PH Scale. Baisc, Neutral Or Acidic?
acidic
26. On the pH scale, a solution with a concentration of H3O+ equal to 6.2 x 10-6 is considered__________. basic neutral
acidic
27. On the pH scale, a solution with a concentration of H3O+ equal to 5.1 x 10-13 is considered__________. basic neutral
acidic
28. On the pH scale, a solution with a concentration of H3O+ equal to 5 x 10-8 is considered__________. basic neutral
acidic
29. On the pH scale, a solution with a concentration of OH- is equal to 4.9 x 10-13 is considered__________. basic neutral
acidic
30. On the pH scale, a solution with a concentration of OH- equal to 3.2 x 10-8 is considered__________. basic neutral
acidic
please show me how this is done as well as the answers if you would so oblige. Thanks!
Answer:
neutral
acidic
basic
basic
acidc
acidic
If the pH = 7 then its neutral
if its between 0 and 6.9 then its acidic
If its between 7.1 and 14 then its basic
pH = -log[H3O+]
So just plug in the value they give you for the H3O+ and you get the pH
For the OH-
pOH = -log[OH-]
Then once you have the pOH, do: 14-pOh
and you have your pH
sorry, I can only tell you how to do it, not the answers!
water equilibrium constant = [H3O+] [OH-]
then you know that the pH is a log scale: pH = -log ([H3O+])
when you are given an OH- concentration, calculate the [H3O-] by rearranging the the first equation!
pH = 7 --> neutral
pH > 7 --> basic
pH< 7 --> acidic
you probably won't need to do the calculations every time... you might manage to spot a pattern.
hope this helps!
The pH scale is nothing more than a logarithmic expression of H+ concentration. A solution is acidic if the concentration of H+ (H3O+) is greater than 10-7 M, basic if less than 10-7 M and neutral at 10-7 M. Or thereabouts, you might also say anywhere between 10-6 and 10-8 M H+ is "neutral", but that is a subjective definition.
The concentration of H+ is also related to the OH- concentration in that [H+] x [OH-] = 10-14.
Those two definitions should make the answers readily apparent.
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