Buffer Solution

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 93 mL of 1.00 M NaOH solution?

  1. 👍
  2. 👎
  3. 👁
  1. I worked this problem (for you) about two days ago. Here is a link.
    http://www.jiskha.com/display.cgi?id=1302555258

    1. 👍
    2. 👎
  2. 45456565

    1. 👍
    2. 👎
  3. Calculate the pH of a buffer formed by combining 50 mL of 0.10
    M
    NaOH and 50 mL of
    0.15 M acetic acid. The pK
    a
    of acetic acid is 4.75.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

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

  2. CHEMISTRY

    HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a

  3. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka

  4. Chemistry

    An acetic acid buffer solution is required to have a pH of 5.27. You have a solution that contains 0.01 mol of acetic acid. How many moles of sodium acetate will you need to add to the solution? The pKa of acetic acid is 4.74.

  1. Buffer

    You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 93 mL of 1.00 M NaOH solution?

  2. Chemistry

    You are asked to go into the lab and prepare an acetic acid-sodium acetate buffer solution with a pH of 5.43 ± 0.02. What molar ratio of CH3COOH to CH3COONa should be used?

  3. Chemistry - Buffers

    A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer? A. .01 mol B. .05 mol C.

  4. 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

  1. school

    What is the pH of 0.1 M formic acid solution? Ka=1.7„e10-4? What is the pH value of buffer prepared by adding 60 ml of 0.1 M CH3COOH to 40 ml of a solution of 0.1 M CH3COONa? What is the pH value of an acetate buffer (pK=4.76)

  2. chemistry-science

    A 500 ml buffer solution contains .2M Acetic acid and .3M sodium acetate. Find the pH of the buffer solution after adding 20 ml of 1M NaOH, what is the pH? (pka = 4.74)

  3. Chemistry

    Acetic acid dissociates/ionizes itself as follows: CH3COOH(aq) ⇔ H+(aq) + CH3COO-(aq) If you add sodium acetate, CH3COONa, to the solution: a) a precipitate will be formed b) more acetic acid will be ionized c) the concentration

  4. Chem--buffers

    Explain why a mixture formed by mixing 100 mL of 0.100M CH3COOH and 50 mL of 0.100M NaOH will act as a buffer? in adittion to this, how do you identify if a an aqueous solution is a buffer solution, such as a solution with an acid

You can view more similar questions or ask a new question.