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

Hey, guys, we're not gonna answer the practice question that was left on the bottom of the page where were asked to find the pH of H two s 04 So this question is different than the others. In this question, I give you MLS with the polarity. So what exactly do we do with those leaders? Those milliliters? Well, you should realize here that we don't have to do anything with this volume. We would Onley use that volume if we were mixing this acid with a base here. I never made mention of another compound it all. So it's on Lee, a strong acid by itself. So again, you on Lee would use that volume if you're mixing this compound with the base because we never make a mention of another compound were done with a strong acid by itself. So all we need to look at is the concentration. Also, we're gonna say, remember, we may have to acidic H s and H two s 04 but that doesn't mean we multiply the concentration times, too. We only were only on the lookout when it comes to strong bases. Because remember, in strong acids, the first age that comes off is very acidic. But then the second one that's gonna come off here is very weak, so it doesn't really contribute to the concentration at all. So it's OK to keep it as this same concentration. So the question simply becomes pH equals negative. Log off. That concentration so equals six point 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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17. Acid and Base Equilibrium

The pH Scale

General Chemistry

17. Acid and Base Equilibrium

The pH Scale

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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

Identify that H2SO4 is a strong acid, but at this low concentration, it behaves differently. Recognize that the concentration is close to the autoionization of water, which is 1.0 x 10^-7 M.

Consider the dissociation of H2SO4 in water. The first dissociation is complete: H2SO4 → 2H+ + SO4^2-. However, at this low concentration, the contribution of H+ from water autoionization must be considered.

Calculate the total concentration of H+ ions by adding the concentration from H2SO4 and the concentration from water autoionization. Use the expression: [H+] = [H2SO4] + [H2O].

Since the concentration of H2SO4 is 4.3 x 10^-7 M, and the autoionization of water contributes 1.0 x 10^-7 M, add these concentrations to find the total [H+].

Calculate the pH using the formula: pH = -log([H+]). Substitute the total [H+] concentration into this formula to find the pH.