You are on the right track. All you need to do is to add some NaCl.
No idea what you mean by "charge of the buffer", but it is definitely some kind of misconception you have. Buffer is not "charged", and every solution is always electrically neutral - it contains exactly the same amount of charge in positive and negative ions. NaCl that you will add is also electrically neutral.
You are on the right track. All you need to do is to add some NaCl.
No idea what you mean by "charge of the buffer", but it is definitely some kind of misconception you have. Buffer is not "charged", and every solution is always electrically neutral - it contains exactly the same amount of charge in positive and negative ions. NaCl that you will add is also electrically neutral.
Hm, I think I see what I did wrong; I was focussing more on the context of Na+ versus NaCl.
One more question -- with the addition of more NaCl, how would this affect your phosphate ions? Because if you solely add in more NaCl, would you not technically have the same amount of Na+ interacting with the phosphate...? If this is the case, I'm not entirely clear how this would affect the ionic strength of the buffer, unless I can assume that NaCl completely dissociates? Sorry, I'm not really sure what to make of it.
Thanks for the response, though -- it's appreciated.
Hm, I think I see what I did wrong; I was focussing more on the context of Na+ versus NaCl.
One more question -- with the addition of more NaCl, how would this affect your phosphate ions? Because if you solely add in more NaCl, would you not technically have the same amount of Na+ interacting with the phosphate...? If this is the case, I'm not entirely clear how this would affect the ionic strength of the buffer, unless I can assume that NaCl completely dissociates? Sorry, I'm not really sure what to make of it.
Thanks for the response, though -- it's appreciated.
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VOTE
No idea what you mean by "charge of the buffer", but it is definitely some kind of misconception you have. Buffer is not "charged", and every solution is always electrically neutral - it contains exactly the same amount of charge in positive and negative ions. NaCl that you will add is also electrically neutral.
No idea what you mean by "charge of the buffer", but it is definitely some kind of misconception you have. Buffer is not "charged", and every solution is always electrically neutral - it contains exactly the same amount of charge in positive and negative ions. NaCl that you will add is also electrically neutral.
More
VOTE
One more question -- with the addition of more NaCl, how would this affect your phosphate ions? Because if you solely add in more NaCl, would you not technically have the same amount of Na+ interacting with the phosphate...? If this is the case, I'm not entirely clear how this would affect the ionic strength of the buffer, unless I can assume that NaCl completely dissociates? Sorry, I'm not really sure what to make of it.
Thanks for the response, though -- it's appreciated.
One more question -- with the addition of more NaCl, how would this affect your phosphate ions? Because if you solely add in more NaCl, would you not technically have the same amount of Na+ interacting with the phosphate...? If this is the case, I'm not entirely clear how this would affect the ionic strength of the buffer, unless I can assume that NaCl completely dissociates? Sorry, I'm not really sure what to make of it.
Thanks for the response, though -- it's appreciated.
More
VOTE