Question
In: Chemistry
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 =
Solutions
queen_honey_blossom answered 2 years 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 0.424 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...
1) A buffer solution contains 0.356 M ammonium chloride and 0.396 M ammonia. If 0.0550 moles...
1) A buffer solution contains 0.356 M
ammonium chloride and
0.396 M ammonia.
If 0.0550 moles of hydroiodic acid are added to 250 ml
of this buffer, what is the pH of the resulting solution?
(Assume that the volume does not
change upon adding hydroiodic acid)
pH=____
2) A buffer solution contains 0.354 M
NaH2PO4 and
0.393 M
K2HPO4.
If 0.0412 moles of sodium
hydroxide are added to 225 mL of this
buffer, what is the pH of the resulting...
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...
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
1.Calculate the pH of a buffer solution that is 0.249 M in HCN and 0.175 M...
1.Calculate the pH of a buffer solution that is 0.249 M
in HCN and 0.175 M in KCN. For HCN, Ka =
4.9×10−10 (pKa = 9.31).
2.Calculate the pH of a buffer solution that is 0.210 M
in HC2H3O2 and 0.200 M in NaC2H3O2. (Ka for
HC2H3O2 is 1.8×10−5.)
3.Consider a buffer solution that is 0.50 M in NH3and
0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate
the pH of 1.0 L of the original buffer, upon addition of 0.020...
2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M ammonium iodide. If 0.16...
2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M
ammonium iodide. If 0.16 moles of hydroiodic acid 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
hydroiodic acid.)
A. The number of moles of NH3 will decrease.
B. The number of moles of NH4+ will increase.
C. The equilibrium concentration of H3O+ will increase.
D. The pH will increase.
E. The...
a. A buffer solution contains 0.274 M NH4Br and 0.379 M NH3 (ammonia). Determine the pH...
a. A buffer solution contains 0.274 M
NH4Br and
0.379 M NH3
(ammonia). Determine the pH
change when 0.103 mol
HBr is added to 1.00 L of the
buffer.
pH after addition − pH before addition = pH change
=
b. A buffer solution contains 0.432 M
NaH2PO4 and
0.209 M
K2HPO4.
Determine the pH change when
0.113 mol KOH is added to
1.00 L of the buffer.
pH after addition − pH before addition = pH change
=
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