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In: Chemistry
Buffer pH by Design Given that Kb = 5.6×10-4 for ethylamine: To prepare exactly 450 mL...
Buffer pH by Design
Given that Kb = 5.6×10-4 for ethylamine: To prepare exactly 450 mL of a buffer solution which has a pH of 10.89 and a final ethylammonium chloride salt concentration [CH3CH2NH3+] = 0.120 M. What mass of CH3CH2NH3Cl(s), would be needed and volume of 3.00 M sodium hydroxide solution needed plus enough water to make up the total volume.
Solutions
Expert Solution
For basic buffer solution
The final concentration of salt (ethylammonium chloride) is 0.120 M
Total concentration 
Hence, we need 0.286 M ethyl ammonium chloride and 0.166 M NaOH.
Total volume 
Volume of 3.00 M NaOH required 
Number of moles of ethylammonium chloride 
Molar mass of ethyl ammonium chloride is 81.5 g/mol.
Mass of ethylammonium chloride 
queen_honey_blossom answered 2 years agoRelated Solutions
Buffer pH by Design Given that Kb = 5.6×10-4 for ethylamine: To prepare exactly 450 mL...
Buffer pH by Design
Given that Kb = 5.6×10-4 for
ethylamine:
To prepare exactly 450 mL of a buffer solution which has a pH of
10.89 and a final ethylammonium chloride salt concentration
[CH3CH2NH3+] = 0.120 M.
What mass of CH3CH2NH3Cl(s), would
be needed and volume of 3.00 M sodium hydroxide solution needed
plus enough water to make up the total volume.
Buffer pH by Design Given that Kb = 5.6×10-4 for ethylamine: To prepare exactly 450 mL...
Buffer pH by Design
Given that Kb = 5.6×10-4 for
ethylamine:
To prepare exactly 450 mL of a buffer solution which has a pH of
10.89 and a final ethylammonium chloride salt concentration
[CH3CH2NH3+] = 0.120 M.
What mass of CH3CH2NH3Cl(s), would
be needed and volume of 3.00 M sodium hydroxide solution needed
plus enough water to make up the total volume.
Buffer pH by Design Given that Kb = 1.8×10-5 for ammonia: To prepare exactly 650 mL...
Buffer pH by Design
Given that Kb = 1.8×10-5 for ammonia: To prepare exactly 650 mL
of a buffer solution which has a pH of 9.47 and a final ammonium
chloride concentration of 0.140 M, one would need to use what
(mass) of ammonium chloride, and what (volume) of 2.50 M sodium
hydroxide solution, plus enough water to make up the total
volume.
Find the [OH−] in a 0.400 M solution of ethylamine (C2H5NH2). For ethylamine, Kb=5.6×10−4.
Find the [OH−] in a 0.400 M solution of ethylamine (C2H5NH2).
For ethylamine, Kb=5.6×10−4.
a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4)...
a. Calculate the pH of a 0.538 M aqueous
solution of ethylamine
(C2H5NH2,
Kb = 4.3×10-4)
b. Calculate the pH of a 0.0473 M aqueous
solution of piperidine
(C5H11N, Kb =
1.3×10-3).
Determine the pH during the titration of 31.7 mL of 0.371 M ethylamine (C2H5NH2, Kb =...
Determine the pH during the titration of 31.7 mL of 0.371 M
ethylamine (C2H5NH2, Kb = 4.3×10-4) by 0.371 M HI at the following
points. (Assume the titration is done at 25 °C.) Note that state
symbols are not shown for species in this problem.
(a) Before the addition of any HI
(b) After the addition of 12.0 mL of HI
(c) At the titration midpoint
(d) At the equivalence point
(e) After adding 49.5 mL of HI
prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH ,...
prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and
concentrated NH4OH , the NH4OH molartiy is 18.1 M ? NH4OH is equal
to NH3 (aq)
You are to prepare 100 mL of a pH 3.76 buffer solution with a formal concentration...
You are to prepare 100 mL of a pH 3.76 buffer solution with a
formal concentration of 0.0500 F (i.e., total concentration of all
acetate species is 0.0500 M). Calculate how many grams, of acetic
acid and sodium acetate mix together.
Describe how to prepare 50 mL of solution buffered at pH 5.00. The buffer must be...
Describe how to prepare 50 mL of solution buffered at pH 5.00.
The buffer must be designed so the pH changes no more than 0.10
units with the addition of 0.001 moles of acid or base. Choose from
the following to design the buffer. Be sure to choose the buffer
pair best suited to the assigned conditions.
1.acetic acid/sodium acetate
2.formic acid/sodium formate
3. benzoic acid/sodium benzoate
please show your work-thank you!
You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 4.90...
You are asked to prepare 500. mL of a 0.150 M acetate buffer at
pH 4.90 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76),
3.00 M NaOH, and water. Answer the following questions regarding
the preparation of the buffer.
2. What volume of 3.00 M NaOH must you add to the acetic acid to
achieve a buffer with a pH of 4.90 at a final volume of 500 mL?
(Ignore activity coefficients.) Answer is not 14.5
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