Enter your answer in the provided box. in a 0.740 m solution, a weak acid is 12.5% dissociated. calculate ka of the acid.

Answer is: the acid dissociation constant for weak acid is 0.0132.
Chemical reaction: HA(aq) ⇄ A⁻(aq) + H⁺(aq).
c(weak acid) = 0,740 M.
α(weak acid)= 12,5% ÷ 100% = 0,125.
Ka = α² · c / 1 - α.
Ka = 0,125² · 0,740 M / 1 - 0,125.
Ka = 0,0132 M = 1,32·10⁻² M.
Ka is the acid dissociation constant, which quantifies the extent of acid dissociation (in this example HA) in water.

Order of filling levels and sublevels of electrons: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²3f¹⁴5d¹⁰6p⁶for an element with 5 electrons in the 3d energy level: full configuration: 1s²2s²2p⁶3s²3p³.

Reaction type : double replacement hcl + lioh = h2o + licl