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Help With The Chemical Equilibrium Of C2h3o2

Chem helpppp! Chemical equilibrium?

Write the chemical equilibrium that describes the acid-base behavior of each of the following species in aqueous solution. Indicate whether the solution should be acidic, basic, or neutral.

a. ClO-
b. (CH3)3NH+
c. CH3CH2COOH
d. Cl-

Please help! I'm having quite a bit of trouble. ^___^;;
Thank you!

Chem equilibrium help!!?

Chemical equilibrium....

Dissociation of acetic acid, a weak acid.

HC2H3O2(aq) <==> H+ + C2H3O2^- ................. Ka = 1.8x10^-5

Altering the concentration of any one of these species will cause a shift in the equilibrium position and change the concentration of the other species. For instance, adding an acid (HCl) increases the concentration of H+ and shifts the equilibrium to the left, increasing the concentration of un-dissociated HC2H3O2 and decreasing the concentration of C2H3O2^- according to LeChatelier's principle.

Changing the concentration will shift the equilibrium, but it will not change the value of the equilibrium constant. Only changes in temperature affect the value of Keq.

HELP writing a balanced chemical equation and base‐equilibrium expression (Kb) for the dissociation of NaC2H3O2 in water?

C2H3O2^- + H2O <==> HC2H3O2 + OH^-

Kb = ([HC2H3O2] [OH^-]) / [C2H3O2^-]

Use the Ka of acetic acid to get the Kb of the acetate ion

Ka * Kb = Kw

(1.77 x 10^-5) (Kb) = 1.00 x 10^-14

Kb = 5.65 x 10^-10

Then, please go here and examine problem #1

http://chemteam.info/AcidBase/Hydrolysis...

Problem #1 is to calculate the pH of a 0.100 M solution of sodium acetate.

Chemistry: equilibrium?

Well, does the addition of OH affect any of the three compounds in your equation? The equation does not indicate any such change.

However, one of your products is H+, which will react with some of the added OH- to produce water because of the water dissociation reaction (write your own dang equation for that).

So, adding OH- causes the removal of H+, and I would hope that you have been taught (and understood) how this would affect the reaction in your question (the reaction will be driven to the right, that is, more ethanoic acid will dissociate into H+ and the ethanoate ion thingy there-i can`t believe I've forgotten how to name it). The quantity on the left side goes down and the quantity on the right goes up, except of course the acid (H+) which is being consumed by reaction with hydroxide and driving the dissociation of ethanoic acid. so the answer is (B).

Consider the equilibrium H2O(l) + HC2H3O2(aq) ---> H3O+(aq) + C2H3O2-(aq)?

For the best answers, search on this site https://shorturl.im/JpFZo

The OH- will react with the H3O+ to form water, thereby increasing the amount of reactant. This imbalance leads to an increase in the forward reaction, to restore the balance, so product formation is favoured.

Mass action equilibrium? help please due soon?

a) Sodium is soluble in water, so the compound immediately goes to C2H3O2-. The equation here would be: C2H3O2 - (aq) + H2O <--> HC2H3O2 (aq) + OH - (aq)
The equilibrium expression here is: Kb = [HC2H3O2] [OH-] / [C2H3O2 -]

b) The Acid dissociation of HC2H3O2 is pretty much the reverse of the first reaction. The reaction equation is: HC2H3O2 (aq) <--> H+ (aq) + C2H3O2 - (aq)
The equilibrium expression is: Ka = [H+] [C2H3O2 -] / [HC2H3O2]

c) For monoprotic acids, Ka x Kb = Kw = 1 x 10^-14
Ka x Kb = [HC2H3O2] [OH-] * [H+] [C2H3O2 -] /
[C2H3O2 -] *[HC2H3O2]
Ka x Kb = [OH -] [H+] = 1 x 10^-14

d) If you have the pH from your lab, all you have to do is

pH = - log [H+] (log base 10)
10^(-pH) = [H+]

---> find this concentration and use your known concentrations for sodium acetate and acetic acid to see what your equilibrium constants equal. To find [OH-], divide 1 x 10^-14 by the [H+] you find.

Hope this helps!

Writing out chemical equations for buffer solutions, Sodium Acetate, Acetic Acid. Chemistry?

1. Write the chemical equation for the acid-ionization equilibrium of acetic acid in water.
This is what I got:

HC2H3O2 (aq) + H2O (l) ------> H3O^+ (aq) + C2H3O2^- (aq)

is this right?

2, Write the chemical equation for the hydrolysis reaction of acetate ion in water. (HINT: it produces a basic solution).

3. Write the net ionic chemical equation for the reaction that you used to prepare this solution. ( solution contains both 0.10M Acetic Acid and 0.10M Sodium Acetate

any help especially on 2 and 3 would be great. thanks! :]

Equilibrium constant expression DUE SOON HELP?

I dont know how to do this right. Can you show me how to solve them please.
5.a.) Write a mass action or equilibrium constant expression for the hydrolysis of sodium acetate, NaC2H3O2.

b.) derive a relationship between the equilibrium constant for hydrolysis in 5a and the equilibrium constant for the dissociation of acetic acid, HC2H3O2.

c.) Evaluate the equilibrium constant for hydrolysis in 5b using Kw and the equilibrim constant for the dissociation of HC2H3O2 calculated in Part C (5.81 x 10^-6).

d.) Compare your calculated equilibrium constant for hydrolysis in 5c with the value that can be calculated from your pH data in part A1.

Can I have help in Chemistry please?

1. Given the reaction at equilibrium: N2(g) + 3H2(g) ↔ 2NH3(g)
If the pressure is increased at a constant temperature, there will be an increase in the number of moles of

NH3(g), only
N2(g), only
H2(g), only
both N2(g) and H2(g)

2.Given the reaction: HC2H3O2(aq) + H2O ↔ H3O+(aq) + C2H3O2-(aq)
When the reaction reaches a state of equilibrium, the concentrations of the reactants

are less than the concentrations of the products
are equal to the concentrations of the products
begin decreasing
become constant

3. An increase in the temperature of a system at equilibrium favors the

endothermic reaction and decreases its rate
endothermic reaction and increases its rate
exothermic reaction and decreases its rate
exothermic reaction and increases its rate

4.Given the reaction at equilibrium: N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the foward reaction rate due to

a decrease in the number of effective collisions
an increase in the number of effective collisions
a decrease in the activation energy
an increase in the activation energy

5.Given the reaction: 2N2(g) + O2(g) ↔ 2N2O(g)
Which statement is true when this system reaches equilibrium?

All of the N2(g) has been consumed.
All of the O2(g) has been consumed.
Pressure changes no longer occur.
The foward reaction no longer occurs.

6. Which type or types of change, if any, can reach equilibrium?

a chemical change, only
a physical change, only
both a chemical and a physical change
neither a chemical nor a physical change

What is the pH of a 0.15m NaC2H3O2 Solution?

prepare the solution and test the pH using pH meter.

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