Question
In: Chemistry
A.) Calculate the pH of 1.0 L of the solution, upon addition of 49.00 mL of...
A.) Calculate the pH of 1.0 L of the solution, upon addition of 49.00 mL of 1.0 MHCl.
Calculate the pH of the solution upon addition of 19.1 mL of 1.00 MHCl to the original buffer
B.)For each of the following solutions, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
1.) 300.0 mL of pure water
2.)300.0 mL of a buffer solution that is 0.210 M in HCHO2 and 0.290 M in KCHO2
3.)300.0 mL of a buffer solution that is 0.295 M in CH3CH2NH2 and 0.270 M in CH3CH2NH3Cl
Solutions
queen_honey_blossom answered 3 months agoRelated Solutions
1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of...
1) Calculate the pH of 1.0 L of the solution upon addition of
0.010 mol of solid NaOH to the original buffer solution.
2) Calculate the pH of 1.0 L of the solution upon addition of
30.0 mL of 1.0 MHCl to the original buffer solution.
3) A 1.0L buffer solution contains 0.100 molHC2H3O2 and 0.100
molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.
3A) Calculate the pH of the solution upon the addition of 0.015
mol of NaOH...
Calculate the pH of 1.0 L upon addition of 0.190 mol of solid NaOH to the...
Calculate the pH of 1.0 L upon addition of 0.190 mol of solid
NaOH to the original buffer solution. Express the pH to two decimal
places. Consider a buffer solution that is 0.50 M in NH3
and 0.20 M in NH4Cl. For ammonia, pKb=4.75.
Which solution would show the least change in pH upon addition of 3.0 mL of 1.0...
Which solution would show the least change in pH upon addition
of 3.0 mL of 1.0 M KOH? Assume equal volumes of each solution are
used. Ka for CHO2H =
1.80 ✕ 10−4)
a. A solution that is 0.50 M formic acid and 0.50 M sodium
formate.
b. A solution that is 0.10 M formic acid and 0.10 M sodium
formate.
c. A solution that is 0.1 M formic acid
d. A solution that is 0.50 M sodium formate
Calculate the final pH of a solution made by the addition of 10 mL of a...
Calculate the final pH of a solution made by the addition of 10
mL of a 0.5 M NaOH solution to 500 mL of a weak acid, HA. The
concentration of the conjugate acid is 0.2M, the pH is 5.00 and
thepKa = 5.00. Neglect the change in volume. (This is all of the
information that was given.)
a.6.10
b. 5.04
c. 7.00
d. 5.99
e. 6.91
a) Calculate the pH of 75 mL of the undiluted buffer solution after the addition of...
a) Calculate the pH of 75 mL of the undiluted buffer solution
after the addition of 1 mL of 3 M HCl.
b) Calculate the pH of 75 mL of the undiluted buffer solution
after the addition of 15 mL of 3 M HCl.
Buffer solution was made from 1 M of sodium acetate, and 1.1005
M of acetic acid. (pKa of acetic acid 4.75). pH of buffer =
4.79.
Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M...
Calculate the pH of the solution resulting from the addition of
10.0 mL of 0.10 M NaOH to 50.0 mL of a 0.10 M solution of aspirin
(acetylsalicic acid, Ka = 3.0 × 10–4)
solution.
A.
2.9
B.
10.5
C.
4.1
D.
3.5
E.
1.8
Calculate the pH of a buffer solution after the addition of 20.0 mL of 0.200 M...
Calculate the pH of a buffer solution after the addition of 20.0
mL of 0.200 M NaOH to 80.0 mL of 0.0500 M HC3H5O2 and 0.0250 M
NaC3H5O2. (Ka = 1.4 x 10^-5)
Find the pH of a solution prepared from 1.0 L of a 0.20 M solution of...
Find the pH of a solution prepared from 1.0 L of a 0.20
M solution of Ba(OH)2 and excess
Zn(OH)2(s). The Ksp of Zn(OH)2 is
3×10−15 and the Kf of
Zn(OH)42− is 2×1015.
calculate the ph of 1.0 l of a buffer that is .01 m of HNO2 and...
calculate the ph of 1.0 l of a buffer that is .01 m of HNO2 and
.15 m NaO2. what is the ph of the same buffer and after the additon
of 1.0 l of 12m hcl (pka of HNO2 is 3.4)
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl...
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0
M HCl (aq)
I know this question is pretty simple, but do I need
to know what the buffer is made of? Is it important? if not how
would I set up the ICE table? thank you!
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