Acid Base Concept
pH Calculations
Buffers
Titrations!
RANDOM TRIVIA
100

Name all strong acids!

HCl, HBr, HI, HNO3, H2SO4, HClO4

100

Calculate pH given concentrations of OH- or H3O+ OR Calculate H3O+ given pOH

[H3O+] = 7.49•10-6

[OH-] = 8.53•10-7

[H3O+] = 7.49•10-6

[OH-] = 6.46•10-6

pOH = 2.9

[H3O+] = 7.49•10-6 pH = 5.17

[OH-] = 8.53•10-7 pH = 7.93

[H3O+] = 1.23•10-6 pH = 10.91

[OH-] = 6.46•10-6 pH = 8.81

pOH = 2.9 [H3O+] = 7.94•10-12

100
What is the pH of a buffer solution that is 0.24M NH3 and 0.20M NH4Cl?

NH4+ Ka = 5.6•10-10

pH = 9.33

100

A 50.0mL solution of 0.100M HCl is titrated with 0.100M NaOH. Calculate pH after addition.

0mL, 25mL, 50mL, 60mL

0mL) pH = 1.00

25mL) pH = 1.48

50mL) pH = 7.00

60mL) pH = 12.00

100

What is the tennis score for (0:0)?

"Love All"

200

Name all strong bases

LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

200

What is the [H3O+], [OH-], pH, and pOH of 0.15 NaOH at room temp?

[H3O+] = 6.7•10-14M

[OH-] = 0.15M

pH = 13.18

pOH = 0.82

200
Determine the pH of a Buffer solution that is comprised of 0.200M Lactic Acid and 0.500M of Lactate. Ka Lactic Acid = 1.38•10-4​


​​​

pH = 4.25

200

100.0 mL solution of 0.100M NH3 is titrated with 0.100M HClO4. Calculate the pH after the following additions of HClO4.


Kb NH3 = 1.8•10-5


200mL and 250mL

pH = 1.48

pH = 1.37

200

What is the condensed electron configuration of cobalt ion, Co3+ ? 

[Ar] 4s0 3d6  

300

Write formula for pKa, pKb, Ka, Kb, Kw and %ionization. (WRITE UNITS if they apply)

Check with SI Leader Amb! :D

300

What is the pH and percent ionization of a 0.696M solution of HCN?

Ka = 4.9•10-10

pH = 4.73

%ion = 0.00266%

300

100.0 mL solution of 0.100M NH3 is titrated with 0.100M HClO4. Calculate the pH after the following additions of HClO4.

Kb NH3 = 1.8•10-5

0mL and 100 mL!

0mL) pH = 11.13

100mL) pH = 5.28

300

What language has the most native speakers worldwide?

Mandarin Chinese

400

What is a buffer, and how would you make a buffer using a weak acid solution with NaOH?

A Buffer is a solution containing a major species of a conjugate weak acid/base pair.

Add NaOH to neutralize HALF of the weak acid to make a buffer.

400

What is the pH and percent ionization of a 0.749M solution of F-? (READ CAREFULLY)

Ka of HF = 3.5•10-4

pH = 8.68

%ion = 0.000601%

400

100.0 mL solution of 0.100M NH3 is titrated with 0.100M HClO4. Calculate the pH after the following additions of HClO4.

Kb NH3 = 1.8•10-5

25mL and 150 mL!

25mL) pH = 9.73

150mL) pH = 1.70

400

Riddle: The more you take, the more you leave behind, what am I?

Footsteps

500

Draw titration curves for

- Titration of Strong Acid with a Strong Base

- Titration of a Strong Base with a Strong Acid

- Titration of a Weak Acid with a Strong Base

- Titration of a Weak Base with a Strong Acid

- (Bonus: 100 more points!) Titration of a Weak Base with a Weak Acid

Check with SI leader Amb! :D

500

what is the pH and percent ionization of 0.214M solution of CH3COO-?

Ka CH3COOH = 1.8•10-5

(READ CAREFULLY!)

pH = 9.04

%ion = 0.00509%

500

A 800.0mL solution of 0.200M CH3NH2 is titrated with 0.800M HI. Calculate the pH after the following additions of HI solution. pKb = 3.36

0mL, 50mL, 100mL, 150mL, 200mL, and 250mL

0mL) pH = 11.97

50mL) pH = 11.12

100mL) pH = 10.64

150mL) pH = 10.16

200mL) pH = 5.72

250mL) pH = 1.42

500

What's the rarest blood type?

AB-negative

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