You are Here: Home

# Buffer Q Watch

1. Calculate the pH of a buffer solution produced by adding 4.00g of sodium ethanoate to 1dm^3 of 0.01M ethanoic acid. The Ka of ethanoic acid is 1.84x10^-5 mol/dm^3 at 300K.

Calculate the pH of this buffer if 5cm^3 of 0.1M HCl is added.

I tried using this pka=ph-log HA/H+ but couldn't do it!

+rep
2. (Original post by arvin_infinity)
Calculate the pH of a buffer solution produced by adding 4.00g of sodium ethanoate to 1dm^3 of 0.01M ethanoic acid. The Ka of ethanoic acid is 1.84x10^-5 mol/dm^3 at 300K.

Calculate the pH of this buffer if 5cm^3 of 0.1M HCl is added.

I tried using this pka=ph-log HA/H+ but couldn't do it!

+rep
find the concentration of A- by finding the moles of ethanoate and then dividing by volume, then stick this into the Ka formula.

Spoiler:
Show

mr of sodium ethanoate = 82
n=4/82 = 0.0488mol
conc of A-= 0.0488 / 1 = 0.0488 moldm-3

Ka=[H+][A-]/[HA]
1.84x10^-5 = [H+] x 0.0488/0.01
so [H+] = 3.77x10^-6
pH = -log [H+]
so pH = 5.42

The volume of acid added in the second part is very small, so by the definition of a buffer, the pH shouldn't change.
3. (Original post by clownfish)
find the concentration of A- by finding the moles of ethanoate and then dividing by volume, then stick this into the Ka formula.

Spoiler:
Show

mr of sodium ethanoate = 82
n=4/82 = 0.0488mol
conc of A-= 0.0488 / 1 = 0.0488 moldm-3

Ka=[H+][A-]/[HA]
1.84x10^-5 = [H+] x 0.0488/0.01
so [H+] = 3.77x10^-6
pH = -log [H+]
so pH = 5.42

The volume of acid added in the second part is very small, so by the definition of a buffer, the pH shouldn't change.
Buffers do change pH only not by very much. The question is designed to show you that, but you do have to do the calculation.

moles of acid (H+) added = 0.1 x 0.005 = 0.0005

This is absorbed by the ethanoate ions increasing the moles of HA by the same amount, hence new moles of HA = 0.01 + 0.0005 = 0.0105

The ethanoate moles are decreased by the same amount = 0.0488 - 0.0005 = 0.0483 mol

1.84 x 10-5 = [H+]*0.0483/0.0105

pH = 5.40
4. (Original post by charco)
Buffers do change pH only not by very much. The question is designed to show you that, but you do have to do the calculation.

moles of acid (H+) added = 0.1 x 0.005 = 0.0005

This is absorbed by the ethanoate ions increasing the moles of HA by the same amount, hence new moles of HA = 0.01 + 0.0005 = 0.0105

The ethanoate moles are decreased by the same amount = 0.0488 - 0.0005 = 0.0483 mol

1.84 x 10-5 = [H+]*0.0483/0.0105

pH = 5.40
Just did the same method using pka=ph+log acid/salt
and I got 4.07..I checked it twice ! wondered why that is?!

EDITbs I got the equation wrong way around!

Updated: May 5, 2012
TSR Support Team

We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out.

This forum is supported by:
Today on TSR

### Grade boundaries not out until results day

What does this mean for you?

### The most OUTRAGEOUS stories from school

Poll
Study resources

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.