Question A solution of pH 7 compared to a solution of pH 9? Help!!
A. is more basic.
B. has no OH- ions
C. has more H+ ions.
D. has a higher pH.
E. all of the choices are correct.What is pH?
Answer:
A. is more basic.
B. has no OH- ions
C. has more H+ ions.
D. has a higher pH.
E. all of the choices are correct.What is pH?
Answer:
It is the negative of the log of the hydrogen (H+) concentration, or [H=}.
pH=7 or -log[H+]=7 or log[H+]=-7, take antilog of both sides, [H+]=10^-7
So a pH 7 has 10^-7 H+ ions, while a pH 9 has 10^-9 H+ ions. remember that -9 is smaller than -7, so ph9 has fewer H+ ions than pH 7.
So the pH 7 has more H+ions, it is more acidic (acids are less than ph7, bases are greater than pH7)
you know D (and therefore E) are wrong because pH 7 is lower pH than pH 9.
we can't say whether B is corrrect or not, because we don't know for sure if it's an aqeous solution, which OH- as counterions to the H+ (but it likely is aquous and both have OH- ions)
It is not more basic, because the lower the pH, the higher the concentrasion of H+ ions, and the more acidic.
pH=7 or -log[H+]=7 or log[H+]=-7, take antilog of both sides, [H+]=10^-7
So a pH 7 has 10^-7 H+ ions, while a pH 9 has 10^-9 H+ ions. remember that -9 is smaller than -7, so ph9 has fewer H+ ions than pH 7.
So the pH 7 has more H+ions, it is more acidic (acids are less than ph7, bases are greater than pH7)
you know D (and therefore E) are wrong because pH 7 is lower pH than pH 9.
we can't say whether B is corrrect or not, because we don't know for sure if it's an aqeous solution, which OH- as counterions to the H+ (but it likely is aquous and both have OH- ions)
It is not more basic, because the lower the pH, the higher the concentrasion of H+ ions, and the more acidic.
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