Destroyer Gchem question
Started by yankees27th
pH is based on concentration of H+ ions and nothing else. It doesn't matter if there is 1000 molar OH- in the solution.
Hence, a lot of H+ and a lot of OH- is read only as a lot of H+. Aka acidic.
But if you find the pOH and then subtract that from 14 don't you get that it's basic?
I think the 14 only applies at room temp.
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Actually, the water is neither acidic nor basic. It's neutral. [H+][OH-]=Kw. The pH ithe negative log of the [H+]. Thus, at Kw=1*10^-14, the H+ OH- concentrations would both be 1*10^-7, and the pH and pOH would be 7. In our case, the Kw is 5*10^-14 and thus the [H+] and [OH-] would each be 2.2*10^-7, making the pH and the pOH both 6.65.
Remember, acidic means that there is more H+ than OH-. If they are equivalent, it is neutral no matter what the pH is. pH=7 is neutral only when Kw=1*10-14.
Remember, acidic means that there is more H+ than OH-. If they are equivalent, it is neutral no matter what the pH is. pH=7 is neutral only when Kw=1*10-14.
Is that the official definition of acidic? If so, then I don't know what to say.
dont forget that "acid" has 3 definitions... Arrenheus, Bronsted-Lowry, and Lewis. so make sure that u know the differences
Thats correct, just be able to differentiate between them.
correct. three defifntions. one is with the H and OH. the othr is with the dots moving. and the other one also is with the H and OH.
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