A solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium chloroacetate in water sufficient to y
ield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the _______ present in the buffer solution. The of chloroacetic acid is 1.36 x 10⁻³. a. H₂O
b. Na⁺
c. chloroacetate ion
d. chloroacetic acid
e. This is a buffer solution: the pH does not change upon addition of acid or base.
The chloroacetic acid, ClCH₂CO₂H, is a weak acid with Ka = 1.36x10⁻³. When this weak acid is in solution with its conjugate base, ClCH₂CO₂⁻ (From sodium chloroacetate) a buffer is produced. The addition of a strong acid as the HCl produce the following reaction
HCl + ClCH₂CO₂⁻ → ClCH₂CO₂H + Cl⁻.
Where the acid reacts with the chloroacetate ion to produce more chloroacetic acid
That means, the HCl reacts with the chloroacetate ion present in the buffer solution
Its magnifying power is: 4X 5X 9X 20X. A 4-inch, f/5 telescope has a 1-inch eyepiece focal. Its magnifying power is 9x. This answer has been confirmed as correct and helpful.
of chloroacetic acid is 1.36 x 10⁻³.