If an acid,HA,is 14.7% dissociated in a 1.0 M solution,what is the K_a for this acid? A)1.7 $\times$ 10^-¹ B)2.5 $\times$ 10^-² C)1.5 $\times$ 10^-¹ D)3.9 $\times$ 10¹ E)none of these

Question

Quizplus · Accepted Answer

The degree of dissociation is 0.147 for a 1.0 M solution. Therefore, [H⁺] = [A⁻] = 0.147 M and [HA] = 1.0 - 0.147 = 0.853 M. The expression for Kₐ is [H⁺][A⁻]/[HA] = (0.147)(0.147)/0.853 = 0.0254, which is approximately 2.5 x 10⁻².

If an Acid,HA,is 14 ×\times× 10-1 B)2 ×\times× 10-2 C)1 ×\times× 10-1 D)3 ×\times×

If an Acid,HA,is 14 $\times$ 10^-¹
B)2 $\times$ 10^-²
C)1 $\times$ 10^-¹
D)3 $\times$