Chemistry (organic)

You have a solution that contains 5.0 g of oxalic acid dissolved in 150 mL of water. This solution is placed in a separatory funnel, and then 100 mL of diethyl either is added to the separatory funnel and an extraction is performed (diethyl ether and water are immiscible). Use the following constants to calculate how much oxalic acid is in each solvent after the extraction: solubility of acid in water= 9.5g/100mL and solubility of acid in ether= 16.9 g/100mL

  1. 👍 0
  2. 👎 0
  3. 👁 519
  1. Do you have a K. I usually use them as g/g and if your prof does the same, then Ko/a = K(16.9/9.5) = 1.78
    Then K = (concn organic phase/concn aqueous phase). Let x = g in organic phase, then 5-x = g in aqueous phase.
    For org phase you have x/100
    For aqueous phase you have (5-x)/150
    Solve for x and 5-x

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL

    asked by Emma on November 7, 2018
  2. Chemistry

    1. Calculate the concentration of H3O+, HC2O4-1, and oxalate ion (C2O42-) in a 0.175 M solution of oxalic acid (C2H2O4). [For oxalic acid, Ka1 = 6.5 ´ 10-2, Ka2 = 6.1 ´ 10-5.]

    asked by Anonymous on December 11, 2014
  3. Chemistry

    Oxalic acid, found in the leaves of rhubarb and other plants, is a diprotic acid. H2C2O4 + H2O ↔ H3O+ + HC2O4- Ka1= ? HC2O4- + H2O ↔ H3O+ + C2O42- Ka2 = ? An aqueous solution that is 1.05 M H2C2O4 has pH = 0.67. The free

    asked by Ashley on November 15, 2016
  4. science

    0.63 gm of oxalic acid (COOH)2 2H20 are dissolved in 500 ml of solution. Calculate the molarity of the solution?

    asked by aarti on June 16, 2013
  5. chemistry

    Calculate the concentration of oxalate ion (C2O42−) in a 0.175 M solution of oxalic acid (C2H2O4). [For oxalic acid, Ka1 = 6.5 × 10−2, Ka2 = 6.1 × 10-5.]

    asked by sarah on February 22, 2011
  1. Chemistry

    A sample of oxalic acid (H2C2O4, with two acidic protons), of volume 37.09 mL was titrated to the stoichiometric point with 22.41 mL of 0.163 M NaOH(aq). What is the molarity of the oxalic acid? Answer in units of M.

    asked by Andrea on May 29, 2016
  2. Chemistry

    Prepare M/20 oxalic acid solution.Using this solution, find molarity, strength, and percentage purity of the sodium hydroxide solution.

    asked by Sara on June 13, 2016
  3. Chemistry

    The amount of oxalic acid in a sample was determined by the reaction: 2Fe3+ + H2C2O4 + 2H2O----> 2Fe2+ + 2CO2 + 2H3O+. In an analysis, 10.62g of sample required 36.44 ml of 0.013 M Fe3+. Calculate the %w of oxalic acid in the

    asked by Jimmy on September 1, 2008
  4. General Chemistry

    Carbonic acid forms when carbon dioxide dissolves in water. A typical can of soda contains a 0.120 M solution of CO2. Assuming that all dissolved CO2 is present as carbonic acid, and that no other substances dissolved in solution

    asked by Erik on March 11, 2016
  5. chemistry

    oxalic acid, h2c2o4, is a weak acid capable of providing two H3O+ ions. ka=.059 k2=6.4E-5 the [h3o]+ in a .38 M solution of h2c2o4 is .12M and can be calculated by the first ionization step only. what is the equilibrium

    asked by anonymous on December 4, 2010
  6. Chemistry

    H2C2O4(aq) + 2 NaOH(aq) → Na2C2O4(aq) + 2 H2O(l) If I use 0.025 moles of NaOH to neutralize the Oxalic acid, how many moles of Oxalic acid are there?

    asked by Donnie on October 21, 2014

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