How to deduce Nature of Salt in Salt Hydrolysis
Chemistry Guru Podcast
A salt can be acidic, neutral or alkaline. We can deduce the nature of the salt from its constituent ions, namely: 1. ion formed from a weak acid will be a conjugate base, eg CH3COO- (from weak acid CH3COOH) 2. ion formed from a strong acid will be neutral, eg Cl- (from strong acid HCl) 3. ion formed from a weak base will be a conjugate acid, eg NH4+ (from weak base NH3) 4. ion formed from a strong base will be neutral, eg Na+ (from strong base NaOH) This can be summarised as shown: salt hydrolysis nature of ions summary Next we can move on to deduce the nature of a salt. Let's have some...
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Bronsted Acids and Bases: Types and Strength
Chemistry Guru Podcast
According to Bronsted-Lowry theory of acids and bases, - an acid is a proton, H3O+ or H+ donor - a base is a proton, H3O+ or H+ acceptor The strength of an acid or base is related to the extent of dissociation in solution: - a strong acid or base is fully dissociated - a weak acid or base is partially dissociated So therefore we will have 4 possible types of acids and bases: 1. Weak Acid 2. Strong Acid 3. Weak Base 4. Strong Base Also, each of these acids and bases will dissociate in solution to give different species. 1. Weak Acid Dissociation eg CH3COOH bronsted theory weak acid CH3COOH...
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Balance Redox Reaction via Half Eqn Method
Chemistry Guru Podcast
Balancing Redox Equations via the Half-Equation Method can be done via the following systematic steps. 1. Balance Redox Equation in Acidic Medium Let's have this reaction as an example: balance redox reaction using half equation method example We can determine which species is oxidised and reduced by comparing the oxidation number: - Oxidation state of manganese decreases from +7 to +4 hence MnO4- is reduced - Oxidation state of iodine increases from -1 to 0 hence I- is oxidised We can then write down the half equations for oxidation and reduction: balance redox reaction half equations Next we...
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How to draw Amino Acids and Proteins
Chemistry Guru Podcast
Learn how to by Maverick Puah the Chemistry Guru.
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Electrophilic Addition Mechanism for Alkenes
Chemistry Guru Podcast
Step-by-step tutorial to learn how to draw the of Alkene by Maverick Puah the Chemistry Guru. Do check out the following for more video lessons: If you are looking for H2 Chemistry Tuition, do consider taking up my .
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How to compare Basicity of Amines, Phenylamines and Amides
Chemistry Guru Podcast
Learn how to compare using Lewis Acid-Base Theory by Maverick Puah the Chemistry Guru Do check out the following for more video lessons: If you are looking for H2 Chemistry Tuition, do consider taking up my .
info_outlineAccording to Bronsted-Lowry theory of acids and bases,
- an acid is a proton, H3O+ or H+ donor
- a base is a proton, H3O+ or H+ acceptor
The strength of an acid or base is related to the extent of dissociation in solution:
- a strong acid or base is fully dissociated
- a weak acid or base is partially dissociated
So therefore we will have 4 possible types of acids and bases:
1. Weak Acid
2. Strong Acid
3. Weak Base
4. Strong Base
Also, each of these acids and bases will dissociate in solution to give different species.
1. Weak Acid Dissociation eg CH3COOH
bronsted theory weak acid CH3COOH dissociation
CH3COOH is a weak acid and dissociates partially in solution (as indicated with reversible arrow) to form H+ and CH3COO- ions.
Since this is a reversible process, CH3COO- can accept H+ to form back CH3COOH.
Therefore the nature of CH3COO- is basic and we call CH3COO- the conjugate base of CH3COOH.
2. Strong Acid Dissociation eg HCl
bronsted theory strong acid HCl dissociation
HCl is a strong acid and will dissociate fully (as indicated with full arrow) in solution to form H+ and Cl- ions.
Since this is an irreversible process, Cl- has no tendency to accept H+ and form back HCl.
Therefore the nature of Cl- is neutral.
3. Weak base dissociation eg NH3
bronsted theory weak base NH3 dissociation
NH3 is a weak base and dissociates partially in solution (as indicated with reversible arrow) to form OH- and NH4+ ions.
Since this is a reversible process, NH4+ can donate H+ to form back NH3.
Therefore the nature of NH4+ is acidic and we call NH4+ the conjugate acid of NH3.
4. Strong base dissociation eg NaOH
bronsted theory strong base NaOH dissociation
NaOH is a strong base and will dissociate fully (as indicated with full arrow) in solution to form OH- and Na+ ions.
Since this is an irreversible process, Na+ has no tendency to donate H+ and form back NaOH.
Therefore the nature of Na+ is neutral.
So in summary:
- weak acid will dissociate to give conjugate base
- weak base will dissociate to give conjugate acid
- strong acid will dissociate to give a neutral ion
- strong base will dissociate to give a neutral ion
bronsted theory dissociation summary
These concepts are fundamental and very important in Ionic Equilibria.
Check out this video lesson to learn more about acids and bases and their dissociation in solution!
Topic: Ionic Equilibria, Physical Chemistry, JC, H2, A Level Chemistry, Singapore
You can also view this video lesson with screenshots and detailed explanation.
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