Question
In: Chemistry
A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia. If 0.0297 moles of...
A buffer solution contains 0.424 M
ammonium chloride and
0.235 M
ammonia.
If 0.0297 moles of potassium
hydroxide are added to 225 mL of this
buffer, what is the pH of the resulting solution
?
(Assume that the volume change does not change upon adding
potassium hydroxide)
pH =
A buffer solution contains 0.382 M
nitrous acid and 0.466 M
potassium
nitrite.
If 0.0176 moles of hydrobromic
acid are added to 150. mL of this buffer,
what is the pH of the resulting solution ?
(Assume that the volume change does not change upon adding
hydrobromic acid)
pH =
A buffer solution contains 0.463 M
KH2PO4 and
0.305 M
Na2HPO4.
If 0.0180 moles of sodium
hydroxide are added to 150. mL of this
buffer, what is the pH of the resulting solution
?
(Assume that the volume does not change upon adding sodium
hydroxide)
pH =
Solutions
queen_honey_blossom answered 10 months agoRelated Solutions
A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia. If 0.0488 moles of...
A buffer solution contains 0.227 M
ammonium bromide and
0.427 M ammonia.
If 0.0488 moles of nitric acid
are added to 225 mL of this buffer, what is the pH
of the resulting solution?
(Assume that the volume does not change upon adding nitric
acid.)
pH =
A buffer solution contains 0.249 M ammonium bromide and 0.410 M ammonia. If 0.0196 moles of...
A buffer solution contains 0.249 M
ammonium bromide and
0.410 M ammonia.
If 0.0196 moles of nitric acid
are added to 125 mL of this buffer, what is the pH
of the resulting solution ?
(Assume that the volume change does not change upon adding
nitric acid)
pH =
To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...
To 160.0 mL of a buffer solution containing 0.250 M ammonia and
0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a)
Calculate the pH of the initial buffer solution. b) Calculate the
pH of the new solution after the addition of acid. c) What becomes
the pH if another 20.00 mL of the same acid solution is added?
To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...
To 160.0 mL of a buffer solution containing 0.250 M ammonia and
0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a)
Calculate the pH of the initial buffer solution. b) Calculate the
pH of the new solution after the addition of acid. c) What becomes
the pH if another 20.00 mL of the same acid solution is added? Pkb=
4.75
A 1.00 liter solution contains 0.45 M ammonia and 0.59 M ammonium perchlorate. If 0.150 moles...
A 1.00 liter solution contains 0.45 M
ammonia and 0.59 M
ammonium perchlorate.
If 0.150 moles of calcium
hydroxide are added to this system, indicate whether the
following statements are true or false.
(Assume that the volume does not change upon the addition of
calcium hydroxide.)
_______TrueFalse A. The number of moles of
NH3 will decrease.
_______TrueFalse B. The number of moles of
NH4+ will
increase.
_______TrueFalse C. The equilibrium
concentration of H3O+ will
increase.
_______TrueFalse D. The pH will...
A 1.00 liter solution contains 0.39 M ammonia and 0.30 M ammonium nitrate. If 0.15 moles...
A 1.00 liter solution contains 0.39 M
ammonia and 0.30 M
ammonium nitrate.
If 0.15 moles of nitric acid are
added to this system,
indicate whether the following statements are TRUE
(T) or FALSE (F).
(Assume that the volume does not change upon the addition of
nitric acid.)
A. The number of moles of
NH3 will
increase.
B. The number of moles of
NH4+ will remain the
same.
C. The equilibrium concentration of
H3O+ will increase.
D. The pH will...
A buffer solution is made by dissolving .17g of ammonia and 1.07g ammonium chloride in enough...
A buffer solution is made by dissolving .17g of ammonia and
1.07g ammonium chloride in enough water to make 250mL of
solution
Detemine molarity of ammonium chloride
Detemine ammonium concentration
Determin solution molarity relative to ammonia
Determine solution pH
a) A buffer contains significant amounts of both ammonia (NH3) and ammonium chloride (NH4Cl). Write the...
a) A buffer contains significant amounts of both ammonia (NH3)
and ammonium chloride (NH4Cl). Write the net ionic equation showing
how this buffer neutralizes added HI. Express your answer as a
chemical equation.
b)A buffer contains significant amounts of both ammonia (NH3)
and ammonium chloride (NH4Cl). Write the net ionic equation showing
how this buffer neutralizes added NaOH. Express your answer as a
chemical equation.
Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, for what reason...
Using a pH 10 buffer solution of aqueous ammonia and aqueous
ammonium chloride, for what reason are we buffering the solution to
be basic? What would happen to the structure of EDTA without a
buffer? Explain how this would affect titration.
Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, which chemical species...
Using a pH 10 buffer solution of aqueous ammonia and aqueous
ammonium chloride, which chemical species is the weak base? Which
is the conjugate acid? How do you know?
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