Answer:
pOH = -log[OH-]
log x =a <=> 10ª = x
so, if pOH is 10.75, we need to aply the anti log of it to get the [OH-], where x is [OH-] and a is pOH
using the calc, we have
-log [OH-] = 10.75 <=>10^(-10.75) = [OH-]
[OH-]= 1.78 x 10^(-11)
We are told that there are solid and liquid phases of acetic acid, but the presence of an odor implies that there is a gaseous phase as well. It is likely that some of the acetic acid has vaporized due to its volatility. Therefore, there are 3 phases present in the bottle. The solid and liquid phases can be observed visually (the gas cannot since it is not colored), and the gas is detected because of its odor.
Explanation:
Sodium hydroxide completely ionizes in water to produce sodium ions and hydroxide ions. Hydroxide ions are in excess and neutralize all acetic acid added by the following ionic equation:
The mixture would contain
if undergoes no hydrolysis; the solution is of volume after the mixing. The two species would thus be of concentration and , respectively.
Construct a RICE table for the hydrolysis of under a basic aqueous environment (with a negligible hydronium concentration.)
The question supplied the <em>acid</em> dissociation constant for acetic acid ; however, calculating the hydrolysis equilibrium taking place in this basic mixture requires the <em>base</em> dissociation constant for its conjugate base, . The following relationship relates the two quantities:
... where the water self-ionization constant under standard conditions. Thus . By the definition of :
First, we write the reaction equation for the formation of HCl from hydrogen and chlorine:
H₂ + Cl₂ → 2HCl
Now, we substitute the values of the enthalpies, denoting that of the Cl-Cl bond by x:
435 + x = -92 + 2(431)
x = 335
The bond dissociation enthalpy for the Cl-Cl bond is 335 kJ/mol