Calculate the pH of 2.0 x 10 -3 M HI. Acid-Base Equilibria.

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Presentation transcript:

Calculate the pH of 2.0 x M HI

Acid-Base Equilibria

Ionization of Water H 2 O (l)  H + (aq) + OH - (aq) 2 H 2 O (l)  H 3 O + (aq) + OH - (aq)

Water Ionization Constant K w = [H + ][OH - ] K w = [H 3 O + ][OH - ] K w = 1.00 x Memorize this

K w Calculations In pure water [H + ] = [OH - ] K w = [H + ][OH - ] = 1.0 x Let [H + ] = x = [OH - ]

K w Calculations K w = [H + ][OH - ] = x 2 K w = x 2 =1.0 x Thus x = 1.0 x M [H + ] = x = 1.0 x M

pH of Pure Water [H + ] = 1.0 x M pH = -log[H + ] pH = -log[1.0 x ] pH = 7 -log 1 Thus pH = 7.00

Calculate [H + ],[OH - ], pH, & pOH of M HCl

Drill: Calculate [H + ],[OH - ], pH, & pOH of M KOH

Calculate [H + ],[OH - ], pH, & pOH of M H 2 SO 4

Weak Acid Ionization HA (aq) H + (aq) + A - (aq) HA (aq) + H 2 O (l) H 3 O + (aq) + A - (aq)

Acid Dissociation Constant HA (aq) H + (aq) + A - (aq) [H + ][A - ] [HA] K a =

Calculate the pH of 3.3 x M HI

Weak Base Ionization NH 3 (aq) + H 2 O (l) NH 4 + (aq) + OH - (aq)

Base Dissociation Constant NH 3(aq) + H 2 O (l) NH 4 + (aq) + OH - (aq) [NH 4 + ][OH - ] [NH 3 ] K b =

Acid-Base Equilibria Problems

Calculate [H + ], [OH - ], pH, & pOH of 2.0 M HC 2 H 3 O 2 (HAc) K a = 1.8 x 10 -5

Calculate [H + ], [OH - ], pH, & pOH of 0.50 M NH 3 K b = 1.8 x 10 -5

Calculate [H + ], [OH - ], pH, & pOH of 0.50 M C 6 H 5 NH 2 K b = 3.2 x 10 -5

Calculate [H + ],[OH - ], pH, & pOH of M HC 7 H 5 O 2 (HBz) K a = 6.4 x 10 -5

Calculate the K a of 0.10 M Hquack when it ionized 5.0 % in an aqueous solution.

Drill: The pH of a 0.79 M solution of Hnut is Calculate its K a

Calculate the pH of a solution of M HBS : K a = 5.0 x

Calculate the pH of M HF: K a = 6.4 x 10 -4

Drill: Calculate the pH of M QOH: K b = 2.0 x 10 -4

Calculate [H 2 CO 3 ], [HCO 3 - ], [CO 3 -2 ], [H + ],[OH - ], & pH of 0.44 M H 2 CO 3 K a1 = 4.4 x K a2 = 4.7 x

Calculate the pH, & pOH of 0.10 M HClO K a = 2.5 x 10 -8

Drill: Calculate the pH of 0.25 M HAx K a = 2.5 x 10 -9

Review

Arhrenius Bronsted- Lowry Lewis

Show the ionization of HClO 4 in solution

Show the ionization of NH 3 in solution

Calculate the [H + ], [OH - ], pH, & pOH of 0.1 M HNO 3

Calculate the [H + ], [OH - ], pH, & pOH of 0.02 M NaOH

Calculate the pH, & pOH of 0.10 M HNO 2 K a = 6.0 x 10 -4

Calculate [H 2 A], [HA - ], [A -2 ], [H + ], & pH of 0.20 M H 2 A K a1 = 2.0 x K a2 = 5.0 x

Calculate [H 3 A],[H 2 A - ], [HA -2 ],[A -3 ],[H + ], & pH of 0.30 M H 3 A K a1 = 3.0 x K a2 = 5.0 x K a3 = 4.0 x

Drill: 831 mL NH 3 was bubbled through 2.0 L of water at 27.0 o C under 150 kPa pressure % of the ammonia reacted with the water. Calculate the pH of the final solution.