodium hydroxide (NaOH) and those that generate hydroxide ions in water, such as ammonia (NH3). It is established that metal hydroxides like NaOH and potassium hydroxide (KOH) ionize completely in water, making them strong bases. In contrast, ammonia undergoes hydrolysis to form ammonium hydroxide, which only partially ionizes, categorizing it as a weaker base. The extent of ionization is crucial in determining the strength of these bases.

PREREQUISITES
  • Understanding of acid-base chemistry
  • Knowledge of ionization and hydrolysis processes
  • Familiarity with strong and weak bases
  • Basic concepts of conductivity in aqueous solutions
NEXT STEPS
  • Research the ionization constants of common bases like NaOH and KOH
  • Learn about the hydrolysis of ammonia and its equilibrium
  • Explore the concept of pH and its relation to base strength
  • Investigate the conductivity of strong vs. weak bases in solution
USEFUL FOR

Chemistry students, educators, and anyone interested in understanding the comparative strengths of bases in aqueous solutions.

HelloMotto
Messages
73
Reaction score
0

Homework Statement


There are two groups of bases, one that contains OH- (example : NaOH), and one that forces water to form OH- (example: NH3). Which of these are the stronger bases? Which are the weaker bases? Why?


Ok so our class just started learning about acids and bases. I've read the pages on the textbook regarding bases and i can't seem to find the answer or any kind of evidence.
Could somebody give me a hint on this question please?:blushing:
is it related to conductivity?
 
Physics news on Phys.org
A base renders hydroxide ion in water (assuming solutions in water as the solvent). Metal hydroxides such as of potassium or sodium (or cesium ? ) ionize in order to supply the hydroxide; at least for sodium and potassium hydroxides, the compounds ionize in water to great extent. Something like ammonia must HYDROLYZE with water to render ammonium hydroxide. Then the ammonium hydroxide will ionize.

Maybe there is another way to describe that with ammonia. Ammonia, a base, reacts with water, which behaving as an acid. The result is ammonium hdroxide, which now can ionize in water. This makes me wonder, how thoroughly does the ammonia react with the water as a neutralization reaction? Is dissolved ammonia present more as ammonia or more as ammonium hydroxide?
 
So the amount of ionization of the compound should give you a clue.
Have you searched the internet for more information?
Here are a couple or references found using key words "strong base" "weak base"

ref1
ref2
 

Similar threads

Chemistry How to take into account autoprotolysis in weak base solution?
  • · Replies 8 ·
Replies
8
Views
3K
Chemistry Understanding how to calculate pH of a buffer solution
  • · Replies 2 ·
Replies
2
Views
2K
Chemistry Are there typos in this snippet causing confusion?
  • · Replies 2 ·
Replies
2
Views
2K
Chemistry Comparing methods of computing pH at equivalence point in titration
  • · Replies 4 ·
Replies
4
Views
2K
Weak bases react with water to produce strong base?
  • · Replies 6 ·
Replies
6
Views
2K
Determine the amount of NaOH and Sr(OH)2 based on pOH
  • · Replies 3 ·
Replies
3
Views
3K
How Do You Calculate pH and [OH-] for a Mixed NH3 and NH4Cl Solution?
  • · Replies 1 ·
Replies
1
Views
2K
Chemistry Why Does Grignard Addition to Esters Form Ketones?
  • · Replies 5 ·
Replies
5
Views
2K
Why Do Bases Release All Hydroxides Simultaneously?
  • · Replies 3 ·
Replies
3
Views
2K
Ionization vs. Dissociation for acids & bases
  • · Replies 6 ·
Replies
6
Views
19K