Question
In: Chemistry
Now that the acid has been standardized and you know it is 0.2496 M H2SO4, you...
Now that the acid has been standardized and you know it is 0.2496 M H2SO4, you perform the actual experiment as follows:
A 3.100-g sample of meat is subjected to Kjeldahl analysis. The
liberated NH3(g) is absorbed by adding 50.00 mL of H2SO4(aq), which
is more than enough. The excess acid requires 19.90 mL of 0.5510 M
NaOH for its complete neutralization.
What is the percentage of protein in the meat?
Solutions
queen_honey_blossom answered 4 hours agoRelated Solutions
If 100 mL of 1.0 M sulfuric acid, H2SO4, is neutralized with 1.0 M calcium hydroxide,...
If 100 mL of 1.0 M sulfuric acid, H2SO4, is neutralized with 1.0
M calcium hydroxide, Ca(OH)2, how many mL of base must be
added?
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid [H2SO4] from an 18...
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid
[H2SO4] from an 18 M concentrated sulfuric acid stock solution.
3. Describe how you would prepare 50 ml of 0.2 M potassium
iodate [KIO3] dissolved in the 0.08 M sulfuric acid [H2SO4] that
you have prepared above.
4. Describe how you would prepare 25 ml of 3.6 M hydrogen
peroxide [h2O2] from a 30% (w/w) stock H2O2 solution (
5. Describe how you would prepare 50 ml of...
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid [H2SO4] from an 18...
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid
[H2SO4] from an 18 M concentrated sulfuric acid stock solution.
3. Describe how you would prepare 50 ml of 0.2 M potassium
iodate [KIO3] dissolved in the 0.08 M sulfuric acid [H2SO4] that
you have prepared above.
4. Describe how you would prepare 25 ml of 3.6 M hydrogen
peroxide [h2O2] from a 30% (w/w) stock H2O2 solution (
5. Describe how you would prepare 50 ml of...
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid [H2SO4] from an 18...
2. Describe how you would prepare 100ml of 0.08 M sulfuric acid
[H2SO4] from an 18 M concentrated sulfuric acid stock solution.
3. Describe how you would prepare 50 ml of 0.2 M potassium
iodate [KIO3] dissolved in the 0.08 M sulfuric acid [H2SO4] that
you have prepared above.
4. Describe how you would prepare 25 ml of 3.6 M hydrogen
peroxide [h2O2] from a 30% (w/w) stock H2O2 solution (
5. Describe how you would prepare 50 ml of...
20. An aqueous solution of nitric acid is standardized by titration with a 0.162 M solution...
20. An aqueous solution of nitric acid is standardized by
titration with a 0.162 M solution of potassium hydroxide. If 27.1
mL of base are required to neutralize 20.7 mL of the acid, what is
the molarity of the nitric acid solution? M nitric acid
Sulfuric acid, H2SO4, is somewhat unique in that it is a diprotic acid but it is...
Sulfuric acid, H2SO4, is somewhat unique in that it is a
diprotic acid but it is also a strong acid. Thefirst dissociation
of H2SO4 is as a strong acid, and is thus a complete dissociation.
However, thesecond dissociation of H2SO4 is as a weak acid. Unlike
with other polyprotic acids, you cannotneglect the second
dissociation of H2SO4 because it will impact the pH of the
solution.
Determine the pH and the concentrations of all aqueous species
(H
+
, OH...
Now that you have been in college for some time you may have know other students,...
Now that you have been in college for some time you may have
know other students, who have left school. Some may have
transferred, and others dropped out. How can you be different from,
them and survive the challenges many college students face ? Read
the article:Toward a Theory of Minority Student
Participation In Predominantly White Colleges and Universities
by Kenneth P. Gonzalez- located in Course Documents
252 mL of 3,00 M H2SO4 are added to 1,50 L of 0,500 M H2SO4. What...
252 mL of 3,00 M H2SO4 are added to 1,50 L of 0,500 M H2SO4.
What is the concentration of the resulting solution?)
Part A Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4....
Part A Suppose that a fully charged lead-acid battery contains
1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in
the battery after 3.80 A of current is drawn from the battery for
7.00 hours ? Express your answer with the appropriate units.
pH of Aqueous Sulfuric Acid Calculate the pH of a 2.07×10-3 M solution of H2SO4. (Ka...
pH of Aqueous Sulfuric Acid Calculate the pH of a 2.07×10-3 M
solution of H2SO4. (Ka = 0.0120 for HSO4-)
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