Question
In: Chemistry
In the buffer portion of the lab, you compared how water and a buffer solution react...
- In the buffer portion of the lab, you compared how water and a buffer solution react to the addition of base (NaOH) and acid (HCl). Based on your observations, which seems to have greater “buffering capacity” (ability to maintain a consistent pH): the distilled water or the buffer?
- The buffer solution consisted of acetic acid and sodium acetate (of which, the acetate ion is the important species). Of this mixture, the weak acid is _____ _____ and its conjugate base is ___ ________.
- Which component of this buffer system (listed in question #2) reacted with the added sodium hydroxide? Acetic acid
Write an equation that represents this reaction.
- Which component of this buffer system (listed in question #2) reacted with the added hydrochloric acid? acetic acid
Write an equation that represents this reaction.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components:
3.46 g of
NaC2H3O2∙3H2O (FW. 136
g/mol)
9.0 mL of 3.0 M HC2H3O2
55.0 mL of water
If you take half of this solution and add 2 mL of 1.00 M NaOH to
it, then what is the pH of this new solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M
HC2H3O2 55.0 mL of water If you take half of this solution and add
2 mL of 1.00 M HCl to it, then what is the pH of this new
solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the
one you made in the lab was prepared using the following
components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M
HC2H3O2 55.0 mL of water If you take half of this solution and add
2 mL of 1.00 M HCl to it, then what is the pH of this new
solution?
FLUORIMETER LAB: A 0.1019 g portion of an aspirin tablet was dissolved in sufficient water to...
FLUORIMETER LAB:
A 0.1019 g portion of an aspirin tablet was dissolved in
sufficient water to prepare 1.000 L of solution. A pipet was used
to transfer 10.00 mL of the solution to a 100.00 mL volumetric
flask. A 2.00 mL portion of 4 M NaOH (aq) was added to the flask,
and the resulting solution was diluted to the mark with water. The
fluorescence of the diluted sample solution was found, by the
working curve method, to correspond to...
Describe how you would prepare 2 mL of solution containing NaCl, MES buffer, and water. NaCl...
Describe how you would prepare 2 mL of solution containing NaCl,
MES buffer, and water. NaCl stock solution is 1M and the working
concentration required is 5mM. MES buffer stock solution is 100 M
and the working concentrations required is 20 mM. To make 2 mL of
solution calcualte the amount of water you would add.
Please Show Work
1. How can you tell if a solution is a good buffer or not? 2. What...
1. How can you tell if a solution is a good buffer or not?
2. What would happen if you messed up the 1st level
of protein organization? What would the effects be?
3. Using the abbreviated periodic table, how can you quickly
figure out how many electrons, valence electrons, and energy levels
an element has?
4. How does the number of valence electrons impact covalent
bonding? Use an example. (hint: octet/duet rule)
Biochem Lab: Explain the basis for the stacking gel portion of a polyacrylamide gel. Describe how...
Biochem Lab: Explain the basis for the stacking gel portion of a
polyacrylamide gel. Describe how it works with respect to the
loaded protein samples as well as the running buffer
components.
Assume you have successfully made a buffer solution, such that you have 0.250 M phosphate buffer...
Assume you have successfully made a buffer solution, such
that you have 0.250 M phosphate buffer at pH 7.2. You dissolve in
this solution sufficient
histidine (side chain pKa = 6.0), such that the final histidine
concentration is 5 mM, all at 25°C.
Therefore, the pH of the solution is controlled by the phosphate
buffer. In this solution, what is
the percent of histidine with a protonated side chain? What is the
total charge on molecules in
this fraction? Explain.
How you would prepare a 500 mL solution of 0.1M "tris" buffer at pH of 7.5...
How you would prepare a 500 mL solution of 0.1M "tris" buffer at
pH of 7.5 starting with solid tris free base. The free base has a
chemical forumla of (HOCH2)3-C-NH2 and a MW of 121.1 g/mol. The
protonated amine form, tris-chloride, has a pKa of 8.10. To prepare
the solution, 1.0M HCl will be used.
Show how would you prepare a solution of 500 ml of a 0.15 M acetate buffer....
Show how would you prepare a solution of 500 ml of a 0.15 M
acetate buffer. You have available the following: 6M HCl, 4 M
acetic, solid sodium acetate, solid sodium hydroxide
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