water chemistry

35.0 mL sample of 0.150 M acetic acid (HC2H3O2) (Ka = 1.8 x 10-5) is titrated with 0.150 M NaOH solution. Calculate the pH after 17.5 mL volumes of base have been added

  1. 👍 0
  2. 👎 0
  3. 👁 349
  1. millimoles HAc = mL x M = 35.0 x 0.150 = approx 5.25
    mmols NaOH = 17.5 x 0.150 = 2.625

    ..........HAc + NaOH ==> NaAc + H2O
    I........5.25....0........0......0
    add.............2.625...............
    C.......-2.625..-2.625...+2.625..+2.625
    E.......2.625.....0.....2.625.....2.625

    Substitute the E line into the Henderson-Hasselbalch equation and solve for pH.

    1. 👍 0
    2. 👎 0

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

    asked by Sarah on May 23, 2007
  2. chemistry

    25.0g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?

    asked by Cynthia on May 28, 2010
  3. 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

    asked by Bob on April 10, 2011
  4. Chemistry

    Calculate the molar concentration of acetic acid (CH3COOH) in a 5.00-mL sample of vinegar (density is 1.00 g/mL) if it is titrated with 25.00 mL of NaOH.

    asked by Jake on March 4, 2009
  5. Chemistry

    Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 35.00 mL of glacial acetic acid at 25°C in enough water to

    asked by Matt on May 16, 2016
  1. Chemistry

    A certain vinegar is 6.02% acetic acid (HC2H3O2) by mass. How many grams of HC2H3O2 are contained in a 355-mL bottle of vinegar? Assume a density of 1.01g/mL.

    asked by lucylu on February 19, 2010
  2. chemistry

    What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?

    asked by nhfgchnr on June 19, 2012
  3. chemitry

    help me.. The pKa of acetic acid, HC2H3O2, is 4.76. A buffer solution was made using an unspecified amount of acetic acid and 0.30 moles of NaC2H3O2 in enough water to make 2.00 liters of solution. Its pH was measured as 4.40. How

    asked by Azy on April 24, 2015
  4. Chemistry

    A 35.0 mL sample of 0.150 M acetic acid is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: a) 0mL, b) 17.5 mL, c) 34.5 mL, d) 35 mL I've figured out a,b, and c. But at 35

    asked by Anonymous on October 28, 2010
  5. Analytical Chemistry

    Suggest a range of sample masses for the indicated primary standard if it is desired to use between 35 and 45mL of titrant: (a) 0.175 M HClO4 titrated against Na2CO3(CO2 product) (b) 0.085 M HCl titrated against Na2C2O4

    asked by Cherie on October 29, 2014
  6. chem-acid-base titrations

    Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. a.write a balanced equation for this

    asked by natash on April 21, 2008

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