Question
In: Chemistry
A student was given buffer solutions to calibrate the pH electrode that were labeled incorrectly. The...
A student was given buffer solutions to calibrate the pH electrode that were labeled incorrectly. The pH's of both buffer solutions were actually lower than the pH's shown on the labels. Explain how such an error would affect the experimental result for the Ka of acetic acid.
Solutions
queen_honey_blossom answered 2 months agoRelated Solutions
Say you are given a buffer at 25 C in pH 6.881. The glass combination electrode...
Say
you are given a buffer at 25 C in pH 6.881. The glass combination
electrode gave a reading of -18.3 mV. When it was placed in a pH
4.002 buffer at 25 C, this same electrode gave a reading of +146.3
mV. What is the electromotive efficiency of the glass electrode? (3
sig figs)
Three flasks, labeled A, B, and C, contained aqueous solutions of the same pH. It was...
Three flasks, labeled A, B, and C, contained aqueous solutions
of the same pH. It was known that one of the solutions was 1.0 ×
10–3 M in nitric acid, one was 6 × 10–3 M in formic acid, and one
was 4 × 10–2 M in the salt formed by the weak organic base aniline
with hydrochloric acid (C6H5NH3Cl). (Formic acid is
monoprotic.)
(a) Describe a procedure for identifying the solutions.
(b) Compare qualitatively (on the basis of the...
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.969 g...
Calculate the pH of the following buffer solutions: (a) a
solution made by dissolving 4.969 g KH2PO4 and 1.757 g K2HPO4 in
water to give 200. mL of solution. Stepwise acid dissociation
constants for phosphoric acid may be found in your textbook. (b) a
solution made by mixing 10.00 mL 0.29 M (CH3)2NH with 40.00 mL 0.17
M (CH3)2NH2Cl. The base dissociation constant Kb is 7.40 x 10-4 for
(CH3)2NH. Assume that the final volume is the sum of the...
You have the following solutions at your disposal to prepare a buffer solution with a pH...
You have the following solutions at your disposal to prepare a
buffer solution with a pH greater than 7.0:
(1) 50.0 mL of 0.35 M NH3 Kb = 1.8×10-5 (2) 55.0 mL
of 0.35 M NaOH
(3) 50.0 mL of 0.35 M HCl (4) 16.5 mL of 0.35 M NaCl NaOH
(5) 16.5 mL of 0.35 M HNO3 (6) 16.5 mL of 0.35 M KOH
(a) Assuming that you are going to mix the entire quantity of
the listed solutions to...
Buffers are solutions that resist changes in pH. find a "common" buffer system and explain what...
Buffers are solutions that resist changes in pH. find a "common"
buffer system and explain what the buffering components are.
post should be a minimum of 150 words
No hand writing please
500ml of an HTS/TS- buffer (pKa = 5.25) at pH 4 was prepared. Unfortunately, the student...
500ml of an HTS/TS- buffer (pKa = 5.25) at pH 4 was prepared.
Unfortunately, the student who had prepared the buffer forgot how
many moles of HTS and TS- he had added. Although HTS does not
fluoresce, TS- does fluoresce. (If = 1000CTS). The intensity of the
fluorescence signal from the buffer is 10. How many moles of HTS
and TS- were used to prepare 500ml of the pH 4 buffer?
A student must make a buffer solution with a pH of 1.00. Determine which weak acid...
A student must make a buffer solution with a pH of 1.00.
Determine which weak acid is the best option to make a buffer at
the specified pH.
formic acid,Ka = 1.77 x 10−4,
2.00 M
sodium bisulfate monohydrate, Ka = 1.20 x
10−2, 3.00 M
acetic acid, Ka = 1.75 x 10−5,
5.00 M
propionic acid, Ka =1.34 x 10−5,
3.00 M
Determine which conjugate base is the best option to make a buffer
at the specified pH.
sodium...
a) You have to prepare a pH 5.25 buffer from the following 0.100 M solutions available:...
a) You have to prepare a pH 5.25 buffer from the following 0.100
M solutions available:
1. hydrocyanic acid
2. hypobromous acid
3. propanoic acid
4. potassium cyanide
5. potassium hypobromite
6. potassium propanoate
Which solutions would you choose to make the most effective
buffer? Why?
b) How many milliliters of each of each o the solutions selected
in part a would you use to make one liter of the final buffer
solution?
You have to prepare a ph 3.50 buffer, and you have the following 0.10M solutions available:...
You have to prepare a ph 3.50 buffer, and you have the following
0.10M solutions available: HCOOH, CH3COOH,H3PO4,HCOONa, CH3COONa,
and NAH2PO4. Which solutions would you use? How many milliliters of
each solution would you use to make approximately a liter of the
buffer?
The answer on the textbook is 360mL of 0.10M HCOONa and 630mL of
0.10M HCOOH. I just need to know how did they get that answer.
The Determination of Magnesium by Direct Titration Preparation of Solutions: Buffer solution, pH 10: Diluted 57mL...
The Determination of Magnesium by Direct Titration
Preparation of Solutions:
Buffer solution, pH 10: Diluted 57mL of NH3 and 7g
NH4Cl totaling 100mL solution
Eriochrome Black T: Dissolved 102.4mg in 15mL ethanolamine and
5mL of absolute ethanol
EDTA: 3.8008g of purified dihydrate Na2H2Y
2H2O, mixed with distilled water to total volume of
1L
I received a Magnesium Sulfate unknown, and diluted it to 500mL
with distilled water then transferred 3 50mL aliquots to separate
conical flasks and added 2mL of...
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