Diet Coke has a pH of about 3.0. Milk has a pH of about 7.0. How much greater is the H+ ion concentration of Diet Coke when compared to milk?
- Would it be 1x10^4 greater concentration
Yes, 7-3=4 and each unit on the pH scale, since it is a log scale, is equal to 10; therefore, the coke is 10^4 times more acidic and that is 10,000 times.
To determine the difference in H+ ion concentration between Diet Coke and milk, we can calculate the ratio of their hydrogen ion concentrations.
pH is a logarithmic scale that measures the concentration of hydrogen ions (H+) in a solution. The formula for pH is pH = -log[H+], where [H+] represents the concentration of hydrogen ions.
First, let's convert the pH values of Diet Coke and milk to their respective hydrogen ion concentrations:
Diet Coke:
pH = 3.0
[H+] = 10^(-pH) = 10^(-3.0) = 0.001 M (mol/L)
Milk:
pH = 7.0
[H+] = 10^(-pH) = 10^(-7.0) = 0.0000001 M (mol/L)
Now, we can calculate the ratio of their hydrogen ion concentrations:
[H+] Diet Coke / [H+] Milk = 0.001 M / 0.0000001 M = 10,000
Therefore, the H+ ion concentration of Diet Coke is 10,000 times greater than that of milk. In scientific notation, this would be written as 1 × 10^4 greater concentration.
To determine the difference in H+ ion concentration between Diet Coke and milk, you need to compare their pH values. The pH scale is logarithmic, meaning that each unit represents a tenfold difference in acidity or alkalinity.
Given that Diet Coke has a pH of 3.0 and milk has a pH of 7.0, we can calculate the difference as follows:
pH of Diet Coke - pH of milk = 3.0 - 7.0 = -4.0
Since the pH value is negative, we know that Diet Coke is more acidic (higher H+ concentration) than milk. To convert the difference into a relative concentration, you need to raise 10 to the power of the pH difference:
H+ ion concentration of Diet Coke / H+ ion concentration of milk = 10^(-4.0)
Evaluating 10^(-4.0) gives you 0.0001.
Therefore, the H+ ion concentration of Diet Coke is 0.0001 times (or 1 x 10^(-4)) greater than that of milk.