The presence of ca2 and turns blue when ca2 is removed

Reference no: EM13698598

Question- Hardness in groundwater is due to the presence of metal ions, primarily Mg2 and Ca2 . Hardness is generally reported as ppm CaCO3 or mmol/L Ca2 . To measure water hardness, a sample of groundwater is titrated with EDTA, a chelating agent, in the presence of the indicator eriochrome black T. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2 and turns blue when Ca2 is removed.

Red blue

Ca(ln)^2+ EDTA >>>> Ca(EDTA)^2+ln

A 50.00-mL sample of groundwater is titrated with 0.0750 M EDTA. Assume that Ca2 accounts for all of the hardness in the groundwater. If 14.10 mL of EDTA is required to titrate the 50.00-mL sample, what is the hardness of the groundwater in molarity?

What is the hardness of the groundwater in parts per million of CaCO3 by mass?

It is not a question in the book, so I just need the full solution of deriving

Reference no: EM13698598

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