Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: umegard on January 17, 2007, 03:44:59 PM
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If I were to remove H+ ions from my destilled water, what would happen to the pH?
I other words, can you construct an acid/base that is just water with a non neutral pH?
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If you remove the H+, you have to replace it with another cation, and then you don't have pure water. Eg. Replace H+ with Na+ and you have a sodium hydroxide solution.
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1 - there is no such thing as 100% pure water, even triply distilled water, or the purest Millipore water has some ions / contaminants.
2 - Kw (water equilibrium (heard of it?, then apply Le Chatelier's priciple; remove the H+ and there will be made more of it from OH-, as well as water will split back up in H+ and OH- to resupply the concentration of these 2 ions)
so answer is very easily: NO
To change pH add acid or base, like sodium as Dan said
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Thanks for your answers!
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If you could selectively remove H+ from water the pH would go up obviously enough. But, the more interesting observation would be to see what a liquid with excess negative charge that is electrically isolated from its environment would do if left to its own devices.
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Kw is also dependent on temperature, if temperature is increased, Kw will also increase, and there are more OH- and H+ ions. Thus, pH will change.
However i am not sure if it increases or decreases, can anyone help me with this?
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In general Kw increases with temperature, pH of pure water goes down with temperature. I don't remember exact details and I can't locate them right now. I think CRC handbook contains table of Kw vs T.
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Kw is also dependent on temperature, if temperature is increased, Kw will also increase, and there are more OH- and H+ ions. Thus, pH will change.
However i am not sure if it increases or decreases, can anyone help me with this?
Excellent point! I'd completely forgotten about that!
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Thanks!
Hey everyone i found this,
T (°C) Kw (mol2 dm-6) pH
0 0.114 x 10-14 7.47
10 0.293 x 10-14 7.27
20 0.681 x 10-14 7.08
25 1.008 x 10-14 7.00
30 1.471 x 10-14 6.92
40 2.916 x 10-14 6.77
50 5.476 x 10-14 6.63
100 51.3 x 10-14 6.14
So in summary pH goes down as temperature increases, but the solution is not considered more acidic, as the number of OH- ions increases as well. The new pH value of pure water at the new temperature is now considered the new "neutral value".
To read up more go here : http://www.chemguide.co.uk/physical/acidbaseeqia/kw.html