At 25 degrees Celsius all of these are true for a neutral solution : pH = 7.00, pOH = 7.00, and [H+] = [OH-] is that correct?
For a neutral, aqueous solution regardless of temperature.. would the only correct statement be [H+] = [OH-]?
pH = 7.00 and pOH = 7.00 would not be included for this when it is regardless of temperature right?
I'm a little confused by the wording. The first paragraph is true; i.e., at 25C H^+ = OH^- and pH = pOH = 7
I don't intend to change the meaning of the last two paragraphs; however, I will write it another way that makes more sense to me. At some temperature other than 25C, a neutral soln will have H^+ = OH^- but pH is not 7 and pOH is not 7 although pH = pOH.
Yes! that is what I meant by the second paragraph. So at some other temperature [H+] = [OH-] is true but pH and pOH will not be 7?
That's right, BUT pH still will be = to pOH but ti won't be 7. For example, at s temperature of 0 C, Kw = .114E-14 which makes
(H^+) = (OH^-) = sqrt Kw = 3.38E-8 so pH = 7.47 and pOH = 7.47.
I see now, THANKS!
okay... but can [H3O] = 1.0*10^-7 also be true for a neutral solution?
To understand whether the given statements are correct for a neutral solution at 25 degrees Celsius, let's break down the terms and concepts involved:
1. pH: pH is a measure of the acidity or alkalinity of a solution and is determined by the concentration of hydrogen ions ([H+]). The pH scale ranges from 0 to 14, where pH 7 is considered neutral, values below 7 are acidic, and values above 7 are alkaline or basic.
2. pOH: pOH is another measure of acidity or alkalinity, but specifically for hydroxide ions ([OH-]). It is calculated by taking the negative logarithm of the hydroxide ion concentration, similar to how pH is calculated for hydrogen ions.
3. [H+]: The concentration of hydrogen ions ([H+]) represents the acidity of a solution. In a neutral solution, the concentration of hydrogen ions is equal to the concentration of hydroxide ions ([OH-]).
Now, let's address your questions:
At 25 degrees Celsius, for a neutral solution, the concentration of hydrogen ions ([H+]) should be equal to the concentration of hydroxide ions ([OH-]), so [H+] = [OH-]. This statement is correct.
However, the values of pH and pOH being equal to 7.00 are specific to a neutral solution at 25 degrees Celsius. pH = 7.00 indicates a neutral solution where the concentration of [H+] is 10^-7 M, and pOH = 7.00 indicates a neutral solution where the concentration of [OH-] is 10^-7 M at this specific temperature.
For a neutral, aqueous solution regardless of temperature, the only correct statement would indeed be [H+] = [OH-]. Without specifying a specific temperature, we cannot determine the exact pH or pOH values.
In summary, for a neutral solution at 25 degrees Celsius, all three statements are correct: pH = 7.00, pOH = 7.00, and [H+] = [OH-]. However, if the temperature is not specified, the only correct statement for a neutral solution would be [H+] = [OH-].