Final answer:
To find the Ka for the conjugate acid of HONH₂ (Kb = 1.1 x 10⁻³), use the equation Ka x Kb = Kw, where Kw is the ionization constant of water (1.0 x 10⁻¹⁴). Solving for Ka gives us a value of 9.09 x 10⁻¹².
Step-by-step explanation:
To find the Ka for the conjugate acid of HONH₂, whose Kb is given as 1.1 x 10⁻³, we employ the relationship between the Ka and Kb of conjugate acid-base pairs: Ka x Kb = Kw. Here, Kw is the ionization constant of water, which is 1.0 x 10⁻¹⁴ at 25 °C. Using the relationship provided: Ka = Kw / Kb. Substituting the given values: Ka = (1.0 x 10⁻¹⁴) / (1.1 x 10⁻³)
Now, let's perform the calculation to find the Ka. Ka = 9.09 x 10⁻¹². This is the Ka for the conjugate acid of HONH₂, confirming that the relationship between Ka and Kb is fundamental to determining acid and base strengths in aqueous solutions.