Question

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 K_b = 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.

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 1 year ago

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.

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

Question

Buffer pH by Design Given that Kb = 5.6×10-4 for ethylamine: To prepare exactly 450 mL...

Solutions

Expert Solution

Related 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...

Buffer pH by Design Given that Kb = 1.8×10-5 for ammonia: To prepare exactly 650 mL...

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)...

Determine the pH during the titration of 31.7 mL of 0.371 M ethylamine (C2H5NH2, Kb =...

prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH ,...

You are to prepare 100 mL of a pH 3.76 buffer solution with a formal concentration...

Describe how to prepare 50 mL of solution buffered at pH 5.00. The buffer must be...

You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 4.90...