Which base is the strongest for the given [H+]?
A)10^-9
B)10^-11
C)10^-10
D)10^-12
(H^+)(OH^-) = 1E-14
So smaller H^+ means higher OH^-
or
higher H^+ means lower OH^-
To determine which base is the strongest for the given [H+], you need to understand the concept of pH and pOH.
pH is a measure of the concentration of hydrogen ions ([H+]) in a solution. It is defined as the negative logarithm (base 10) of the hydrogen ion concentration: pH = -log[H+].
pOH, on the other hand, is a measure of the concentration of hydroxide ions ([OH-]) in a solution. It is defined as the negative logarithm (base 10) of the hydroxide ion concentration: pOH = -log[OH-].
In neutral solutions, the product of the hydrogen ion concentration and the hydroxide ion concentration is always equal to 1 x 10^-14 at 25°C. This relationship can be represented as [H+][OH-] = 1 x 10^-14.
For a given [H+], you can calculate the pOH using the following equation: pOH = 14 - pH.
Now let's calculate the pH and pOH for each option to determine which base is the strongest:
A) [H+] = 10^-9
pH = -log(10^-9) = -(-9) = 9
pOH = 14 - 9 = 5
B) [H+] = 10^-11
pH = -log(10^-11) = -(-11) = 11
pOH = 14 - 11 = 3
C) [H+] = 10^-10
pH = -log(10^-10) = -(-10) = 10
pOH = 14 - 10 = 4
D) [H+] = 10^-12
pH = -log(10^-12) = -(-12) = 12
pOH = 14 - 12 = 2
From the calculations, we can see that option D has the highest pH value (12), which means it has the lowest [H+] concentration. Since higher pH corresponds to lower acid concentration, option D (10^-12) represents the strongest base among the given choices.