What is the concentration of H3O+ in a solution with the following pH values. Enter your answer in scientific notation.
a. 6.66
b. 13.40
c. 13.17
d. 2.39
pH=-logHconcentration
Hconcentration=10^-pH
a. 10^-6.66= 2.19E-7
c. 10^-13.17=1.70E-14
To find the concentration of H3O+ in a solution with a given pH value, we can use the equation:
pH = -log[H3O+]
To solve for [H3O+], we need to take the antilog (inverse logarithm) of the negative pH value. The antilog function is commonly denoted as 10^x.
Let's calculate the concentration of H3O+ for each pH value given:
a. pH = 6.66
[H3O+] = 10^(-pH) = 10^(-6.66)
b. pH = 13.40
[H3O+] = 10^(-pH) = 10^(-13.40)
c. pH = 13.17
[H3O+] = 10^(-pH) = 10^(-13.17)
d. pH = 2.39
[H3O+] = 10^(-pH) = 10^(-2.39)
Now, let's express the answers in scientific notation:
a. [H3O+] = 10^(-6.66) = 2.31 x 10^(-7) M
b. [H3O+] = 10^(-13.40) = 3.98 x 10^(-14) M
c. [H3O+] = 10^(-13.17) = 7.62 x 10^(-14) M
d. [H3O+] = 10^(-2.39) = 4.13 x 10^(-3) M
Therefore, the concentrations of H3O+ in the given solutions are:
a. 2.31 x 10^(-7) M
b. 3.98 x 10^(-14) M
c. 7.62 x 10^(-14) M
d. 4.13 x 10^(-3) M