1️⃣ #THERMODYNAMICS
✔️ Branch of chemistry dealing with energy changes
✔️ Studies relation between heat, work & energy
✔️ Does NOT tell rate or mechanism of reaction
2️⃣ #THERMODYNAMICSYSTEM
✔️ Part of universe under study
📌 Types:
✔️ Open system → exchanges mass + energy
✔️ Closed system → exchanges only energy
✔️ Isolated system → no exchange
3️⃣ #SURROUNDINGS
✔️ Rest of universe except system
📌 Universe = System + Surroundings
4️⃣ #STATEFUNCTION
✔️ Depends only on initial & final state
✔️ Path independent
📌 Examples:
✔️ Internal energy (U)
✔️ Enthalpy (H)
✔️ Entropy (S)
5️⃣ #PATHFUNCTION
✔️ Depends on path followed
📌 Examples:
✔️ Heat (q)
✔️ Work (w)
6️⃣ #ZEROTHLAWOFTHERMODYNAMICS
✔️ If A is in thermal equilibrium with B
✔️ And B is in thermal equilibrium with C
✔️ Then A is also in thermal equilibrium with C
📌 Basis of temperature measurement
7️⃣ #FIRSTLAWOFTHERMODYNAMICS (VERY IMP )
✔️ Law of conservation of energy
✔️ Energy cannot be created or destroyed
📌 Mathematical form:
ΔU = q + w
✔️ ΔU = change in internal energy
✔️ q = heat absorbed by system
✔️ w = work done on system
8️⃣ #SIGNCONVENTION (NEET ⚠️)
✔️ Heat absorbed → q = +ve
✔️ Heat released → q = –ve
✔️ Work done on system → w = +ve
✔️ Work done by system → w = –ve
9️⃣ #WORKDONEINGASEXPANSION
✔️ w = –PΔV
📌 Expansion (ΔV +ve) → w –ve
📌 Compression (ΔV –ve) → w +ve
🔟 #SPECIALCASES
✔️ At constant volume
w = 0
ΔU = q
✔️ At constant pressure
qₚ = ΔH
1️⃣1️⃣ #ENTHALPY
✔️ Heat content of system
✔️ H = U + PV
📌 Change in enthalpy:
ΔH = ΔU + Δ(PV)
1️⃣2️⃣ #SECONDLAWOFTHERMODYNAMICS
✔️ Natural processes occur in direction of increase in entropy
✔️ Total entropy of universe always increases
📌 ΔS(universe) > 0 → spontaneous
📌 ΔS(universe) = 0 → equilibrium
1️⃣3️⃣ #ENTROPY
✔️ Measure of randomness or disorder
✔️ Higher disorder → higher entropy
📌 Solid < Liquid < Gas
1️⃣4️⃣ #GIBBSFREEENERGY ( IMPORTANT )
✔️ G = H – TS
📌 Change in Gibbs energy:
ΔG = ΔH – TΔS
✔️ ΔG < 0 → spontaneous
✔️ ΔG = 0 → equilibrium
✔️ ΔG > 0 → non-spontaneous
1️⃣5️⃣ #THIRDLAWOFTHERMODYNAMICS
✔️ Entropy of perfectly crystalline solid at 0 K is zero
📌 S = 0 at 0 K
1️⃣6️⃣ #NEETONELINERS
✔️ Internal energy is state function
✔️ Heat & work are path functions
✔️ First law is special case of energy conservation
✔️ Entropy predicts spontaneity
✔️ Gibbs energy decides feasibility
@Ayano1me @Neetugpoll @Neetugquiz
✔️ Branch of chemistry dealing with energy changes
✔️ Studies relation between heat, work & energy
✔️ Does NOT tell rate or mechanism of reaction
2️⃣ #THERMODYNAMICSYSTEM
✔️ Part of universe under study
📌 Types:
✔️ Open system → exchanges mass + energy
✔️ Closed system → exchanges only energy
✔️ Isolated system → no exchange
3️⃣ #SURROUNDINGS
✔️ Rest of universe except system
📌 Universe = System + Surroundings
4️⃣ #STATEFUNCTION
✔️ Depends only on initial & final state
✔️ Path independent
📌 Examples:
✔️ Internal energy (U)
✔️ Enthalpy (H)
✔️ Entropy (S)
5️⃣ #PATHFUNCTION
✔️ Depends on path followed
📌 Examples:
✔️ Heat (q)
✔️ Work (w)
6️⃣ #ZEROTHLAWOFTHERMODYNAMICS
✔️ If A is in thermal equilibrium with B
✔️ And B is in thermal equilibrium with C
✔️ Then A is also in thermal equilibrium with C
📌 Basis of temperature measurement
7️⃣ #FIRSTLAWOFTHERMODYNAMICS (VERY IMP )
✔️ Law of conservation of energy
✔️ Energy cannot be created or destroyed
📌 Mathematical form:
ΔU = q + w
✔️ ΔU = change in internal energy
✔️ q = heat absorbed by system
✔️ w = work done on system
8️⃣ #SIGNCONVENTION (NEET ⚠️)
✔️ Heat absorbed → q = +ve
✔️ Heat released → q = –ve
✔️ Work done on system → w = +ve
✔️ Work done by system → w = –ve
9️⃣ #WORKDONEINGASEXPANSION
✔️ w = –PΔV
📌 Expansion (ΔV +ve) → w –ve
📌 Compression (ΔV –ve) → w +ve
🔟 #SPECIALCASES
✔️ At constant volume
w = 0
ΔU = q
✔️ At constant pressure
qₚ = ΔH
1️⃣1️⃣ #ENTHALPY
✔️ Heat content of system
✔️ H = U + PV
📌 Change in enthalpy:
ΔH = ΔU + Δ(PV)
1️⃣2️⃣ #SECONDLAWOFTHERMODYNAMICS
✔️ Natural processes occur in direction of increase in entropy
✔️ Total entropy of universe always increases
📌 ΔS(universe) > 0 → spontaneous
📌 ΔS(universe) = 0 → equilibrium
1️⃣3️⃣ #ENTROPY
✔️ Measure of randomness or disorder
✔️ Higher disorder → higher entropy
📌 Solid < Liquid < Gas
1️⃣4️⃣ #GIBBSFREEENERGY ( IMPORTANT )
✔️ G = H – TS
📌 Change in Gibbs energy:
ΔG = ΔH – TΔS
✔️ ΔG < 0 → spontaneous
✔️ ΔG = 0 → equilibrium
✔️ ΔG > 0 → non-spontaneous
1️⃣5️⃣ #THIRDLAWOFTHERMODYNAMICS
✔️ Entropy of perfectly crystalline solid at 0 K is zero
📌 S = 0 at 0 K
1️⃣6️⃣ #NEETONELINERS
✔️ Internal energy is state function
✔️ Heat & work are path functions
✔️ First law is special case of energy conservation
✔️ Entropy predicts spontaneity
✔️ Gibbs energy decides feasibility
@Ayano1me @Neetugpoll @Neetugquiz
🔥2❤1🕊1🏆1
Q1. Zeroth Law
Assertion (A): If two systems are separately in thermal equilibrium with a third system, they are in thermal equilibrium with each other.
Reason (R): All systems in thermal equilibrium have the same temperature.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true
Q2. First Law
Assertion (A): Internal energy of an isolated system remains constant.
Reason (R): Energy can neither be created nor destroyed, only converted from one form to another.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true
Q3. Second Law
Assertion (A): Heat cannot spontaneously flow from a colder body to a hotter body.
Reason (R): Total entropy of an isolated system always increases for a spontaneous process.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true
Q4. Third Law
Assertion (A): Entropy of a perfectly crystalline substance is zero at absolute zero temperature.
Reason (R): At absolute zero, only one microstate is possible.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true
🤩3❤1🐳1
Chemistry booster series
⭐ 𝗖𝗜𝗘 𝗪EE (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 — 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 (𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞 𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲 ⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧…
Join kr lena all bcz in sbke full lec + crash course+ handwriting notes +short notes + test All in one milega
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1️⃣ #GIBBSFREEENERGY
✔️ Thermodynamic state function
✔️ Determines spontaneity of process
✔️ Denoted by G
📌 Relation:
G = H − TS
2️⃣ #TERMSINFORMULA
✔️ H → Enthalpy
✔️ T → Absolute temperature (K)
✔️ S → Entropy
📌 Unit of G → Joule
3️⃣ #CHANGEINGIBBSENERGY
📌 Formula:
ΔG = ΔH − TΔS
✔️ Applies at constant T & P
4️⃣ #SIGNIFICANCEOFΔG (VERY IMP )
✔️ ΔG < 0 → Spontaneous process
✔️ ΔG = 0 → Equilibrium
✔️ ΔG > 0 → Non-spontaneous
5️⃣ #CASESBASEDONΔHANDΔS
✔️ ΔH < 0 and ΔS > 0
Process spontaneous at all temperatures
✔️ ΔH > 0 and ΔS < 0
Process non-spontaneous at all temperatures
✔️ ΔH < 0 and ΔS < 0
Spontaneous at low temperature
✔️ ΔH > 0 and ΔS > 0
Spontaneous at high temperature
6️⃣ #TEMPERATUREEFFECT
✔️ Increase in T increases importance of entropy term
✔️ TΔS dominates at high temperature
7️⃣ #GIBBSENERGYATEQUILIBRIUM
✔️ At equilibrium:
ΔG = 0
📌 Relation with equilibrium constant:
ΔG° = −RT ln K
8️⃣ #STANDARDGIBBSFREEENERGY
✔️ Measured at:
✔️ 1 bar pressure
✔️ 298 K temperature
📌 Formula:
ΔG° = ΔH° − TΔS°
9️⃣ #REACTIONQUOTIENTRELATION
📌 Formula:
ΔG = ΔG° + RT ln Q
✔️ Q = reaction quotient
📌 At equilibrium Q = K
🔟 #MAXIMUMWORKCONCEPT
✔️ ΔG gives maximum non-expansion work
✔️ Useful in electrochemistry
📌 Electrical work = −ΔG
1️⃣1️⃣ #GIBBSENERGYINELECTROCHEMISTRY
📌 Relation:
ΔG° = −nFE°
✔️ n = number of electrons
✔️ F = Faraday constant
✔️ E° = standard emf
1️⃣2️⃣ #UNITSOFΔG
✔️ Joule
✔️ kJ mol⁻¹ (mostly used in chemistry)
1️⃣3️⃣ #NEET
✔️ ΔG decides feasibility, not rate
✔️ Spontaneous ≠ fast
✔️ ΔG depends on T, P & composition
✔️ ΔG is state function
1️⃣4️⃣ #ONELINEREVISION
✔️ Gibbs free energy predicts spontaneity
✔️ ΔG = 0 at equilibrium
✔️ Negative ΔG → feasible process
✔️ ΔG° related to K and E°
✔️ Thermodynamic state function
✔️ Determines spontaneity of process
✔️ Denoted by G
📌 Relation:
G = H − TS
2️⃣ #TERMSINFORMULA
✔️ H → Enthalpy
✔️ T → Absolute temperature (K)
✔️ S → Entropy
📌 Unit of G → Joule
3️⃣ #CHANGEINGIBBSENERGY
📌 Formula:
ΔG = ΔH − TΔS
✔️ Applies at constant T & P
4️⃣ #SIGNIFICANCEOFΔG (VERY IMP )
✔️ ΔG < 0 → Spontaneous process
✔️ ΔG = 0 → Equilibrium
✔️ ΔG > 0 → Non-spontaneous
5️⃣ #CASESBASEDONΔHANDΔS
✔️ ΔH < 0 and ΔS > 0
Process spontaneous at all temperatures
✔️ ΔH > 0 and ΔS < 0
Process non-spontaneous at all temperatures
✔️ ΔH < 0 and ΔS < 0
Spontaneous at low temperature
✔️ ΔH > 0 and ΔS > 0
Spontaneous at high temperature
6️⃣ #TEMPERATUREEFFECT
✔️ Increase in T increases importance of entropy term
✔️ TΔS dominates at high temperature
7️⃣ #GIBBSENERGYATEQUILIBRIUM
✔️ At equilibrium:
ΔG = 0
📌 Relation with equilibrium constant:
ΔG° = −RT ln K
8️⃣ #STANDARDGIBBSFREEENERGY
✔️ Measured at:
✔️ 1 bar pressure
✔️ 298 K temperature
📌 Formula:
ΔG° = ΔH° − TΔS°
9️⃣ #REACTIONQUOTIENTRELATION
📌 Formula:
ΔG = ΔG° + RT ln Q
✔️ Q = reaction quotient
📌 At equilibrium Q = K
🔟 #MAXIMUMWORKCONCEPT
✔️ ΔG gives maximum non-expansion work
✔️ Useful in electrochemistry
📌 Electrical work = −ΔG
1️⃣1️⃣ #GIBBSENERGYINELECTROCHEMISTRY
📌 Relation:
ΔG° = −nFE°
✔️ n = number of electrons
✔️ F = Faraday constant
✔️ E° = standard emf
1️⃣2️⃣ #UNITSOFΔG
✔️ Joule
✔️ kJ mol⁻¹ (mostly used in chemistry)
1️⃣3️⃣ #NEET
✔️ ΔG decides feasibility, not rate
✔️ Spontaneous ≠ fast
✔️ ΔG depends on T, P & composition
✔️ ΔG is state function
1️⃣4️⃣ #ONELINEREVISION
✔️ Gibbs free energy predicts spontaneity
✔️ ΔG = 0 at equilibrium
✔️ Negative ΔG → feasible process
✔️ ΔG° related to K and E°
🔥2👍1😍1
⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲
⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦
⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲
⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲
⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 𝗢𝗙 𝗧𝗛𝗜𝗦
⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦
⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲
⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲
⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 𝗢𝗙 𝗧𝗛𝗜𝗦
❤1🔥1👏1
Chemistry booster series
⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜…
Join kr lena all bcz in sbke full lec + crash course+ handwriting notes +short notes + test All in one milega
Haar batch ka even more then batch content
Haar batch ka even more then batch content
❤1🤩1🏆1
Q1.
Assertion (A): For a spontaneous process at constant temperature and pressure, ΔG is negative.
Reason (R): Spontaneous processes occur with decrease in Gibbs free energy.
Options:
(1) A & R true, R correct explanation
(2) A & R true, R not explanation
(3) A true, R false
(4) A false, R true
Q2.
Assertion (A): When ΔG = 0, the system is at equilibrium.
Reason (R): At equilibrium, forward and backward reaction rates are equal
Q3.
Assertion (A): A reaction with ΔH < 0 and ΔS < 0 is spontaneous at all temperatures.
Reason (R): Decrease in enthalpy always favours spontaneity.
Q5. (Numerical concept)
Assertion (A): If ΔH = −40 kJ and ΔS = −100 J K⁻¹, reaction is spontaneous at low temperature.
Reason (R): Negative ΔS disfavors spontaneity at high temperature
🕊1😍1🐳1
⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲
⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦
⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲
⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲
⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 𝗢𝗙 𝗧𝗛𝗜𝗦
⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦
⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲
⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲
⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 𝗢𝗙 𝗧𝗛𝗜𝗦
❤2🔥1🙏1
Chemistry booster series
⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜…
Krdo request send jisko bhi need ho bcz ab iske baad link nhi krunga m upload 3 baar copyright aa gya h inme
Link night 12 pr delete
Link night 12 pr delete
❤🔥4❤2🥰1
1️⃣ #CHEMICALEQUILIBRIUM
✔️ State where forward & reverse reactions occur at same rate
✔️ Concentrations of reactants & products become constant
📌 Example:
N₂ + 3H₂ ⇌ 2NH₃
2️⃣ #EQUILIBRIUMCONSTANT (K)
✔️ Ratio of product concentrations to reactant concentrations
✔️ Each raised to power of stoichiometric coefficient
📌 General reaction:
aA + bB ⇌ cC + dD
📌 Expression:
Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ
3️⃣ #TYPESOFEQUILIBRIUMCONSTANT
✔️ Kc → concentration based
✔️ Kp → partial pressure based
📌 Relation:
Kp = Kc(RT)ⁿ
✔️ n = moles of gaseous products − moles of gaseous reactants
4️⃣ #SIGNIFICANCEOFK
✔️ Predicts extent of reaction
✔️ Tells position of equilibrium
📌 Values:
✔️ K ≫ 1 → Product favoured
✔️ K ≪ 1 → Reactant favoured
✔️ K ≈ 1 → Both present
5️⃣ #REACTIONQUOTIENT (Q)
✔️ Same expression as K
✔️ Calculated at any stage of reaction
📌 Comparison:
✔️ Q < K → reaction proceeds forward
✔️ Q > K → reaction proceeds backward
✔️ Q = K → equilibrium
6️⃣ #APPLICATION1DIRECTIONOFREACTION
✔️ Compare Q with K
✔️ Predict spontaneous direction
📌 Very important for numericals
7️⃣ #APPLICATION2DEGREEOFDISSOCIATION
✔️ Used for weak electrolytes
📌 Example:
HA ⇌ H⁺ + A⁻
K = α²C / (1 − α)
✔️ α = degree of dissociation
✔️ C = initial concentration
8️⃣ #APPLICATION3IONIZATIONOFWEAKELECTROLYTES
✔️ Acids & bases have small K value
📌 Example:
CH₃COOH ⇌ H⁺ + CH₃COO⁻
✔️ Small K → weak acid
9️⃣ #APPLICATION4CALCULATIONOFCONCENTRATION
✔️ Find unknown equilibrium concentration
✔️ Used in ICE table method
📌 Steps:
✔️ Initial concentration
✔️ Change
✔️ Equilibrium
🔟 #APPLICATION5EFFECTOFCHANGINGCONDITIONS
✔️ Temperature change affects K
✔️ Concentration & pressure do NOT change K
📌 Only temperature changes K value
1️⃣1️⃣ #EFFECTOFTEMPERATURE
✔️ Endothermic reaction:
Temperature ↑ → K ↑
✔️ Exothermic reaction:
Temperature ↑ → K ↓
1️⃣2️⃣ #RELATIONWITHGIBBSFREEENERGY
📌 Formula:
ΔG° = −RT ln K
✔️ ΔG° < 0 → K > 1 (spontaneous)
✔️ ΔG° > 0 → K < 1
1️⃣3️⃣ #HETEROGENEOUSEQUILIBRIUM
✔️ Solids & liquids not included in K
📌 Example:
CaCO₃(s) ⇌ CaO(s) + CO₂(g)
Kp = P(CO₂)
1️⃣4️⃣ #REVERSINGREACTION
✔️ K(reverse) = 1 / K(forward)
1️⃣5️⃣ #MULTIPLYINGREACTION
✔️ If reaction multiplied by n
✔️ New K = Kⁿ
1️⃣6️⃣ #NEET⚠️
✔️ K depends only on temperature
✔️ Catalyst does not change K
✔️ Pure solids not included
✔️ Units of K depend on reaction
1️⃣7️⃣ #ONELINEREVISION
✔️ K predicts extent of reaction
✔️ Q vs K gives direction
✔️ Only temperature affects K
✔️ Kp–Kc relation important
✔️ State where forward & reverse reactions occur at same rate
✔️ Concentrations of reactants & products become constant
📌 Example:
N₂ + 3H₂ ⇌ 2NH₃
2️⃣ #EQUILIBRIUMCONSTANT (K)
✔️ Ratio of product concentrations to reactant concentrations
✔️ Each raised to power of stoichiometric coefficient
📌 General reaction:
aA + bB ⇌ cC + dD
📌 Expression:
Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ
3️⃣ #TYPESOFEQUILIBRIUMCONSTANT
✔️ Kc → concentration based
✔️ Kp → partial pressure based
📌 Relation:
Kp = Kc(RT)ⁿ
✔️ n = moles of gaseous products − moles of gaseous reactants
4️⃣ #SIGNIFICANCEOFK
✔️ Predicts extent of reaction
✔️ Tells position of equilibrium
📌 Values:
✔️ K ≫ 1 → Product favoured
✔️ K ≪ 1 → Reactant favoured
✔️ K ≈ 1 → Both present
5️⃣ #REACTIONQUOTIENT (Q)
✔️ Same expression as K
✔️ Calculated at any stage of reaction
📌 Comparison:
✔️ Q < K → reaction proceeds forward
✔️ Q > K → reaction proceeds backward
✔️ Q = K → equilibrium
6️⃣ #APPLICATION1DIRECTIONOFREACTION
✔️ Compare Q with K
✔️ Predict spontaneous direction
📌 Very important for numericals
7️⃣ #APPLICATION2DEGREEOFDISSOCIATION
✔️ Used for weak electrolytes
📌 Example:
HA ⇌ H⁺ + A⁻
K = α²C / (1 − α)
✔️ α = degree of dissociation
✔️ C = initial concentration
8️⃣ #APPLICATION3IONIZATIONOFWEAKELECTROLYTES
✔️ Acids & bases have small K value
📌 Example:
CH₃COOH ⇌ H⁺ + CH₃COO⁻
✔️ Small K → weak acid
9️⃣ #APPLICATION4CALCULATIONOFCONCENTRATION
✔️ Find unknown equilibrium concentration
✔️ Used in ICE table method
📌 Steps:
✔️ Initial concentration
✔️ Change
✔️ Equilibrium
🔟 #APPLICATION5EFFECTOFCHANGINGCONDITIONS
✔️ Temperature change affects K
✔️ Concentration & pressure do NOT change K
📌 Only temperature changes K value
1️⃣1️⃣ #EFFECTOFTEMPERATURE
✔️ Endothermic reaction:
Temperature ↑ → K ↑
✔️ Exothermic reaction:
Temperature ↑ → K ↓
1️⃣2️⃣ #RELATIONWITHGIBBSFREEENERGY
📌 Formula:
ΔG° = −RT ln K
✔️ ΔG° < 0 → K > 1 (spontaneous)
✔️ ΔG° > 0 → K < 1
1️⃣3️⃣ #HETEROGENEOUSEQUILIBRIUM
✔️ Solids & liquids not included in K
📌 Example:
CaCO₃(s) ⇌ CaO(s) + CO₂(g)
Kp = P(CO₂)
1️⃣4️⃣ #REVERSINGREACTION
✔️ K(reverse) = 1 / K(forward)
1️⃣5️⃣ #MULTIPLYINGREACTION
✔️ If reaction multiplied by n
✔️ New K = Kⁿ
1️⃣6️⃣ #NEET⚠️
✔️ K depends only on temperature
✔️ Catalyst does not change K
✔️ Pure solids not included
✔️ Units of K depend on reaction
1️⃣7️⃣ #ONELINEREVISION
✔️ K predicts extent of reaction
✔️ Q vs K gives direction
✔️ Only temperature affects K
✔️ Kp–Kc relation important
❤3👍2👌2💯1
⃣ #SOLUBILITYPRODUCT
✔️ Solubility product = product of molar concentrations of ions in saturated solution
✔️ Each concentration raised to power of its stoichiometric coefficient
📌 For salt: AₓBᵧ
Ksp = [A⁺]ˣ [B⁻]ʸ
2️⃣ #CONDITIONOFAPPLICABILITY
✔️ Salt must be sparingly soluble
✔️ Solution must be saturated
✔️ At constant temperature
.
3️⃣ #IONICDISSOCIATION
✔️ AB(s) ⇌ A⁺ + B⁻
✔️ A₂B(s) ⇌ 2A⁺ + B²⁻
✔️ AB₂(s) ⇌ A⁺ + 2B⁻
.
4️⃣ #MOLARSOLUBILITY (S)
✔️ Molar solubility = moles dissolved per litre to form saturated solution
📌 Units: mol L⁻¹
⭐⭐5️⃣ #KspINTERMSSOLUBILITY (VERY IMP )
5️⃣1️⃣ For AB
AB ⇌ A⁺ + B⁻
Ksp = S²
S = √Ksp
5️⃣2️⃣ For A₂B
A₂B ⇌ 2A⁺ + B²⁻
Ksp = (2S)²(S) = 4S³
S = (Ksp / 4)¹ᐟ³
5️⃣3️⃣ For AB₂
AB₂ ⇌ A⁺ + 2B⁻
Ksp = S(2S)² = 4S³
S = (Ksp / 4)¹ᐟ³
5️⃣4️⃣ For A₃B
A₃B ⇌ 3A⁺ + B³⁻
Ksp = (3S)³(S) = 27S⁴
6️⃣ #IONICPRODUCT (IP)
✔️ IP = product of ionic concentrations at any instant
📌 Comparison:
✔️ IP < Ksp → Unsaturated
✔️ IP = Ksp → Saturated
✔️ IP > Ksp → Precipitation
.
7️⃣ #COMMONIONEFFECT (NEET )
✔️ Solubility decreases in presence of common ion
📌 Example:
AgCl solubility ↓ in NaCl solution
📌 Reason: Equilibrium shifts backward
8️⃣ #EFFECTOFPHONCOMMONION
✔️ Solubility increases if no common ion present
9️⃣ #SELECTIVEPRECIPITATION
✔️ Salt with lower Ksp precipitates first
📌 Used in qualitative analysis
🔟 #RELATIONBETWEENSOLUBILITYANDKsp
✔️ Higher Ksp ≠ higher solubility always
✔️ Depends on stoichiometry of salt
1️⃣1️⃣ #SOLUBILITYINPRESENCEOFCOMMONION
For AB in presence of B⁻ concentration = C
Ksp = S × C
S = Ksp / C
📌 Used in buffer & salt solutions
1️⃣2️⃣ #SOLUBILITYINPRESENCEOFPH
✔️ For salts of weak acids → solubility increases in acidic medium
✔️ For salts of weak bases → solubility increases in basic medium
📌 Example:
CaCO₃ dissolves more in acidic solution
1️⃣3️⃣ #TEMPERATUREEFFECT
✔️ Ksp increases with temperature (usually)
✔️ Endothermic dissolution favoured
1️⃣4️⃣ #UNITOFKsp
✔️ Depends on stoichiometry
✔️ No fixed unit
📌 NEET note: Ksp has no unit
1️⃣5️⃣ #COMPARISONOFKspVALUES
✔️ Compare only salts with same formula type
✔️ Otherwise comparison invalid
1️⃣6️⃣ #PRECIPITATIONCONDITION
✔️ Precipitation starts when IP just exceeds Ksp
1️⃣7️⃣ #SOLUBILITYORDER
✔️ Lower Ksp → lower solubility (for same type salts)
1️⃣8️⃣ #NEET⚠️TRAPS
✔️ Ksp valid only for saturated solution
✔️ Ksp ≠ solubility
✔️ Common ion reduces solubility
✔️ Ksp independent of initial concentration
✔️ Compare Ksp only at same temperature
1️⃣9️⃣ #NUMERICALSHORTCUT
✔️ If Ksp = 10⁻¹⁰ for AB
S ≈ 10⁻⁵
✔️ If Ksp = 4×10⁻¹² for AB₂
S ≈ 10⁻⁴
2️⃣0️⃣ #ONELINEREVISION
✔️ Ksp = ionic product at saturation
✔️ Precipitation when IP > Ksp
✔️ Common ion ↓ solubility
✔️ Same Ksp ≠ same solubility
✔️ Solubility product = product of molar concentrations of ions in saturated solution
✔️ Each concentration raised to power of its stoichiometric coefficient
📌 For salt: AₓBᵧ
Ksp = [A⁺]ˣ [B⁻]ʸ
2️⃣ #CONDITIONOFAPPLICABILITY
✔️ Salt must be sparingly soluble
✔️ Solution must be saturated
✔️ At constant temperature
.
3️⃣ #IONICDISSOCIATION
✔️ AB(s) ⇌ A⁺ + B⁻
✔️ A₂B(s) ⇌ 2A⁺ + B²⁻
✔️ AB₂(s) ⇌ A⁺ + 2B⁻
.
4️⃣ #MOLARSOLUBILITY (S)
✔️ Molar solubility = moles dissolved per litre to form saturated solution
📌 Units: mol L⁻¹
⭐⭐5️⃣ #KspINTERMSSOLUBILITY (VERY IMP )
5️⃣1️⃣ For AB
AB ⇌ A⁺ + B⁻
Ksp = S²
S = √Ksp
5️⃣2️⃣ For A₂B
A₂B ⇌ 2A⁺ + B²⁻
Ksp = (2S)²(S) = 4S³
S = (Ksp / 4)¹ᐟ³
5️⃣3️⃣ For AB₂
AB₂ ⇌ A⁺ + 2B⁻
Ksp = S(2S)² = 4S³
S = (Ksp / 4)¹ᐟ³
5️⃣4️⃣ For A₃B
A₃B ⇌ 3A⁺ + B³⁻
Ksp = (3S)³(S) = 27S⁴
6️⃣ #IONICPRODUCT (IP)
✔️ IP = product of ionic concentrations at any instant
📌 Comparison:
✔️ IP < Ksp → Unsaturated
✔️ IP = Ksp → Saturated
✔️ IP > Ksp → Precipitation
.
7️⃣ #COMMONIONEFFECT (NEET )
✔️ Solubility decreases in presence of common ion
📌 Example:
AgCl solubility ↓ in NaCl solution
📌 Reason: Equilibrium shifts backward
8️⃣ #EFFECTOFPHONCOMMONION
✔️ Solubility increases if no common ion present
9️⃣ #SELECTIVEPRECIPITATION
✔️ Salt with lower Ksp precipitates first
📌 Used in qualitative analysis
🔟 #RELATIONBETWEENSOLUBILITYANDKsp
✔️ Higher Ksp ≠ higher solubility always
✔️ Depends on stoichiometry of salt
1️⃣1️⃣ #SOLUBILITYINPRESENCEOFCOMMONION
For AB in presence of B⁻ concentration = C
Ksp = S × C
S = Ksp / C
📌 Used in buffer & salt solutions
1️⃣2️⃣ #SOLUBILITYINPRESENCEOFPH
✔️ For salts of weak acids → solubility increases in acidic medium
✔️ For salts of weak bases → solubility increases in basic medium
📌 Example:
CaCO₃ dissolves more in acidic solution
1️⃣3️⃣ #TEMPERATUREEFFECT
✔️ Ksp increases with temperature (usually)
✔️ Endothermic dissolution favoured
1️⃣4️⃣ #UNITOFKsp
✔️ Depends on stoichiometry
✔️ No fixed unit
📌 NEET note: Ksp has no unit
1️⃣5️⃣ #COMPARISONOFKspVALUES
✔️ Compare only salts with same formula type
✔️ Otherwise comparison invalid
1️⃣6️⃣ #PRECIPITATIONCONDITION
✔️ Precipitation starts when IP just exceeds Ksp
1️⃣7️⃣ #SOLUBILITYORDER
✔️ Lower Ksp → lower solubility (for same type salts)
1️⃣8️⃣ #NEET⚠️TRAPS
✔️ Ksp valid only for saturated solution
✔️ Ksp ≠ solubility
✔️ Common ion reduces solubility
✔️ Ksp independent of initial concentration
✔️ Compare Ksp only at same temperature
1️⃣9️⃣ #NUMERICALSHORTCUT
✔️ If Ksp = 10⁻¹⁰ for AB
S ≈ 10⁻⁵
✔️ If Ksp = 4×10⁻¹² for AB₂
S ≈ 10⁻⁴
2️⃣0️⃣ #ONELINEREVISION
✔️ Ksp = ionic product at saturation
✔️ Precipitation when IP > Ksp
✔️ Common ion ↓ solubility
✔️ Same Ksp ≠ same solubility
❤2💯2😎1
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Short notes ,mind map & teachers hand writing notes
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#SystomaticallyAvailbale #EasyToSearch
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Q1
Assertion (A): Solubility of AgCl decreases on addition of NaCl.
Reason (R): Addition of NaCl increases concentration of Cl⁻ ions.
Q2
Assertion (A): Larger the value of Ksp, higher is the solubility of a salt.
Reason (R): Ksp is directly proportional to solubility for all salts
Q3
Assertion (A): Precipitation occurs when ionic product exceeds Ksp.
Reason (R): Solution becomes supersaturated under this condition.
Q4
Assertion (A): Solubility of BaSO₄ increases in presence of dilute HCl.
Reason (R): H⁺ ions react with SO₄²⁻ ions to form HSO₄⁻.
Q5
Assertion (A): Two salts having same Ksp may have different solubilities.
Reason (R): Solubility depends on number of ions produced on dissociation
.
❤1🎉1
1️⃣ #WEAKELECTROLYTES
✔️ Weak acids & weak bases ionise partially in aqueous solution
✔️ Establish equilibrium between ionised & unionised form
📌 Examples:
✔️ Weak acid → CH₃COOH
✔️ Weak base → NH₄OH
2️⃣ #IONISATIONOFWEAKACID
✔️ Partial dissociation in water
📌 General reaction:
HA + H₂O ⇌ H₃O⁺ + A⁻
📌 Example:
CH₃COOH + H₂O ⇌ H₃O⁺ + CH₃COO⁻
3️⃣ #ACIDDISSOCIATIONCONSTANT (Ka)
✔️ Measure of strength of weak acid
✔️ Higher Ka → stronger acid
📌 Expression:
Ka = [H⁺][A⁻] / [HA]
✔️ Unit: mol L⁻¹
4️⃣ #DEGREEOFIONISATION (α)
✔️ Fraction of total molecules ionised
📌 Formula:
α = Number of molecules ionised / Total molecules
✔️ For weak acids → α ≪ 1
5️⃣ #RELATIONBETWEENKaANDα (NEET FAV )
For weak acid of concentration C:
📌 Formula:
Ka = Cα²
📌 Therefore:
α = √(Ka / C)
✔️ Ionisation increases on dilution
6️⃣ #pKaCONCEPT
✔️ pKa = –log Ka
✔️ Lower pKa → stronger acid
📌 Relation:
Strong acid → small pKa
Weak acid → large pKa
7️⃣ #pHOFWEAKACID
For weak acid of concentration C:
📌 Formula:
[H⁺] = √(Ka × C)
📌 pH formula:
pH = ½ ( pKa – log C )
✔️ Very important for numericals
8️⃣ #IONISATIONOFWEAKBASE
✔️ Partial dissociation in water
📌 General reaction:
BOH ⇌ B⁺ + OH⁻
📌 Example:
NH₄OH ⇌ NH₄⁺ + OH⁻
9️⃣ #BASEDISSOCIATIONCONSTANT (Kb)
✔️ Measure of strength of weak base
✔️ Higher Kb → stronger base
📌 Expression:
Kb = [B⁺][OH⁻] / [BOH]
🔟 #RELATIONBETWEENKbANDα
For weak base of concentration C:
📌 Formula:
Kb = Cα²
📌 Therefore:
α = √(Kb / C)
1️⃣1️⃣ #pKbCONCEPT
✔️ pKb = –log Kb
✔️ Lower pKb → stronger base
1️⃣2️⃣ #pHOFWEAKBASE
For weak base of concentration C:
📌 [OH⁻] = √(Kb × C)
📌 pOH formula:
pOH = ½ ( pKb – log C )
📌 pH = 14 – pOH
1️⃣3️⃣ #DILUTIONEFFECT (VERY IMP 🔥)
✔️ On dilution → degree of ionisation increases
✔️ But total ions per unit volume decrease
📌 Ostwald’s dilution law applies
1️⃣4️⃣ #COMMONIONEFFECT
✔️ Ionisation of weak electrolyte decreases
✔️ Presence of common ion shifts equilibrium backward
📌 Example:
CH₃COOH + CH₃COONa → ionisation decreases
1️⃣5️⃣ #WEAKACIDVSWEAKBASE
✔️ Weak acid → H⁺ producing
✔️ Weak base → OH⁻ producing
✔️ Both show partial ionisation
1️⃣6️⃣ #NEET⚠️KEYPOINTS
✔️ Ka & Kb are temperature dependent
✔️ α increases with dilution
✔️ pH of weak acid > strong acid (same concentration)
✔️ pH of weak base < strong base (same concentration)
1️⃣7️⃣ #ONELINEREVISION
✔️ Weak electrolytes ionise partially
✔️ Ka = Cα²
✔️ [H⁺] = √(Ka × C)
✔️ pH weak acid = ½ (pKa – log C)
✔️ Dilution increases ionisation
✔️ Weak acids & weak bases ionise partially in aqueous solution
✔️ Establish equilibrium between ionised & unionised form
📌 Examples:
✔️ Weak acid → CH₃COOH
✔️ Weak base → NH₄OH
2️⃣ #IONISATIONOFWEAKACID
✔️ Partial dissociation in water
📌 General reaction:
HA + H₂O ⇌ H₃O⁺ + A⁻
📌 Example:
CH₃COOH + H₂O ⇌ H₃O⁺ + CH₃COO⁻
3️⃣ #ACIDDISSOCIATIONCONSTANT (Ka)
✔️ Measure of strength of weak acid
✔️ Higher Ka → stronger acid
📌 Expression:
Ka = [H⁺][A⁻] / [HA]
✔️ Unit: mol L⁻¹
4️⃣ #DEGREEOFIONISATION (α)
✔️ Fraction of total molecules ionised
📌 Formula:
α = Number of molecules ionised / Total molecules
✔️ For weak acids → α ≪ 1
5️⃣ #RELATIONBETWEENKaANDα (NEET FAV )
For weak acid of concentration C:
📌 Formula:
Ka = Cα²
📌 Therefore:
α = √(Ka / C)
✔️ Ionisation increases on dilution
6️⃣ #pKaCONCEPT
✔️ pKa = –log Ka
✔️ Lower pKa → stronger acid
📌 Relation:
Strong acid → small pKa
Weak acid → large pKa
7️⃣ #pHOFWEAKACID
For weak acid of concentration C:
📌 Formula:
[H⁺] = √(Ka × C)
📌 pH formula:
pH = ½ ( pKa – log C )
✔️ Very important for numericals
8️⃣ #IONISATIONOFWEAKBASE
✔️ Partial dissociation in water
📌 General reaction:
BOH ⇌ B⁺ + OH⁻
📌 Example:
NH₄OH ⇌ NH₄⁺ + OH⁻
9️⃣ #BASEDISSOCIATIONCONSTANT (Kb)
✔️ Measure of strength of weak base
✔️ Higher Kb → stronger base
📌 Expression:
Kb = [B⁺][OH⁻] / [BOH]
🔟 #RELATIONBETWEENKbANDα
For weak base of concentration C:
📌 Formula:
Kb = Cα²
📌 Therefore:
α = √(Kb / C)
1️⃣1️⃣ #pKbCONCEPT
✔️ pKb = –log Kb
✔️ Lower pKb → stronger base
1️⃣2️⃣ #pHOFWEAKBASE
For weak base of concentration C:
📌 [OH⁻] = √(Kb × C)
📌 pOH formula:
pOH = ½ ( pKb – log C )
📌 pH = 14 – pOH
1️⃣3️⃣ #DILUTIONEFFECT (VERY IMP 🔥)
✔️ On dilution → degree of ionisation increases
✔️ But total ions per unit volume decrease
📌 Ostwald’s dilution law applies
1️⃣4️⃣ #COMMONIONEFFECT
✔️ Ionisation of weak electrolyte decreases
✔️ Presence of common ion shifts equilibrium backward
📌 Example:
CH₃COOH + CH₃COONa → ionisation decreases
1️⃣5️⃣ #WEAKACIDVSWEAKBASE
✔️ Weak acid → H⁺ producing
✔️ Weak base → OH⁻ producing
✔️ Both show partial ionisation
1️⃣6️⃣ #NEET⚠️KEYPOINTS
✔️ Ka & Kb are temperature dependent
✔️ α increases with dilution
✔️ pH of weak acid > strong acid (same concentration)
✔️ pH of weak base < strong base (same concentration)
1️⃣7️⃣ #ONELINEREVISION
✔️ Weak electrolytes ionise partially
✔️ Ka = Cα²
✔️ [H⁺] = √(Ka × C)
✔️ pH weak acid = ½ (pKa – log C)
✔️ Dilution increases ionisation
❤5💯2🔥1
1️⃣ #REDOXREACTION
✔️ Redox reaction = reaction involving simultaneous oxidation and reduction
✔️ Oxidation → loss of electrons
✔️ Reduction → gain of electrons
📌 Example:
Zn + Cu²⁺ → Zn²⁺ + Cu
✔️ Zn → Zn²⁺ + 2e⁻ (Oxidation)
✔️ Cu²⁺ + 2e⁻ → Cu (Reduction)
2️⃣ #OXIDATIONNUMBERCONCEPT
✔️ Oxidation number (ON) = hypothetical charge if all bonds ionic
✔️ Increase in ON → oxidation
✔️ Decrease in ON → reduction
📌 Rules:
✔️ Element in free state → ON = 0
✔️ Monatomic ion → ON = charge
✔️ Oxygen → usually –2
✔️ Hydrogen → usually +1
✔️ Sum of ONs in molecule → 0
✔️ Sum of ONs in polyatomic ion → ion charge
3️⃣ #TYPESOFREDOXREACTIONS
✔️ Combination reaction → A + B → AB
✔️ Decomposition → AB → A + B
✔️ Displacement → A + BC → AC + B
✔️ Disproportionation → X → Xⁿ⁺ + Xᵐ⁻
📌 Example:
2H₂O₂ → 2H₂O + O₂
✔️ O in H₂O₂: –1 → 0 & –2 (disproportionation)
4️⃣ #OXIDISINGAGENT
✔️ Substance that accepts electrons
✔️ Causes oxidation of other species
📌 Example:
✔️ Cu²⁺ in Zn + Cu²⁺ → Cu²⁺ is oxidising agent
5️⃣ #REDUCINGAGENT
✔️ Substance that donates electrons
✔️ Causes reduction of other species
📌 Example:
✔️ Zn in Zn + Cu²⁺ → Zn is reducing agent
6️⃣ #ELECTRONBALANCEMETHOD (NEET FAV )
✔️ Step 1 → Write oxidation & reduction half-reactions
✔️ Step 2 → Balance atoms other than O & H
✔️ Step 3 → Balance O by H₂O
✔️ Step 4 → Balance H by H⁺ (acidic) or OH⁻ (basic)
✔️ Step 5 → Balance electrons
✔️ Step 6 → Combine half-reactions
7️⃣ #IONICEQUATIONEXAMPLE
✔️ Fe²⁺ + Cr₂O₇²⁻ → Fe³⁺ + Cr³⁺ (acidic medium)
📌 Half-reactions:
Fe²⁺ → Fe³⁺ + e⁻
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O
📌 Multiply Fe reaction by 6 → 6Fe²⁺ → 6Fe³⁺ + 6e⁻
📌 Combine → 6Fe²⁺ + Cr₂O₇²⁻ + 14H⁺ → 6Fe³⁺ + 2Cr³⁺ + 7H₂O
8️⃣ #DISPROPORTIONATIONREACTIONS
✔️ Same element undergoes oxidation & reduction simultaneously
📌 Example:
3Cl₂ + 6OH⁻ → 5Cl⁻ + ClO₃⁻ + 3H₂O
✔️ Cl → –1 & +5
9️⃣ #NEET⚠️KEYPOINTS
✔️ Redox can occur in acidic or basic medium
✔️ Use oxidation number method for quick identification
✔️ Disproportionation = special redox with same element
✔️ Oxidising & reducing agents always appear on opposite sides
1️⃣0️⃣ #ONELINEREVISION
✔️ Redox = Oxidation + Reduction
✔️ Oxidation → loss e⁻, ON ↑
✔️ Reduction → gain e⁻, ON ↓
✔️ Oxidising agent → gains e⁻
✔️ Reducing agent → loses e⁻
✔️ Use half-reaction method for balancing
✔️ Redox reaction = reaction involving simultaneous oxidation and reduction
✔️ Oxidation → loss of electrons
✔️ Reduction → gain of electrons
📌 Example:
Zn + Cu²⁺ → Zn²⁺ + Cu
✔️ Zn → Zn²⁺ + 2e⁻ (Oxidation)
✔️ Cu²⁺ + 2e⁻ → Cu (Reduction)
2️⃣ #OXIDATIONNUMBERCONCEPT
✔️ Oxidation number (ON) = hypothetical charge if all bonds ionic
✔️ Increase in ON → oxidation
✔️ Decrease in ON → reduction
📌 Rules:
✔️ Element in free state → ON = 0
✔️ Monatomic ion → ON = charge
✔️ Oxygen → usually –2
✔️ Hydrogen → usually +1
✔️ Sum of ONs in molecule → 0
✔️ Sum of ONs in polyatomic ion → ion charge
3️⃣ #TYPESOFREDOXREACTIONS
✔️ Combination reaction → A + B → AB
✔️ Decomposition → AB → A + B
✔️ Displacement → A + BC → AC + B
✔️ Disproportionation → X → Xⁿ⁺ + Xᵐ⁻
📌 Example:
2H₂O₂ → 2H₂O + O₂
✔️ O in H₂O₂: –1 → 0 & –2 (disproportionation)
4️⃣ #OXIDISINGAGENT
✔️ Substance that accepts electrons
✔️ Causes oxidation of other species
📌 Example:
✔️ Cu²⁺ in Zn + Cu²⁺ → Cu²⁺ is oxidising agent
5️⃣ #REDUCINGAGENT
✔️ Substance that donates electrons
✔️ Causes reduction of other species
📌 Example:
✔️ Zn in Zn + Cu²⁺ → Zn is reducing agent
6️⃣ #ELECTRONBALANCEMETHOD (NEET FAV )
✔️ Step 1 → Write oxidation & reduction half-reactions
✔️ Step 2 → Balance atoms other than O & H
✔️ Step 3 → Balance O by H₂O
✔️ Step 4 → Balance H by H⁺ (acidic) or OH⁻ (basic)
✔️ Step 5 → Balance electrons
✔️ Step 6 → Combine half-reactions
7️⃣ #IONICEQUATIONEXAMPLE
✔️ Fe²⁺ + Cr₂O₇²⁻ → Fe³⁺ + Cr³⁺ (acidic medium)
📌 Half-reactions:
Fe²⁺ → Fe³⁺ + e⁻
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O
📌 Multiply Fe reaction by 6 → 6Fe²⁺ → 6Fe³⁺ + 6e⁻
📌 Combine → 6Fe²⁺ + Cr₂O₇²⁻ + 14H⁺ → 6Fe³⁺ + 2Cr³⁺ + 7H₂O
8️⃣ #DISPROPORTIONATIONREACTIONS
✔️ Same element undergoes oxidation & reduction simultaneously
📌 Example:
3Cl₂ + 6OH⁻ → 5Cl⁻ + ClO₃⁻ + 3H₂O
✔️ Cl → –1 & +5
9️⃣ #NEET⚠️KEYPOINTS
✔️ Redox can occur in acidic or basic medium
✔️ Use oxidation number method for quick identification
✔️ Disproportionation = special redox with same element
✔️ Oxidising & reducing agents always appear on opposite sides
1️⃣0️⃣ #ONELINEREVISION
✔️ Redox = Oxidation + Reduction
✔️ Oxidation → loss e⁻, ON ↑
✔️ Reduction → gain e⁻, ON ↓
✔️ Oxidising agent → gains e⁻
✔️ Reducing agent → loses e⁻
✔️ Use half-reaction method for balancing
❤3🔥3👍1🎉1
Periodic table order
Exceptional like
1st ⭐#Radii grp 13 p block al>Ga
d series mn 3d5 sw so vahi sw reverse then fe=co=ni then cu<zn
2nd ⭐ #IE 3d<4d<5d but in 4th to 12th grp
4d=5d (appro) LC.
In grp 13 Beet, GAI
14th pb>sn
3rd ⭐EA : 2nd period se 3rd vale ki hmesha jyada
Highest Cl
Oxygen family M O last m
Exceptional like
1st ⭐#Radii grp 13 p block al>Ga
d series mn 3d5 sw so vahi sw reverse then fe=co=ni then cu<zn
2nd ⭐ #IE 3d<4d<5d but in 4th to 12th grp
4d=5d (appro) LC.
In grp 13 Beet, GAI
14th pb>sn
3rd ⭐EA : 2nd period se 3rd vale ki hmesha jyada
Highest Cl
Oxygen family M O last m
❤2🔥2😘2💯1