For problems 2 & 3, the density of the sample is 0.9977 g/ml and the molar mass of calcium carbonate is 100.0 g/mol.
calculate the mass(in grams)of calcium carbonate present in a 50.00ml sample of an aqueous calcium carbonate standard, assuming the standard is known to have a hardness of 75.0 ppm (hardness due to caco3).
if the 50.00ml sample from problem 2 above was titrated with a 0.00500medta, what volume (in milliliters) of edta solution would be needed to reach the endpoint?

Thank you for posting your question here. 

For the question "Calculate the mass(in grams)of calcium carbonate present in a 50.00mL sample of an aqueous calcium carbonate standard, assuming the standard is known to have a hardness of 75.0 ppm (hardness due to CaCO3).", the answer is 3740gCaCO3 

For the question "If the 50.00mL sample from problem 2 above was titrated with a 0.00500MEDTA, what volume (in milliliters) of EDTA solution would be needed to reach the endpoint?", the answer is 7470.L of EDTA.

Ch4 is nonpolar and insoluble in water. since all of the hydrogen atoms are evenly spread around the carbon atom even through the c h bond is polar all the poles cancel each other out.

Hey how did you manage to type such a big lab report