If the pH of a nitric acid solution is 2.34, then what is the molarity of nitric acid in the solution?
A. 1.6 × 10-4 M
B. 3.8 × 10-3 M
C. 2.2 × 10-2 M
D. 4.6 × 10-3 M
Oh Robert......
Bruh js answer the question someone
Bob was right, just annoying that you refuse to actually answer it. Holy we're only here cus we don't wanna answer it all the time.
ANYWAYS:
pH = -Log(H^+)
2.34 = -Log(H^+)
-2.34 = Log(H^+) [Divided both sides by -1]
H^+ = 10^-2.34
H^+ = 4.6 x 10^-3
FINAL ANSWER IS: Option D
Well, let me tell you a "pHunny" story!
Once upon a time, there was a nitric acid solution with a pH of 2.34. Now, to find the molarity of nitric acid in the solution, we need to do a little calculation.
The pH of a solution is equal to the negative logarithm (base 10) of the concentration of hydronium ions (H3O+).
Using this formula, we can convert the pH of 2.34 to a concentration. So, the concentration of H3O+ ions is 10^(-2.34) M.
Since nitric acid is a strong acid and fully ionizes in water, the concentration of nitric acid is the same as the concentration of H3O+ ions.
Therefore, the molarity of nitric acid in the solution is 10^(-2.34) M.
And if we crunch the numbers, we find that the answer is B. 3.8 × 10^(-3) M!
So, now you know the "pHunny" way to calculate the molarity of nitric acid. Keep those acid-base jokes rollin'!
To find the molarity of nitric acid in the solution, we need to understand the relationship between pH and molarity.
pH is a measure of the concentration of hydrogen ions (H+) in a solution. It is defined on a logarithmic scale, ranging from 0 to 14. In this scale, a pH of 7 is considered neutral, values below 7 are acidic, and values above 7 are basic.
The formula to calculate pH is:
pH = -log[H+]
Where [H+] is the concentration of hydrogen ions in moles per liter (M).
Now, let's solve the problem using the given information. The pH of the nitric acid solution is 2.34.
Since pH = -log[H+], we can rearrange the equation to find [H+]:
[H+] = 10^(-pH)
[H+] = 10^(-2.34)
[H+] ≈ 4.46 × 10^(-3) M
Therefore, the molarity of nitric acid in the solution is approximately 4.46 × 10^(-3) M.
Looking at the given answer choices, the closest option is:
D. 4.6 × 10^(-3) M
So the correct answer is D. 4.6 × 10^(-3) M.
pH = -log(H^+).
Substitute and solve for (H^+). That will be the molarity in mols/L.