Household ammonia has a pH of 11, therefore its H+ concentration is how many times less than a solution with a pH of 7?
1000
To determine the H+ concentration in household ammonia compared to a solution with a pH of 7, we need to understand the concept of pH and its relation to H+ concentration.
The pH scale is a logarithmic scale that measures the acidity or alkalinity of a solution. A lower pH value indicates higher acidity, while a higher pH value indicates higher alkalinity. Each unit on the pH scale represents a tenfold difference in acidity or alkalinity. For example, a solution with a pH of 6 is ten times more acidic than a solution with a pH of 7, and a solution with a pH of 8 is ten times more alkaline than a solution with a pH of 7.
Given that household ammonia has a pH of 11, which is 4 units higher than a pH of 7, we can calculate the difference in H+ concentration using the relationship between pH and H+ concentration. Since ammonia is a base, it accepts H+ ions, resulting in a low H+ concentration.
To find the H+ concentration in a solution, we can use the reverse of the formula for pH:
pH = -log [H+]
Rearranging the equation:
[H+] = 10^(-pH)
For a solution with a pH of 7, [H+] = 10^(-7)
For a solution with a pH of 11, [H+] = 10^(-11)
To find the ratio of the H+ concentration in household ammonia (pH 11) to a solution with a pH of 7, divide the H+ concentration of the ammonia by the H+ concentration of the pH 7 solution:
[H+]ammonia/[H+]pH 7 = (10^(-11)) / (10^(-7))
Simplifying the expression:
[H+]ammonia/[H+]pH 7 = 10^(-11+7)
[H+]ammonia/[H+]pH 7 = 10^(-4)
Therefore, the H+ concentration in household ammonia (pH 11) is 10^(-4) times less than the H+ concentration in a solution with a pH of 7.
In numerical terms, this means that the H+ concentration in household ammonia is 10,000 times less than in the pH 7 solution.