1) What is the pH of a 0.187 M aqueous solution of potassium
fluoride, KF?
2) What is the pH of a 7.42×10-2 M aqueous solution of ammonium
nitrate, NH4NO3 ?
Please show work, I'm confused on how to solve when NO Ka or Kb
value is given in the problem!
1. An aqueous solution of potassium hydroxide is standardized by
titration with a 0.117 M solution of hydrobromic acid. If 18.7 mL
of base are required to neutralize 15.7 mL of the acid, what is the
molarity of the potassium hydroxide solution?
2. .An aqueous solution of nitric acid is standardized by
titration with a 0.183 M solution of calcium hydroxide. If 28.5 mL
of base are required to neutralize 21.4 mL of the acid, what is the
molarity of...
A) What is the pH of a
3.15×10-2 M aqueous solution of ammonium
iodide,
NH4I ?
The solution is ________. (acidic,
basic, neutral)
B)The substance benzoic acid
(C6H5COOH)
is a weak acid (Ka = 6.3×10-5).
What is the pH of a
0.101
M aqueous solution of
sodium
benzoate,
NaC6H5COO?
The solution is ________.(acidic,
basic, neutral)
1a) What is the pH of a solution of adding 10 mL of a 0.10 M
NaOH solution to pure water?
b) What is the pH of a buffered solution created by adding 10 mL
of a 0.10 M NaOH to 40
mL of a 0.15M solution of HF, Ka =6.8x10–4?
c) Buffer 1 is created such that the weak acid, HA, is 0.80 M
and base, A–, is 0.80 M. Buffer
2 is created such that the weak acid,...
1. A solution contains 1.48×10-2 M potassium sulfide and
5.38×10-3 M potassium hydroxide. Solid copper(II) nitrate is added
slowly to this mixture.
What is the concentration of sulfide ion when hydroxide ion
begins to precipitate? [sulfide] = ? M
2. A solution contains 1.21×10-2 M
potassium sulfide and
1.08×10-2 M potassium
carbonate.
Solid nickel(II) nitrate is added slowly to
this mixture.
What is the concentration of sulfide ion when
carbonate ion begins to precipitate?
[sulfide] = ? M
An aqueous solution contains 0.459 M hydrocyanic acid. How many
mL of 0.244 M potassium hydroxide would have to be added to 150 mL
of this solution in order to prepare a buffer with a pH of 9.300?
mL note in case u need this
Acid/Base Ionization Constants at 25 oC
Acid
Formula
Ka1
Ka2
Ka3
Acid/Base Ionization Constants at 25 oC
Acid
Formula
Ka1
Ka2
Ka3
Acetic acid
CH3COOH
1.8×10-5
Acetylsalicylic acid (aspirin)
HC9H7O4
3.0×10-4
Aluminum ion
Al(H2O)43+
1.2×10-5...
An aqueous solution contains 0.341 M nitrous acid. How many mL
of 0.393 M potassium hydroxide would have to be added to 150 mL of
this solution in order to prepare a buffer with a pH of 3.140?