Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature.
Solution
Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature..
ĐỀ THAM KHẢO KÌ THI TUYỂN SINH VÀO LỚP 10 MÔN TIẾNG ANH FORM 50 CÂU TRẮC NGHI...
Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We.pdf
1. Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature.
Solution
Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature.
![Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature.
Solution
Kw= [H+][OH-] =1x10^-14 at 25 degrees celsius. We know this is true. Therefore
because this statement is true: (1x10^-14)/[OH-] = [H+]. Therefore, if the [OH-] is less than
1x10^-7 (when the ph would equal 7, neutral) , the [H+] will be greater than 1x10^-7. Therefore,
when calculating ph (-log[H+]) the ph will be lower than 7. Therefore H2O can act as a weak
acid. It cant be strong because because, remember, the autoionization of water is very very small,
rapid and constantly going back and forth. Whereas, in a strong acid, there is complete
ionization. Therefore, the answer is B, because kw does change with temperature.](https://image.slidesharecdn.com/kwhoh-1x10-14at25degreescelsius-230408052659-b5ff1e5d/85/Kw-H-OH-1x10-14-at-25-degrees-celsius-We-pdf-1-320.jpg)
