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The latest Messages 13
2022-03-30 15:19:09
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2022-03-01 11:45:13
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2022-03-01 08:43:20
" Workshop Session on 01 Mar at 01:00 PM
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2022-02-28 13:14:37
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2022-02-27 15:09:04
✯ ❥˙ ｡..... NCERT
Electrolytes: The substances that conduct electricity either in molten state or in their aqueous solutions are called electrolytes.
> Ionic Equilibrium : It is defined as the equilibrium established between the unionized molecules and the ions in a solution of weak electrolytes.
> Arrhenius Acid : It is the substance that dissociates in water to give hydrogen ions (H+).
> Arrhenius Base: It is the substance that dissociates in water to give hydroxyl ions (OH-).
> Bronsted - Lowry Acid : It is a substance that is capable of donating a proton (H+)
> Bronsted - Lowry Base : It is a substance that is capable of accepting a proton (H+)
> Conjugate Acid-Base Pair: The acid base-pair that differs only by one proton is called a conjugate acid-base pair.
➤ Lewis Acid : It is defined as a species which accepts electron pair
➤ Lewis Base: It is defined as a species which donates an electron pair.
> pH Scale: Hydronium ion concentration in molarity is more conveniently expressed on a logarithmic scale known as the pH scale.
> pH : The pH of a solution is defined as the negative logarithm to base 10 of the activity (a) of hydrogen ion. > Acid Ionization Constant: The equilibrium constant for acid ionization is called acid ionization constant.
> Base Ionization Constant: The equilibrium constant for base ionization is called base ionization constant
> Common Ion Effect: It can be defined as a shift in equilibrium on adding a substance that provides more of an ionic species already present in the dissociation equilibrium.
> Hydrolysis: The process of interaction between water and cations or anions or both of salts is called hydrolysis.
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2022-02-27 12:38:16
" Join Live Session at 6:00 PM and Give Yourself a new Direction
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2022-02-26 17:21:08
✯ ❥˙ ｡..... NCERT
Molarity of pure water =Density /Molar Mass
1000 g/L/18.0 g/mol
= 55.55 M
> We can distinguish acidic, neutral and basic aqueous solutions by the relative values of the H₂O+ and OH concentrations:-
Acidic [H₂O+]> [OH-]
Neutral [H20+] = [OH-]
Basic [H₂O+] <[OH-]
➤ pH range:-
(Acidic solution) (pH<7)
(Neutral solution) (pH = 7)
(Basic solution) (pH>7) ▃✧▃▃▃✧▃▃
┊ ┊ ┊ ┊ ┊ ┊
✿ ✿
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2022-02-26 14:17:25
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2022-02-25 13:17:52
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2022-02-25 12:09:36
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