# Buffer solutions and concentration change question.Watch

Thread starter 1 year ago
#1
Okay so in my mock, I've had a problem understanding this question:

"When the student prepares the buffer solution, the volume of solution increases slightly.

Suggest whether the pH of the buffer solution would be the same,greater than or less than your calculated value. Explain your reasoning."

So you're told the buffer solution has a pH of 4.50

I put that an increase in volume would decrease the amount of Hydrogen ions which would increase the ph but apparently it remains the same?

could anybody tell me why?
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1 year ago
#2
it's a buffer solution which means it resist a pH change when a relatively small quantity of volume of acid/alkali is added to it.
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Thread starter 1 year ago
#3
(Original post by BTAnonymous)
it's a buffer solution which means it resist a pH change when a relatively small quantity of volume of acid/alkali is added to it.
yeah but i am not adding acid or alkali, im making the buffer solution. How would the buffer's ph remain unchanged if the volume does increase?
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1 year ago
#4
(Original post by Appazap)
yeah but i am not adding acid or alkali, im making the buffer solution. How would the buffer's ph remain unchanged if the volume does increase?
ah.

well pH is dependant on the concentration of H+ ions, not the quantity of hydrogen ions. so when making the buffer solution, the concentration of H+ ions remain the same.
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Thread starter 1 year ago
#5
(Original post by BTAnonymous)
ah.

well pH is dependant on the concentration of H+ ions, not the quantity of hydrogen ions. so when making the buffer solution, the concentration of H+ ions remain the same.
Okay that makes a lot of sense, thank you xx
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