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Thermochemistry

Temperature Conversion

°C = K - 273 K = °C + 273

Heat transfer

Q = mc?T

Hess's Law (Enthalpy)

?H = ??H_products ? ??H_reactants

Entropy

?S = ?S_products - ?S_reactants

Gibbs Free Energy

?G = ??G^°_products - ??G^°_reactants

and ?G = ?H - T?S

Chemical Equilibrium

Equilibrium Constant.

for a general reaction equation: aA + bB cC + dD

K_eq

=

[C]^c × [D]^d

[A]^a × [B]^b

Solutions

Molarity, M

Molarity =

moles solute

litre solution

Parts per million, ppm

ppm =

mass solute

mass solution

x 1,000,000

dilutions

M₁V₁= M₂V₂

Solubility product constant, K_sp

for a general reaction:

A_bX_{y (s)} bA⁺_(aq) + yX^?_(aq)

K_sp = [A⁺]^b × [X^?]^y

Acids and Bases

K_a and K_b

for a general reaction:

H_bX_{y (s)} bH⁺_(aq) + yX^?_(aq)

K_a= [H⁺]^b × [X^?]^y

K_w

H₂O_(l) H⁺_(aq) + OH^-_(aq)

K_w = [H⁺][OH^-] = 1.0 × 10^-14

pH

pH = - log [H⁺]

pH and pOH

pH + pOH = 14

Titration (for 1:1 Acid:Base ratio)

Community Contributions - Articles by goIITians

Thermochemistry

Temperature Conversion

°C = K - 273 K = °C + 273

Heat transfer

Q = mc?T

Hess's Law (Enthalpy)

?H = ??Hproducts ? ??Hreactants

Entropy

?S = ?Sproducts - ?Sreactants

Gibbs Free Energy

?G = ??G° products - ??G° reactants

and ?G = ?H - T?S

Chemical Equilibrium

Equilibrium Constant. for a general reaction equation: aA + bB cC + dD

Keq

=

[C]c × [D]d

[A]a × [B]b

Solutions

Molarity, M

Molarity =

moles solute

litre solution

Parts per million, ppm

ppm =

mass solute

mass solution

x 1,000,000

dilutions

M1V1= M2V2

Solubility product constant, Ksp

for a general reaction: AbXy (s) bA+(aq) + yX?(aq)

Ksp = [A+]b × [X?]y

Acids and Bases

Ka and Kb

for a general reaction: HbXy (s) bH+(aq) + yX?(aq)

Ka= [H+]b × [X?]y

Kw

H2O(l) H+(aq) + OH-(aq)

Kw = [H+][OH-] = 1.0 × 10-14

pH

pH = - log [H+]

pH and pOH

pH + pOH = 14

Titration (for 1:1 Acid:Base ratio)

MAVA = MBVB

?H = ??H_products ? ??H_reactants

?S = ?S_products - ?S_reactants

?G = ??G^°_products - ??G^°_reactants

Equilibrium Constant.

for a general reaction equation: aA + bB cC + dD

K_eq

[C]^c × [D]^d

[A]^a × [B]^b

M₁V₁= M₂V₂

Solubility product constant, K_sp

for a general reaction:

A_bX_{y (s)} bA⁺_(aq) + yX^?_(aq)

K_sp = [A⁺]^b × [X^?]^y

K_a and K_b

for a general reaction:

H_bX_{y (s)} bH⁺_(aq) + yX^?_(aq)

K_a= [H⁺]^b × [X^?]^y

K_w

H₂O_(l) H⁺_(aq) + OH^-_(aq)

K_w = [H⁺][OH^-] = 1.0 × 10^-14

pH = - log [H⁺]

M_AV_A = M_BV_B