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How to calculate the standard state Gibbs Free Energy values at pH 0 and for dissociation of acetic acid with a Ka 1.75 X 10-5?
Wiki User
∙ 13y ago
Delta G (rxn) = - RT ln K.
Wiki User
∙ 13y ago
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What happens when you mix H2O and acetic acid?
Acetic acid simply becomes ionized in water (about 5% dissociation).
How do you calculate the Degree of Ionization of Acetic Acid?
measure pH of a known solution, say 0.1 mol/L acetic acid. pH = - log10[H3O+], rearrange that and: [H3O+] = 1 / (10^pH) so now you have concentration of hyronium ions. If acetic acid completely dissociated into its ions, then 0.1mol/L would be ions, but it doesn't! So the percentage of dissociation = 0.1 / [H3O+] = 0.1 / [ 1 / (10^pH)]
Which effect can explain increase in dissociation of acetic acid on addition of naoh?
Because hydroxide (OH-) is a strong base reacting completely with undissociated acetic acod (CH3COOH) to leave only acetate ions (CH3COO-) and water when completed.
What is the difference between aqueous solutions of acetic acid and nitric acid?
Nitric acid and acetic acid are different substances; the chemical properties and physical properties are also different (density of the solutions, corrosiveness, chemical reactions, dissociation, etc.).
Why is acetic weaker than hydrochloric acid?
The strength of the acid depends on the amount of hydrogen ions which come from the dissociation of the acid. Hydrochloric acid (HCl) splits entirely into ions: H+ and Cl-, due to a large acid dissociation constant (Ka). Ka of an acetic acid is relatively small (10-4.8). That means that lots of molecules stays undissociated and do not produce H+ ions.
What happens when you mix H2O and acetic acid?
Acetic acid simply becomes ionized in water (about 5% dissociation).
How do you calculate the Degree of Ionization of Acetic Acid?
measure pH of a known solution, say 0.1 mol/L acetic acid. pH = - log10[H3O+], rearrange that and: [H3O+] = 1 / (10^pH) so now you have concentration of hyronium ions. If acetic acid completely dissociated into its ions, then 0.1mol/L would be ions, but it doesn't! So the percentage of dissociation = 0.1 / [H3O+] = 0.1 / [ 1 / (10^pH)]
Which effect can explain increase in dissociation of acetic acid on addition of naoh?
Because hydroxide (OH-) is a strong base reacting completely with undissociated acetic acod (CH3COOH) to leave only acetate ions (CH3COO-) and water when completed.
What is the difference between aqueous solutions of acetic acid and nitric acid?
Nitric acid and acetic acid are different substances; the chemical properties and physical properties are also different (density of the solutions, corrosiveness, chemical reactions, dissociation, etc.).
Why is acetic weaker than hydrochloric acid?
The strength of the acid depends on the amount of hydrogen ions which come from the dissociation of the acid. Hydrochloric acid (HCl) splits entirely into ions: H+ and Cl-, due to a large acid dissociation constant (Ka). Ka of an acetic acid is relatively small (10-4.8). That means that lots of molecules stays undissociated and do not produce H+ ions.
Calculate pH of 1.0 m acetic acid?
2.4
Why formic acid is more acidic than acetic acid?
Because it has a greater/higher Ka (dissociation constant). This is related to the ease with which the H+ can be released from the COOH group.
What is the morphology of acetic acid bacteria?
Acetic acid bacteria gains energy from the oxidation of acetic acid and ethanol during the fermentation period. The are found in areas where ethanol is produced by the fermentation of sugars.
If 0.1MHAC is titrated with 0.1MNaoh and the dissociation constant ka of acetic acid is 1.8210-5 and the solubility product of water is 110-14 what is the initial pH of the acid?
I don't even understand what you are saying.
What is the type of bacteria that uses heat and acid for energy?
acetic acid
What is the most acetic energy drink?
Yes, it has. A womans heart blew up from ONE energy drink.
What happen when vinegar and water mix?
You get diluted vinegar. Most vinegar sold today is already diluted with water, so any dissociation of the acetic acid molecules has already occurred before you get it.
