Calculate the pH of 50.00 mL of 4.3 x 10 -7 M H 2 SO 4 .

Hey, guys. We're now going to answer the practice question that was left on the bottom of the page where we're asked to find the pH of H2SO4. 4. So, this question is different than the others. In this question, I give you ml's with the molarity. So, what exactly do we do with those liter, those milliliters? Well, you should realize here that we don't have to do anything with this volume. We would only use that volume if we were mixing this acid with a base. Here, I never made mention of another compound at all, so it's only a strong acid by itself. So again, you only would use that volume if you're mixing this compound with a base. Because we never make a mention of another compound. We don't with a strong acid by itself, so all we need to look at is the concentration. Also, we're going to say, remember, we may have 2 acidic H's and H2SO4 but that doesn't mean we multiply the concentration times 2. We're only on the lookout when it comes to strong bases. Because remember, in strong acids, the first stage that comes off is very acidic. But then the second one that's going to come off here is very weak. It doesn't really contribute to the concentration at all. It's okay to keep it as the same concentration. The question simply becomes pH equals negative log of that concentration. So equals 6.37. Hopefully, you guys were able to get this answer correct. If not, don't worry. It was kind of tricky. I didn't tell you exactly what to do with that volume.

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10. Acids and Bases

pH of Strong Acids and Bases

GOB Chemistry

10. Acids and Bases

pH of Strong Acids & Bases

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Multiple Choice

Calculate the pH of 50.00 mL of 4.3 x 10^-7M H₂SO₄.

6.37

6.07

7.67

7.37

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Verified step by step guidance

Understand that the pH of a solution is related to the concentration of hydrogen ions (H⁺) in the solution. The pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration: \( \text{pH} = -\log[\text{H}^+] \).

Given the pH of the solution is 4.34, use the pH formula to find the concentration of hydrogen ions: \( [\text{H}^+] = 10^{-\text{pH}} \). Substitute the given pH value into the equation: \( [\text{H}^+] = 10^{-4.34} \).

Calculate the hydrogen ion concentration using the expression \( 10^{-4.34} \). This will give you the molarity of H⁺ ions in the solution.

Recognize that for a strong acid like HBrO4, which dissociates completely in water, the concentration of H⁺ ions is equal to the initial concentration of the acid. Therefore, the molarity of HBrO4 is the same as the calculated \( [\text{H}^+] \).

Compare the calculated molarity of HBrO4 with the given options to identify the correct answer. The calculated value should match one of the provided choices.