analytical chemistry

posted by .

An EDTA solution is standardized against a solution of primary standard CaCO3 (0.5622 g dissolve in 1000 ml of solution) and titrating aliquots of it with the EDTA. If a 25.00 ml aliquot required 21.88 ml of the EDTA, what is the concentration of the EDTA?

  • analytical chemistry -

    mols CaCO3 = grams/molar mass
    M CaCO3 = mols/L
    mol = 0.5622/100 = 0.005622 and that is in 1L; therefore M = 0.005622M.
    Then I would use
    MEDTA x 21.88mL EDTA = MCaCO3 x 25.00 mL CaCO3. Solve for MEDTA

  • analytical chemistry -

    first get for the moles of CaCO3
    mols CaCO3= 0.5662g*(1mol CaCO3/100gCaCO3)
    Molarity of CaCO3= mols CaCO3/L of solution
    =0.005622mols/1L
    M EDTA= [(molarity CaCO3)(mL aliquot)]/
    mL of EDTA
    M EDTA= [(0.005622)(25)]/21.88
    = 0.00642 M

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    25.00 mL aliquots of the solution from Part 1 are titrated with EDTA to the Eriochrome Black T end point. A blank containing a small measured amount of Mg2+ requires 2.60 mL of the EDTA to reach the end point. An aliquot to which the …
  2. Chemistry

    A 15.00 ml sample of a standard solution containing 1 g of CaCO3/L required 8.45 ml of EDTA to fully complex the Ca present. Calculate the volume of EDTA stoichiometrically equivalent to 1.0 mg of CaCO3.' Sorry, forgot to write the …
  3. Chemistry

    A 25.00 ml sample of a standard solution containing 1 g of CaCO3/L required 25.20 ml of EDTA to fully complex the Ca present. Calculate the volume of EDTA stoichiometrically equivalent to 1.0 mg of CaCO3. From the volume of EDTA required …
  4. Chemistry

    The reaction of a metal ion, M^2+, with EDTA is given in the following equation: M^2+(aq) + Y^4-(aq) <==> MY^2-(aq) The EDTA was standardized with a 0.04 M Zn^2+ solution. 25.05 mL of EDTA solution was used to titrate the Zn^2+ …
  5. analytical chemistry

    In an experiment for determining water hardness, 75.00 ml of a water sample required 13.03 ml of an EDTA solution that is 0.009242 M. What is the ppm CaCO3 in this sample?
  6. Analytical chemistry

    A 25.0-mL solution of 0.0660 M EDTA was added to a 33.0-mL sample containing an unknown concentration of V3 . All V3 present formed a complex, leaving excess EDTA in solution. This solution was back-titrated with a 0.0450 M Ga3 solution …
  7. analytical chemistry

    A solution containing both Fe 3+ and Al 3+ can be selectively analyzed for Fe 3+ by buffering to a pH of 2 and titrating with EDTA. Th e pH of the solution is then raised to 5 and an excess of EDTA added, resulting in the formation …
  8. Chem 2

    A 100-mL sample of water is titrated with EDTA solutions in problem 2. The same amount of Mg2+ is added as previously, and the volume of EDTA required is 31.84mL. What volume of EDTA is used in titrating the Ca2+ in hard water?
  9. Chemistry

    An EDTA solution is standardised against high-purity CaCO3 by dissolving 0.4835 g CaCO3 in HCl, adjusting the pH to 10 with ammoniacal buffer and titrated with an EDTA solution. If 35.18ml were required for the titration, what was …
  10. Chemistry (Re-post)

    A solution contains 1.694 mg of CoSO4 (MW 155.0) per mL. Calculate a) The volume of 0.008640 M EDTA needed to titrate a 25.00 ml aliquot of this solution. So this is my working out for this section, Step 1. Moles of CoSO4 = 0.0001694mg …

More Similar Questions