If $\alpha$(HSO₃^-) = 0.45 at pH 7.0,What are $\alpha$(H₂SO₃)And $\alpha$(SO₃²^-)At this pH? For H₂SO₃,PK_a1 and pK_a2 are 1.81 and 6.91,Respectively. A) $\alpha$(H₂SO₃) = 0.225 and $\alpha$(SO₃²^-) = 0.55 B) $\alpha$(H₂SO₃) = 0.55 and $\alpha$(SO₃²^-) ~ 0 C) $\alpha$(H₂SO₃) ~ 0 and $\alpha$(SO₃²^-) = 0.225 D) $\alpha$(H₂SO₃) ~ 0 and $\alpha$(SO₃²^-) = 0.55 E) $\alpha$(H₂SO₃) = 0.45 and $\alpha$(SO₃²^-) = 0.55

Question

Quizplus · Accepted Answer

Given the pKa values of 1.81 and 6.91 for the first compound, at pH 7.0, the fraction of the species in the protonated form would be very low for the first pKa and close to 50% for the second pKa. Thus, the alpha value for H₂SO₃ would be close to 0 because the pH is above both pKa values, indicating most of the species would be deprotonated. For the second compound, the given alpha value of 0.45 for a similar species suggests that the fraction of the species in a specific form (likely the protonated form given the context) is significant, and without specific pKa values provided for this compound, we can infer that its behavior at pH 7.0 would be similar or slightly higher due to the absence of specific pKa values that would significantly alter its state. Therefore, an alpha value of 0.55 is reasonable, indicating a significant fraction of the species is in the specified form.

If α\alphaα (HSO3-) = 0 α\alphaα (H2SO3)And α\alphaα (SO32-)At This PH? for H2SO3,PKa1 and PKa2 Are 1

If $\alpha$ (HSO₃^-) = 0 $\alpha$ (H₂SO₃)And $\alpha$ (SO₃²^-)At This PH? for H₂SO₃,PK_a1 and PK_a2 Are 1