College Chemistry

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calculate the moles of sulfuric acid that remained in the solution after reaction with the carbonate.

the tared mass of carbonate is 1.5179g

  • College Chemistry -

    You didn't post all of the problem.

  • College Chemistry -

    i've calculated the moles of sulfuric acid present in the 50ml of standard acid solution to be 2.378x10^-1mol. the average volume of sodium hydroxide required for the back titration to be 31.03mL. and the moles of sodium hydroxide required for the back titration to be 2.951x10^-3. I'm not sure how to proceed

  • College Chemistry -

    You've still posted portions although the last helps. My guess is that you added an excess of a standard H2SO4 soln to a CO3^= unknown and you're back titrating to find amount of excess H2SO4 added.
    total mols H2SO4 added initially minus 1/2 the mols NaOH to back titrate gives you mols carbonate ion there originally in the unknown.

  • College Chemistry -

    im guessing im missing the concentration of H2SO4 is 0.04755M and concentration for sulfuric acid is 0.09510M. In the flash i have 50.00ml of sulfuric acid and 25.00ml of impure sodium carbonate solution.

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