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100

[H3O+] of a solution with a pH of 4.56 

2.75 x 10-5 M

100

Rank the following from weakest to strongest acid 

HCl, NH3, HI

NH3< HCl< HI

100

What will be the salt of the given reaction? 

Zn(OH)2 + HNO3 →  ???

Zn(NO3)2 + 2 H2O

100

What is the Henderson-Hasselbach equation?

pH = pka + log([A-]/[HA])

100

Define the Acid, Base, Conj Acid, and Conj in this reaction:

HCO3- + H2O --> OH- + H2CO3

A = H2O

B=HCO3-

CA: H2CO3

CB: OH-

200

pOH of a 0.3 M HCl Solution

pOH = 13.47

200

Rank the following from highest to lowest pH: 

HI, NaOH, HCN, Ca(OH)2, NH3

Ca(OH)2>NaOH>NH3>HCN>HI

200

A neutral solution contains what?

  1. No free ions
  2. Salts of metals
  3. Electrons and protons
  4. Equal number of H+ and OH– ions

4. Equal number of H+ and OH– ions

200

How do you make an acidic buffer solution?

A mixture of a weak acid and its conjugate strong base as a salt

200

A compound that can react as both an acid and base is _______.

amphoteric

300

[OH] = 4.7 x 10-4. What is the pH, and is this solution acidic or basic?

pH = 10.67 and basic

300

Draw the weak acid of the imidazole ion on the whiteboard.


Lone pair on nitrogen with original positive charge

300

What do you expect the pH to be if KCN is mixed in water?

pH > 7, basic

300

What is the pH of a buffer solution comprised of 0.25 M NH3 and 0.56 M NH4+? The pKb is 4.74.

pH=pKa + log [A-]/[HA-]

pH = 8.9097

300

If an acid has a pKa of 4.6, what is its Kb?

Kb = 3.981 x 10-10

400

The [OH¯] in a solution containing a pH of 3.45

2.818 x 10-11 M

400

What is the [HA] initially of a weak monoprotic acid if the resulting pH is 3.6 and the Ka=1.5x10-6?

[HA]=0.0421

400

Find the pH of a solution of 0.200 M NH4NO3 where (Ka = 1.8 * 10-5).

pH = 2.72

400

A 0.1 mol of CH3NH2 with Kb = 5 X 10-4 is mixed with 0.08 mol of HCl and diluted to one liter. What is the [H+] concentration in the solution?

[H+] = 8.00 X 10-11 M

400

What is the pH of a solution containing 60mg of KOH in 300 mL? 

The molar mass of KOH is 56 g/mol.

pH=11.55

500

The pH of a 0.4 M solution of Ba(OH)2

pH = 13.9 

500

What is the pKb of a weak monoprotic base if the pOH of a 0.35 M solution is 1.95 at 25°C?

pkb = 3.44

500

Find the pH of a solution of 0.200 M Na3PO4 where (Ka1 = 7.25 * 10-5, Ka2 = 6.31 * 10-8, Ka3 = 3.98 * 10-10). (hint: which Ka represents the most deprotonation?)

pH = 8.72

500

You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid and 0.220 M sodium benzoate. The pKa of benzoic acid is 4.20.

How many milliliters of each solution should be mixed to prepare this buffer?

22 mL benzoate

78 mL benzoic acid

500

What is the pH of a 0.17 M solution of salt KCN at 25°C? The Ka of HCN is 4.9 x 10-10.

pH = 11.27