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Buffer Solutions |
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| Nov29-04, 07:22 AM | #1 |
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Buffer Solutions
I am very stuck on this question and I am hoping someone can help me with this. We did this in lab and mine did not come out right, but I still have to turn it in and my lab teacher said to figure it out!
Buffer solutions using a cabbage dye indicator: Which of these is a buffered solution after the addition of 5 drops of HCl, 10 drops HCl: distilled water (I think no?) 0.1 M NaCl pH 12 buffer pH 2 buffer Which if these is a buffered solution after 5 drops NaOH, 10 drops NaOH: juice(pH around 4.5) soda(pH around 3) pH 12 buffer pH 2 buffer I know this is a loaded question, but I can't figure out which ones...HELP!!! |
| Nov29-04, 09:51 AM | #2 |
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Hi pinky, a buffer is a solution that contains a mixture of acids and bases.. if an acid or base is added to the solution the pH won't change. If you add a solution to a buffer outside it's buffering range, the buffer will loose it's power.
So thinking of that, which do you think the correct answer will be to your own question? Hint: what is the approximate pH of HCl and NaOH? |
| Nov29-04, 03:27 PM | #3 |
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HCl is a pH 2 and NaOH is about pH-13-14 right? So, pH 2 is a buffer solution when HCl is added and not when NaOH is right? The rest I am still lost on!?
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