# chemistry-

posted by .

How do I construct an ICE table for this question.
CH3COOH + NaOH --> CH3COONa + H2O

Fill in the equilibrium line of the table. [Think about the initial pH and think about the pH at the end point of the titration.
Initial pH 2.72
When the solution turned pink pH was 8.49

I forgot to add that the
concentration of acetic acid is 0.2M and volume is 25ml

the concentration of NaOH is 0.2M and the volume is 50mL

Is that all of the data in the problem? If so, the pH = -log(H^+). Use that and ionization of CH3COOH to calculate the concn of CH3COOH at the beginning.
CH3COOH ==> CH3COO^- + H^+

pH at the equivalence point is 8.49. Similarly, determine (H^+) and from that determine (OH^-).
Knowing that the pH at the equivalence point is due to the hydrolysis of the acetate ion,
CH3COO^- + HOH ==> CH3COOH + OH^-

Kb = Kw/Ka = (OH^-)^2/(CH3COO^-). Solve for CH3COO^- (the salt).

Knowing beginning (CH3COOH) and the CH3COO^- at the equivalence point will allow you to determine (NaOH).

I think you need the above data before you can construct and ICE table. But perhaps there is more to the problem than that. Post your work if you get stuck.

I guess all my typing was futile.
Determine #mols CH3COOH
Detemine #mols NaOH.
Then
CH3COOH + NaOH ==>CH3COONa + HOH
initial --you can fill in.
change-- the smaller number of mols will be the mols CH3COONa and mols HOH formed. That same number will be subtracted from the beginning for the reactants.
equilibrium--add the intial to change to find equilibrium.
Post your work if you get stuck.

# of mols for acetic acid = 5mols
# of mols for salt =10mols

CH3COOH + NaOH ==>CH3COONa + HOH
I 0.2M 0.2M 0 0
C -x -x ? ?
E 0.2-x 0.2-x ? ?

do I placed 5mols (since it is the smaller numebr of mols) where CH3COONa and HOH are?

CH3COOH + NaOH ==>CH3COONa + HOH
OK. First, you didn't change volume to liters. You can make a chart on paper but I can't type it onto the screen. It is difficult to leave spaces.

Initially:

CH3COOH = 0.025 x 0.2 M = 0.005 mol.
NaOH = 0.05 L x 0.2 M = 0.01 mol,
CH3COONa = 0
HOH = 0

change:

CH3COOH is the limiting reagent because that is the smaller one. Therefore,
mols CH3COONa formed = 0.005
mols HOH formed = 0.005
mols taken from CH3COOH = 0.005
mols taken from NaOH = 0.005

CH3COONa = 0 + 0.005 mol = 0.005
HOH = 0 + 0.005 = 0.005
CH3COOH = 0.005 - 0.005 = 0 mol
NaOH = 0.01 - 0.005 = 0.005 mol

Therefore, the solution consists of 0.005 mol CH3COONa (sodium acetate) + 0.005 mol NaOH (the amount in excess) after the reaction is complete.
If you want concentrations, divide each of the mol values by 0.075 liters (25 mL + 50 mL = 75 mL). I'm not sure this is exactly what you wanted. If not, clarify and explain what you need.

yes thank you very much, I understand it

## Similar Questions

1. ### Chemistry

Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic …
2. ### Chemistry

You are carrying out the titration of 100.0 mL of 1.000M acetic acid with 1.000 M sodium hydroxide. Ka = 1.76x10^-5 of acetic acid. (a) Calculate the initial pH of your acetic acid sample. (b) Calculate the pH of the solution after …
3. ### Chemistry

The following table contains data for the equilibrium reaction CH3COOH(g)+ C2H5OH(g)↔ CH3COOC2H5(g)+ H2O(g) T = 100oC. Each row in the table represents a different experiment (diffferent intial concentrations). Initial concentration …
4. ### Chemistry

Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution?
5. ### Chemistry 102

For a question like â€ścalculate the pH of an aq.solution that is 1.0 M CH3COOH and 1.0 M CH3COONa, how do you know to write the equation like this: CH3COOH + H2O => H3O+ + CH3COO- and not like H3O+ + CH3COO- => CH3COOH + H2O …
6. ### CHEMISTRY

The major component of vinegar is acetic acid CH3COOH. Which of the following reactions represents the balanced equation between acetic acid and sodium bicarbonate?
7. ### chemistry

Which of the following has the greatest buffer capacity?
8. ### chemistry

Using the concentration of CH3COOH (0.8326M) and the equilibrium concentration of H3O+ (OJ = 31.6x10^-6 and milk = 3.16x10^-8), complete the reaction table for vinegar. Then calculate the acidity constant. Please show all work in solving …
9. ### Chemistry

Problem: Calculate the pH titration of 50 mL of 0.02M H3PO4 from pH 1 to 13 with 0.4M NaOH. So I believe the balanced reaction is: H3PO4 + OH --> H2PO4 + H2O (Since Na I believe is insignificant, maybe that's wrong. If so then, …
10. ### Chemistry

Using the concentration of CH3COOH (0.8326M) and the equilibrium concentration of H3O+ (3.2x10-3), complete the reaction table for vinegar. Then calculate the acidity constant. Reaction table is given Ch3COOH + H2O --CH3COO- + H3O+ …

More Similar Questions