Acertain weak acid, ha, has a ka value of 7.1×10−7. part a calculate the percent ionization of ha in a 0.10 m solution.

Answer is: the percent ionization of weak acid is 0.266%.
Chemical reaction: HA(aq) ⇄ H⁺(aq) + A⁻(aq).
Ka(HA) = 7.1·10⁻⁷.
c(HA) = 0.10 M.
[H⁺] = [A⁻] = x; equilibrium concentration.
[HA] = 0.10 M - x.
Ka = [H⁺] · [A⁻] / [HA].
0,00000071 = x² / 0.1 M - x.
Solve quadratic equation: x = 0.000266 M.
α = 0.000266 ÷ 0.1 M · 100% = 0.266%.

h let me think about that

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.