Chemistry

A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....?
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP,
with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and a final
buret reading of 31.32 mL.
“KHP” is shorthand for a certain acid. It contains NO phosphorus.

•Write the reaction equation for the acid-base neutralization.
I got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct?

•Name the secondary standard used in the titration of the unknown KHP mixture.

• Calculate the amount of NaOH (in millimoles) delivered in the titration.

• Find the mass of KHP neutralized in the reaction.

• Calculate the mass percent of KHP in the original sample.

  1. 👍
  2. 👎
  3. 👁
  1. got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct?
    yes

    •Name the secondary standard used in the titration of the unknown KHP mixture.
    NaOH

    • Calculate the amount of NaOH (in millimoles) delivered in the titration.

    mL x M = millimols


    • Find the mass of KHP neutralized in the reaction.

    millimoles KHP = millimoles NaOH
    g KHP = (millimoles/1000)*molar mass


    • Calculate the mass percent of KHP in the original sample.

    %KHP in sample = (grams KHP/mass sample)*100 = ?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Ethanoic acid can be reacted with alcohols to form esters, an equilibrium mixture being formed. CH3CO2H + ROH CH3CO2R + H2O The reaction is usually carried out in the presence of an acid catalyst. In an experiment to determine Kc

  2. Chemistry

    The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated KHP). KHP is an acid with one acidic hydrogen and a molar mass of

  3. chemistry(Urgent Please help)

    A student is asked to standardize a solution of barium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 33.9 mL of barium hydroxide to reach the endpoint. A.

  4. Inorganic chemistry

    Potassium hydrogen phthalate (molar mass = 204.2 g/mol is used to standardize sodium hydroxide. If 23.67 ml of NaOH (aq) is required to titrate 0.7719 g KHP to the equivalence point, what is the concentration of the NaOH(aq)?

  1. chemistry

    What is the equivalent weight of: (a) Potassium tetraoxalate, KHC2O4•H2C2O4•2H2O, if the complete neutralization is assumed. (b) Sodium carbonate if it is titrated to the phenolphthalein end point with HCl. The reaction is

  2. chemistry

    what is the balanced equation for the reaction of potassium dichromate and potassium hydrogen phthalate?

  3. chemistry

    calculate the mass of potassium hydrogen phthalate needed to prepare a 0.1M solution in a 250 ml volumetric flask given that the molar mass of potassium hydrogen phthalate is 204,23g/mol

  4. CHEMISTRY: URGENT DRBob222

    Why was the reaction mixture titrated quickly? (question fom: 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

  1. Chemistry

    A standard KHP solution is made by dissolving 2.12 grams of KHP in 100.00 mL of water. The KHP solution is then titrated with NaOH solution. It takes 23.12 mL of NaOH to reach the endpoint. What is the concentration of the NaOH?

  2. Chemistry

    Hello, I need help with calculations for lab. I prepared excess NaOH and HCL solutions (unknown conc., ~0.1M). Then I standardized my NaOH solution by titrating known amounts of KHP (Potassium hydrogen phthalate)with it in the

  3. Chemistry

    The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl

  4. Chemistry

    A sample of 1.018 g of KHP (potassium hydrogen phthalate, molar mass = 204.22 g/mol) was dissolved in ~ 25 mL distilled water and titrated with a NaOH solution of unknown concentration. If 28.69 mL of base was used to reach the

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