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13 Dec 2019

You are asked to prepare a buffer with a pH of 4.66

a) Determine an appropiate acid-base combination.

b) Calculate volumes of 1.00 M solutions of the acid and base needed to produce 100 mL of the buffer.

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16 Dec 2019
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Related questions


Using the chemicals
-0.50 M HC2H3O2
-0.50 M NaC2H3O2
-0.50 M HCOOH
-0.50 M NaCOOH

Create the following buffers..
Buffer 1: Prepare 0.100 L of a pH = 3.74 buffer with a total bufferstrength of 0.100 M
Buffer 2: Prepare 0.100 L of a pH = 4.04 buffer with a total bufferstrength of 0.100 M

Show calculations of the volumes of acid and base needed to createthe two target buffers. Label which acid/base pair is used for eachbuffer system, and once volumes are found write down the volume ofwater to be added.

Helpful values: pKa for formic acid = 3.74 and for acetic acid,4.74

Steps...

-Use to calculate expected pH

pH = pKa + log([base]/[acid]

-Given the information we can fnd the ratio of base:acid for agiven buffer

[buffer] = [acid] + [base]

where the two buffer component concentrations equal the totalbuffer strength

-Finally we determine the correct volumes of the conjugateacid/base pair to give desire concentration using

m1v1=m2v2

you are asked to prepare 100. ml of 0.100 m (buffer ... Question: You are asked to prepare 100. mL of 0.100 M (buffe... You are asked to prepare 100. mL of 0.100 M (buffer concentration), pH 8.00 Tris buffer. This will be achieved by titrating a solution of tris base using 1.00 M HCl. The pKa of tris is 8.30 at 20 oC. pKa of tris changes according to the equation \DeltapKa = -0.031/oC. The temperature of the solution was found to be 23.5 oC. Therefore, the newly adjusted pKa is 8.19. Calculate the theoretical volume of HCl needed to adjust the Tris buffer to pH 8.00 at 23.5 oC (pKa 8.19), starting with the henderson-hasselbach equation. Equations to remember: pH = pKa + log10([conj. Base]/[wk. acid]) Conc.buff = Conc.wk.acid + Conc.conj.base VHCl x CHCl = Vbuff x Conc.wk.acid

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