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Hi everyone, I'm looking at TBR Gen Chem Question in the book, example 4.13.
How many milliliters of 0.6M HCl are required to neutralize 3.0 grams CaCO3?
The answer gives this balanced reaction:
CaCO3 + 2 HCl --> CaCl2 + CO2 + H2O
Here's my though process. Since there are 2 molecules of HCl per molecule of CaCO3 we need to multiple 0.6M by 2 (because of the amount of acidic protons in solution) and then set that equal to .03 moles of CaCO3. We then solve for volume with the following equation:
2*.6M HCl*(x) = .03moles CaCO3
Could someone please clarify and provide an answer? Thanks!
How many milliliters of 0.6M HCl are required to neutralize 3.0 grams CaCO3?
The answer gives this balanced reaction:
CaCO3 + 2 HCl --> CaCl2 + CO2 + H2O
Here's my though process. Since there are 2 molecules of HCl per molecule of CaCO3 we need to multiple 0.6M by 2 (because of the amount of acidic protons in solution) and then set that equal to .03 moles of CaCO3. We then solve for volume with the following equation:
2*.6M HCl*(x) = .03moles CaCO3
Could someone please clarify and provide an answer? Thanks!