# chemistry

posted by .

n one experiment, a mixture of 1.000 mol acetic acid and 0.5000 mol ethanol is brought to equilibrium. A sample containing exactly one-hundredth of the equilibrium mixture requires 28.80mL 0.1040M Ba(OH)2 for its titration.

Calculate the equilibrium constant, , for the ethanol-acetic acid reaction based on this experiment.

• chemistry -

Ethanol + acetic acid ==> ethyl acetate + H2O

Ba(OH)2 + 2CH3COOH ==> Ba(CH3COO)2 + 2H2O
moles Ba(OH)2 = 0.02880*0.1040 = 0.002995.
moles CH3COOH remaining after the rxn (in the aliquot taken for analysis) = 2*0.002995 = 0.00599 moles.
Since that was exactly 1/100 of the equilibrium mixture, mol CH3COOH after the rxn = 0.599. I don't have enough room to write the equation unless we shorten how we write the chemicals. Therefore CH3COOH becomes HAc and ethanol becomes EtOH.
............HAc + EtOH ==> EtAc + H2O
initial..... 1.0...0.50.....0......0
change.......-x......-x......+x....+x
final........0.599....0.099..401...401
So if we start with 1.0 mol HAc and we have 0.599 at equilibrium, that means x, the amount reacted must be 0.401 and you can complete the ICE table as I've done above.
Then substitute equilibrium values into the Kc expression for the reaction and calculate the Keq.

## Similar Questions

1. ### chemistry

In an esterification experiment, 2.0 mol of ethanol were mixed with 1.0 mol of ethanoic acid in a container of volume 30cm3 and the chemicals were allowed to come to equilibrium at 25°, CH3CO2H + C2HOH <-> CH3COOC2H5 + H20 If …
2. ### chemistry

A classic experiment in equilibrium studies dating from 1862 involved the reaction in solution of ethanol and acetic acid to produce ethyl acetate and water. The reaction can be followed by analyzing the equilibrium mixture for its …
3. ### Chemistry

A mixture containing 0.5 mol of H2 (g) and 0.5 mol of I2 (g) was introduced into a 10L container at a temperature of 448 C. At this temperature the equilibrium constant Kp is 50. i. What is the total pressure in the container before …
4. ### Chemistry

A mixture containing 0.5 mol of H2 (g) and 0.5 mol of I2 (g) was introduced into a 10L container at a temperature of 448 C. At this temperature the equilibrium constant Kp is 50. i. What is the total pressure in the container before …
5. ### chemistry

please help and explain. At a certain temperature, Keq = 10.5 for the equilibrium below. CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g) Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing 1.01 …
6. ### CHEMISTRY: URGENT DRBob222

A mixture of 0.50 mol of ethanoic acid and 1.00 mol of ethanol was shaken for a long time to reach equilibrium. The whole mixture was titrated quickly with 1.00 mol dm3 sodium hydroxide and 80cm3 of alkali were required. 1. Write an …
7. ### Chemistry

An equilibrium mixture in a 10.0 L flask contains 7.0 mol HI(g) and 1.0 mol each of I2(g) and H2(g). If 2.5 mol H2, 5.0 mol I2 and 2.0 mol HI are added to that equilibrium mixture how many moles of each gas will be present when equilibrium …
8. ### CHEM- need help ASAP

An equilibrium mixture in a 10.0 L flask contains 7.0 mol HI(g) and 1.0 mol each of I2(g) and H2(g). If 2.5 mol H2, 5.0 mol I2 and 2.0 mol HI are added to that equilibrium mixture how many moles of each gas will be present when equilibrium …
9. ### Chemistry

Consider the reaction HCHO(g) *) H2(g) + CO(g). 1.0 mol of HCHO, 1.0 mol of H2 and 1.0 mol of CO exist in equilibrium in a 2.0 L reaction vessel at 600C. a) Determine the value of the equilibrium constant Kc for this system. 2.0 moles …
10. ### Chemistry

When 0.20 mol of hydrogen gas and 0.15 mol of iodine gas are heated at 723 K until equilibrium is established, the equilibrium mixture is found to contain 0.26 mol of hydrogen iodide. The equation for the reaction is as follows. H2(g) …

More Similar Questions