Chem Exam 2

I.C.E Tables

1. Initial

2. Change in concentration

3. End/Equilibrium.

K_b

K_a

H⁺ = …

K_w

Steps to Acid-Base EQ

1. Dissociate completely.

2. Conduct main reaction w/ I.C.E table.

3. Find K_b

4. Plug in ICE table values equal to K_b

5. Solve for X

6. Conduct second reaction, determine if negligible.

7. Find final concentrations

8. Find H+

K_c

Equilibrium constant in terms of concentration. Brackets are concentrations and exponents on coefficients from balanced equation.

Concentration

moles per liter (mol/L)

Quadratic Formula

Henderson-Hasselbach EQ

Strong Acids (everything else weak)

• HCl (hydrochloric acid)

• HBr (hydrobromic acid)

• HI (hydroiodic acid)

• HNO₃ (nitric acid)

• HClO₄ (perchloric acid)

• H₂SO₄ (sulfuric acid — strong for first H⁺)

Strong bases (everything else weak)

(LiNaKoCaSrBa)

• LiOH

• NaOH

• KOH

• Ca(OH)₂

• Sr(OH)₂

• Ba(OH)₂

pH

pOH

Brønsted-Lowry acid

Proton donor and creates conjugate base

Brønsted-Lowry base

Proton acceptor and creates conjugate acid

Conjugate base of weak acid: more acidic solution =

More soluble

Conjugate base of strong acid: more basic solution =

Less soluble

Increase solubility by…

Removing ions (Or add H)

Decrease solubility by…

Adding a common ion (or add OH)

Weak acid conjugate base

Acid increases solubility

Strong acid conjugate base

No effect

If X is basic from weak acid, solubility…

Increases

If X is neutral from strong acid, solubility…

Doesn’t change.

What determines if acid affects solubility

Whether anion reacts with H+

Larger Ka of conjugate acid means weaker what and less what effect?

Weaker base and less pH effect.

Higher Ksp

More soluble

Cation

Positive (left side of table)

Anion

Negative (right side of table)

Ksp

Ksp=∏(ion concentration)coefficient

• Multiply all ions

• Raise to power of their coefficient

• Ignore the solid