How many more [H+] are there in a sol’n
of pH2 than pH6?
my guess is 10,000 because ph is a log scale but that seems off
To determine how many more [H+] ions there are in a solution at pH 2 compared to pH 6, we need to understand the relationship between pH and the concentration of hydrogen ions ([H+]).
The pH scale is a logarithmic scale that measures the acidity or alkalinity of a solution. The pH scale ranges from 0 to 14, where a pH of 7 is considered neutral, below 7 is acidic, and above 7 is alkaline.
The formula to calculate pH is: pH = -log[H+], where [H+] represents the concentration of hydrogen ions in moles per liter.
Since pH 2 is more acidic than pH 6, we can conclude that the [H+] concentration at pH 2 is higher. To find out how many more [H+] ions there are at pH 2 compared to pH 6, we can use the formula:
[H+]2 = 10^(-pH2) and [H+]6 = 10^(-pH6)
Substituting the given pH values, we have:
[H+]2 = 10^(-2) and [H+]6 = 10^(-6)
Calculating these values, we get:
[H+]2 = 0.01 and [H+]6 = 0.000001
To determine the difference, we subtract the smaller value from the larger value:
[H+]2 - [H+]6 = 0.01 - 0.000001 = 0.009999
Therefore, there are 0.009999 moles per liter (or 9.999 x 10^(-3) M) more [H+] ions in a solution at pH 2 compared to pH 6.