Chemistry

posted by .

Calculate the pH of a 100mL solution of 0.10M acetic acid ka=1.8x10(-5)

i calculated the pH to be 2.87

from the square root of
(1.8x10(-5) * 0.1, the negative log gives me the pH.

The next question wants you to calculate the pH with 50mL HCl added. I found the pH to be 2.78 by just adding .05 to the bottom [HA] value are these correct so far?

  • Chemistry -

    2.87 is correct for the first one.
    For #2, you don't provide the (HCl). Although (HCl) is not listed; I suspect your answer of 2.78 is not right. Assume (HCl) is 0.1M and you add 50 mL so that is 5 millimoles/150 mL = 0.0333M HCl.
    Since HCl is 100% ionized (and acetic acid is only about 1% ionized) most of the H^+ will be contributed by HCl and pH = 1.48.
    If (HCl) is 0.01M, we add 0.5 millimole HCl and that in 150 mL = 0.00333 which is 2.48 for pH.

  • Chemistry -

    2

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry!!

    At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
  2. Chemistry

    At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
  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. Chemistry

    so i had to calculate the pH of a 100ml solution of .10M acetic acid (ka=1.8x10(-5) I came out to 2.87. But then, they want the pH if 50ml HCL is added. So i thought...Ka = x2/.15M, therefore the square root of .15M x 1.8x10(-5) = …
  5. Chemistry

    Ok, moving on from my last question, you have 100mL of 0.10M acetic acid with ka = 1.8x10(-5) and add 50mL (0.10M) NaOH.
  6. Chemistry

    if you have 100mL of 0.1M acetic acid (ka = 1.8x10(-5)what is the pH after 10mL NaOH is added?
  7. chemistry

    (Re-posting because no one was answering chemistry questions) if you have 100mL of 0.1M acetic acid (ka = 1.8x10(-5)what is the pH after 10mL NaOH is added?
  8. AP Chem

    Calculate the correct volumes of the 0.1M acetic acid solution and the 0.1M sodium acetate solution needed to make 50mL of a buffer solution with a pH vaule of 5.00. (Ka = 1.8x10^-5)
  9. Chemistry

    What is the hydrogen-ion concentration of a solution that is 0.016M in acetic acid and 0.016M in sodium acetate at 25 Celsius?
  10. Chemistry

    First, the question I'm given is: What is the pH of a 1.0 L solution containing 0.25M acetic acid and 0.75M sodium acetate ( Ka for acetic acid= 1.8x 10-5) So I took the -log(1.8x10-5)= 4.74+log(.75/.25)= 5.22 pH But then I'm asked …

More Similar Questions