Calculate [H3O] for a solution of hydrochloric acid that is:
pH=2.00
pH=3.00
pH = -log(H^+)
Haha, oh, I hope you're ready for this! It's time for a little chemistry circus act. 🎪
For the first question, when pH is 2.00, we need to calculate the concentration of hydronium ions ([H3O+]) in a solution of hydrochloric acid. Well, according to our chemistry ringmasters, pH is defined as the negative logarithm of the hydronium ion concentration. So, if the pH is 2.00, the concentration of hydronium ions would be 10^(-2.00) moles per liter. Ta-da!
Now, on to the second question. When pH is 3.00, we once again need to calculate the concentration of hydronium ions ([H3O+]) in the hydrochloric acid solution. Since pH is defined as the negative logarithm of the hydronium ion concentration, if the pH is 3.00, the concentration of hydronium ions would be 10^(-3.00) moles per liter. Bravo!
Remember, stay amused and let the chemistry circus continue! 🤡
To calculate the concentration of hydronium ions ([H3O+]) for a given pH value, we can use the formula:
pH = -log[H3O+]
Let's calculate [H3O+] for each given pH:
1. pH = 2.00:
Using the formula, we can rearrange it to solve for [H3O+]:
-log[H3O+] = 2.00
Taking the antilog (inverse log) of both sides to eliminate the logarithm:
[H3O+] = 10^(-2.00)
Evaluating the expression:
[H3O+] = 0.01 M or 1.00 x 10^(-2) M
Therefore, the concentration of hydronium ions for a solution with a pH of 2.00 is 0.01 M.
2. pH = 3.00:
Similar to the previous calculation, rearrange the equation:
-log[H3O+] = 3.00
Taking the antilog of both sides:
[H3O+] = 10^(-3.00)
Evaluating the expression:
[H3O+] = 0.001 M or 1.00 x 10^(-3) M
Hence, the concentration of hydronium ions for a solution with a pH of 3.00 is 0.001 M.
To calculate the concentration of [H3O+] (also known as hydronium ion concentration), we need to use the equation:
pH = -log [H3O+]
From the given pH value, we can determine the [H3O+] concentration.
For a solution with pH = 2.00:
Using the equation, rearrange it to solve for [H3O+]:
[H3O+] = 10^(-pH)
[H3O+] = 10^(-2.00)
[H3O+] = 0.01 M or 1.0 x 10^(-2) M
Therefore, the concentration of [H3O+] for a solution with pH = 2.00 is 0.01 M or 1.0 x 10^(-2) M.
For a solution with pH = 3.00:
Again, using the equation, rearrange it to solve for [H3O+]:
[H3O+] = 10^(-pH)
[H3O+] = 10^(-3.00)
[H3O+] = 0.001 M or 1.0 x 10^(-3) M
Therefore, the concentration of [H3O+] for a solution with pH = 3.00 is 0.001 M or 1.0 x 10^(-3) M.