The pH scale ranges from 0 to 14. What is the range of the hydronium ion concentration covered by this scale?
Can't you calculate that>
pH = -log(H^+)
0 = -log(H^+)
(H^+)= 10^-pH = 1.0M
Now you do 14.
To determine the range of hydronium ion concentration covered by the pH scale, we need to understand the relationship between pH and hydronium ion concentration.
The pH scale measures the acidity or alkalinity of a solution based on the concentration of hydronium ions (H3O+). A lower pH value indicates a higher concentration of hydronium ions and more acidic solution, while a higher pH value indicates a lower concentration of hydronium ions and a more alkaline solution.
The pH scale is logarithmic, meaning that each unit represents a tenfold difference in hydronium ion concentration. Mathematically, we can express this relationship using the formula:
pH = -log[H3O+]
Solving this equation for [H3O+], we get:
[H3O+] = 10^(-pH)
Now let's use this information to determine the range of hydronium ion concentration covered by the pH scale.
Starting with the lowest pH value, which is 0, we can calculate the corresponding hydronium ion concentration using the formula:
[H3O+] = 10^(-pH) = 10^(-0) = 1
Therefore, the lowest hydronium ion concentration covered by the pH scale is 1.
Moving on to the highest pH value, which is 14, we can calculate the corresponding hydronium ion concentration:
[H3O+] = 10^(-pH) = 10^(-14)
Calculating this value, we find that the highest hydronium ion concentration covered by the pH scale is:
[H3O+] = 10^(-14) ≈ 1 x 10^(-14)
Therefore, the range of hydronium ion concentration covered by the pH scale is from 1 to 1 x 10^(-14).