The ka of acetic acid (hc2h3o2) is 1.8 ⋅ 10-5. what is the ph at 25.0 °c of an aqueous solution that is 0.100 m in acetic acid? the ka of acetic acid (hc2h3o2) is 1.8 10-5. what is the ph at 25.0 °c of an aqueous solution that is 0.100 m in acetic acid? +2.87 -2.87 -11.13 +6.61 +11.13

2.872.

Explanation:

∴ [H⁺] = √(Ka.C) = √(1.8 x 10⁻⁵)(0.1 M) = 1.342 x 10⁻³.

∵ pH = - log[H⁺].

∴ pH = - log(1.342 x 10⁻³) = 2.872.

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.