Thursday
March 23, 2017

Post a New Question

Posted by on Monday, December 3, 2012 at 10:31pm.

a 110 g solid sample that is a mixture of CaCO3 and CaCl2 is reacted with 1.50 L of 1.45M HCl. Of the calcium salts, only calcium carbonate reacts with HCl- the reaction forms CaCl2 and CO2. The excess/unreacted HCl requires 0.850 L of 0.543 M NaOH to titrate it to the endpoint.
Determine the mass and mass percent of calcium carbonate in the original solid sample

  • Chemistry - , Tuesday, December 4, 2012 at 12:06am

    CaCO3 + 2HCl ==> CaCl2 + H2O + CO2

    1. mols HCl added = 1.5L x 1.45M = about 2 mol HCl but you need to do it more accurately. That reacts with all of the CaCO3 but doesn't use all of the HCl.

    2. Excess HCl requires how many mols. That's 0.850L x 0.543M NaOH = about .46 mols NaOH.

    3. mols HCl used = about 2 - 0.46 = about 1.5.

    4. Use the coefficients in the balanced equation to convert to mols CaCO3. That is mols HCl x 1/2.

    5. mass CaCO3 = mols x molar mass

    6. %CaCO3 = (mass CaCO3/mass sample)*100 = ?

Answer This Question

First Name:
School Subject:
Answer:

Related Questions

More Related Questions

Post a New Question