06Class 11 Chemistry

Equilibrium formulas

Equilibrium constant, pH, buffer and solubility formulas. Ionic equilibrium is formula-heavy, and a sheet like this helps a lot here.

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Chemical equilibrium

Equilibrium constant: $\displaystyle K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}$
Kp and Kc: $\displaystyle K_p = K_c(RT)^{\Delta n_g}$
Reaction quotient: $\displaystyle Q < K: \text{forward}, \quad Q > K: \text{backward}, \quad Q = K: \text{at equilibrium}$

pH: $\displaystyle \text{pH} = -\log[\text{H}^+]$
Water: $\displaystyle K_w = [\text{H}^+][\text{OH}^-] = 10^{-14}$
At 298 K, so pH + pOH = 14.
Conjugate pairs: $\displaystyle K_a\times K_b = K_w$
Weak acid: $\displaystyle \alpha = \sqrt{\frac{K_a}{C}}, \quad [\text{H}^+] = \sqrt{K_aC}$
For small α.
Acidic buffer: $\displaystyle \text{pH} = \text{p}K_a + \log\frac{[\text{salt}]}{[\text{acid}]}$
Basic buffer: $\displaystyle \text{pOH} = \text{p}K_b + \log\frac{[\text{salt}]}{[\text{base}]}$

Including pure solids and liquids in K. Their concentrations aren't written.
Assuming K changes with concentration or a catalyst. Only temperature changes it.
Using pH + pOH = 14 at temperatures other than 298 K.

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