Question
In: Chemistry
An aqueous solution contains 0.352 M methylamine (CH3NH2). How many mL of 0.309 M hydrobromic acid...
An aqueous solution contains 0.352 M
methylamine
(CH3NH2).
How many mL of 0.309 M hydrobromic
acid would have to be added to 150 mL of
this solution in order to prepare a buffer with a pH of
10.600.
Solutions
queen_honey_blossom answered 6 months agoRelated Solutions
43.An aqueous solution of methylamine (CH3NH2) has a pH of 10.65. How many grams of methylamine...
43.An aqueous solution of methylamine
(CH3NH2)
has a pH of 10.65. How many grams of methylamine are there
in
100.0 mL
of the solution?
_____g
Calculate the pH and percent ionization of a 0.990 M HNO2
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An aqueous solution contains 0.419 M ammonia (NH3). How many mL of 0.305 M perchloric acid...
An aqueous solution contains 0.419 M
ammonia (NH3).
How many mL of 0.305 M perchloric
acid would have to be added to 150 mL of
this solution in order to prepare a buffer with a pH of
9.380.
mL
An aqueous solution contains 0.459 M hydrocyanic acid. How many mL of 0.244 M potassium hydroxide...
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...
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?
An aqueous solution contains 0.480 M acetic acid. How many mL of 0.327 M potassium hydroxide...
An aqueous solution contains 0.480 M acetic acid. How many mL of
0.327 M potassium hydroxide would have to be added to 250 mL of
this solution in order to prepare a buffer with a pH of 4.680?
(please explain. thank you!)
50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride (CH3NH3Cl)...
50. mL 2.0 M methylamine (CH3NH2) solution
and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The
Kb for methylamine is 4.4 x
10-4.
What is the pH of the resulting solution after adding 100 mL of
1.0 M KOH to the original buffer solution?
11.12
b)
10.64
c)
12.32
d)
0.48
e) 5.32
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared:
50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of 2.0 M
methylamine hydrochloride (CH3NH3Cl) solution. The Kb for
methylamine is 4.4 x 10-4.
What is the pH of the resulting solution after adding 100 ml of
1.0 M HCl to the original buffer solution?
a) 11.12 b) 10.64 c) 12.32 d) 0.48 e) 5.32
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared:
50. mL 2.0 M methylamine (CH3NH2) solution
and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The
Kb for methylamine is 4.4 x
10-4.
A. What is the pH of the resulting solution after adding 200 ml
of 1.0 M HCl to the original buffer solution?
a)11.12
b)
10.64
c)
12.32
d) 0.48
e) 5.32
B.What is the pH of the resulting solution after adding 50 mL of
1.0 M KOH to the...
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared: 50. mL 2.0 M methylamine
(CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The Kb for methylamine is 4.4 x 10-4. What is
the pH of the resulting solution after adding 100 mL of 1.0 M KOH
to the original buffer solution?
The following buffer was prepared: 50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of...
The following buffer was prepared: 50. mL 2.0 M methylamine
(CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride
(CH3NH3Cl) solution. The Kb for methylamine is 4.4 x 10-4
What is the pH of the resulting solution after adding 100mL of
1.0M HCl to the original buffer solution?
A) 11.12 B) 10.64 C) 12.32 D) 0.48 E) 5.32 (Correct Answer:
5.32) Please show work, and explain why.
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