A 20.00-mL sample of hard water (with Mg2 added) is titrated with 0.0105 M EDTA. A blank solution with the same amount of Mg2 requires 2.35 mL of EDTA to reach its end point. A total of 34.13 mL of EDTA was used for the titration of the 20.00-mL sample of hard water (with Mg2+ added). M. W. CaCO3= 100.1 g/mol. Requried:
a. How many moles of EDTA are rquired to titrate the Ca²+ present in the 20.00-mL sample?
b. Assuming that Cat is present as Cacos, how many grams of CaCO3 are there in 20.00 mL of hard water?
c. What is the concentration of CaCO3 in parts per million?

iron and sleel

make siroeel

sorry i was late, but i don't know what assignment your talking about, i'm in flvs as well, im in earth space science. but u are behind pace bc every class should be in the 3's or 4'

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.