CHEMISTRY

posted by .

1.Chemistry Question:
A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized? The equilibrium constant (Ka) for acetic acid is 1.8x10^-5

2. Chemistry question:

On average, how far is a molecule of air in the room in which you're sitting from the nearest molecule of air to it, assuming it is an ideal gas. Appropriate assumptions about the temperature and pressure.

  • CHEMISTRY -

    I think it is easier if you assume some arbitrary number for the volume of acetic acid. Something like 100 mL.
    moles acetic acid = M x L.
    moles NaOH when 60 mL acetic acid have been neutralized = M x L.
    Then use the Henderson-Hasselbalch equation to solve for pH.

    2. I would assume a volume for the room, use PV = nRT to determine the number of moles at some P and T, convert to number of molecules and go from there. Another approach is to take a volume of 1 L, you know the density of air is about 1.29 g/L, convert to molecules/L, then take the cube root to convert to molecules along one side and convert to distance between molecules.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    A sample of 25.00 mL of vinegar is titrated with a standard 1.02 M NaOH solution. It was found that a volume of 19.60 mL of the standard NaOH solution is used to completely neutralize the acetic acid in the solution. Calculate the …
  2. chemistry

    19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution Please judge my work: Becasue NaOH and acetic acid react in a 1:1 ratio, initital moles of …
  3. chemistry

    A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized?
  4. organic chemistry

    A solution of acetic acid (CH3COOH; Ka = 1.74 x 10-5) was titrated to a final pH of 4.76 by using NaOH solution. What % of acetic acid is converted to sodium acetate (CH3COO-Na+)?
  5. Chemistry

    40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution?
  6. Chemistry

    40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution?
  7. Chemistry

    If you have 200 ml of a 0.1M solution of acetic acid (pka=4.75), 1. How many ml of a solution of 1.O M NaOH would you need to adjust the pH to 5.2?
  8. chemistry

    You were given 25.00 ml of an acetic acid solution of unknown concentration. You find that it requires 29.60 ml of a 0.1050 M NaOH solution to exaclty neutralize this sample. A) What is the molarity of the acetic acid solution?
  9. Chemistry

    In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student …
  10. chemistry II

    What is the molarity of a solution of acetic acid if 35.00mL is titrated to the end point with 68.20ml of 0.750M KOH?

More Similar Questions