IONIC EQUILIBRIUM 🧪🧑🏻‍🔬

What are electrolyte

What are two types of electrolytes

Any substance which get dissociated into its ion in its solution is called electrolyte

2 type

1 strong electrolyte : 100 percent dissociation into ions

2 weak electrolyte : not 100 percent dissociation into ions

Background details for knowing why ionic equilibrium will be establish only by weak electrolyte

Strong electrolyte don't exist equilibrium

Cause reactants get over

Weak electrolyte reaction will not completel over reactants

Do equilibrium establish hence reversible reaction

It is involving ions so it is ionic equilibrium

Hence weak electrolyte will only establish ionic equilibrium

Ostwalds dilution law

Common ion effect

If a strong containing atleast one common ion is added to a solution of weak electrolyte then degree of weak electrolyte then degree of dissociation of weak electrolyte decreases

Approximations

Concentration of common ion at equilibrium to be considered coming only from strong electrolyte

Equilibrium concentration of weak electrolyte to be considered equal to its initial concentration

Now solve the given question

Just solve it 💅🏻 🫰🏻

Just solve it 💅🏻 🫰🏻

Ionic product of water (Kw)

Water is a very weak electrolyte

Water undergoes self ionisation

Kw is just like expression of eqm constant of dissociation water

At 25 degree celcius 10^-14

Pure water at 25 degree celcius ionizes into equals no. Of OH- AND H +

LIKE 1MOLECULE OF WATER WILL DISSOCIATE INTO 1 OH MINUS AND H PLUS

H PLUS IS OF ACIDIC NATURE AND OH MINUS IS OF BASIC NATURE HENCE PURE WATER US ALWAYS NEUTRAL

OH MINUS AND H PLUS CONCN LIKELY TO SAY ACTIVE MASS IS 10 TO THE POWER MINUS 7

pH scale

It is a way of representing molar concn oh H plus

Is solutions are always neutral on pH 7 ???

No solution are not neutral because of pH it is neutral when [OH-] = [H+]

14=pH +pOH (FOR ANY AQUEOUS SOLUTION SUM OF H AND OH IS ALWAYS EQUALS TO 14 AT 25 DEGREE CELCIUS)

Calculate pH of 0.01M HNO3 solution at 25 degree

Calculate pH of 0.05 M H2SO4 solution at 25 degree celcius

If some ion comes from two electrolyte and their concn difference is more than 10¹ then ignore smaller one

If concentration are equal or differ just by 10¹ then don't ignore any of the concentration

Calculate pH of 10-⁸bM HCl solution at 25 degree celcius

PKw equalsto minuslogKw

At any temperature concentration of proton in water is HPLUS EQUALS TO UNDER ROOT OF Kw

Calculate pH of 10^-12 M HCl solution at 25 degree celcius

Calculate the pH of 0.001M KOH. (aq) solution at 25 degree celcius

Option 2

Ionic product if water increases idpf

1 pressure is reduced

2 Hplus is added

3 OH minus is added

4 Temperature increases

Option 4

Calculate the pH of 0.001 KOH (aq) solution at 25 degree celcius

The ionic product if water is 10^-14. The Hplus ion concentration in o.o1 M NaOH. Solution is

And 10 to the power minus 12

The number of H plus ions in 1ml of a solution having pH equals to 13 is

Ans 6.023 × 10⁷

pOH of 0.002 M HNO3 is

Ans 11 plus log 2

The concentration of an acid is 10 –9 The pOH if the solution is

Ans almost 7

If pH. of solution of NaOH is 12.0 the pH of H2SO4 solution of same molarity will be

Ans 1.7

Answer 0.4g per litre

Calculate [H+] in a solution having pH 3.7

Calculate Hplus concentration in a beer having pH. 2.3

Pehle usko next integer me lao 3.7 ko jo ki milega 4 toh ab usko 10 ki power minus 4 kr de uske baad dekh ki kitna subtract krne par 4 me se 3.7 aayega aur woh hoga 0.3 auryeh aata hai log 2 ke wjh se toh ab answer hogya 2 into 10 to the power minus 4

pH calculation of weak acid and weak base

Calculate the pH of 0.01 NH4OH (Kb = 10–⁶) solution at 25 degree celcius

Answer 10

A solution of pH. 9.0 is 1000 times more basic as a solution The pH of this solution is

The pH of 1 M aqueous solution of a a weak acid HA is 6.0 It's dissociation constankt is

Answer 10-¹²

The concentration of a monoprotic acid is C moles per litre and ionisation constant ka The pH of the solution is

Calculate pH of 0.1 M NH4OH (aq) solution at 25 degree celcius

You may have forgot that NH4OH is a weak electrolyte😐🫡

Calculate pH of 0.1M NH4OH (aq) solution at 25degree celcius

(Ka(NH4+) = 10-⁹ )

You may have forgot that ka or kb is not the concentration it's is equilibrium constant

pH mixture idpf acids

Calculate pH of a solution obtained by mixing 1L of 0.01M HCl with 1L of 0.02 M NaOH solution

Answer 11.7

How many grams of caustic potach required to completely neutralise 12.6 g HNO3

Answer 11.2 g

Caustic potash is KOH.

At wt if K is 39

pH of mixture of weak acid

Calculate (HPLUS ) (HCOOMINUS) APand (OCN MINUS) in a solution that contains 0.1 M HCOOH (Ka equals to 2.4 into 10 to the minus 4 ) and 0.1 M ( Ka equals to 4 into 10 to the power minus four )

Answer

For H PLUS. 8 into 10to the power minus 3

3 into 10 to the power minus 3

5 to the power minus 3

You may have forgot when we add two reactions then their equilibrium constant get multiplied to give equilibrium constant of the resultant reaction

Salt hydrolysis

Reverse reaction of neutralisation is called salt hydrolysis

It is the breaking up of salt in presence to regenerate respective acid or base

Only acid or only base or both can be regenerated

Types of salts

Salts are of 4 types

Salt of strong acid and strong base

NaCl KNO3. Na2SO4

Salt of strong acid and weak base

NH4Cl (NH4)2SO4.

Salt of weak acid and strong base

NaCN CH3COONa

Salt of weak acid and weak base

CH3COONH4. NH4CN

Hydrolysis of salt of SA and SB

Eg NaCl

Na