A calcium based carbonate mineral powder (Mohs scale= 3.0) was characterized
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The hardness of a water sample (in terms of equivalents of $\mathrm{CaCO}_{3}$ ) containing $10^{-3} \mathrm{M} \mathrm{CaSO}_{4}$ is: (molar mass of $\mathrm{CaSO}_{4}=136 \mathrm{~g} \mathrm{~mol}^{-1}$ ) [Main Jan. 12, 2019 (I)] (a) $10 \mathrm{ppm}$ (b) $50 \mathrm{ppm}$ (c) $90 \mathrm{ppm}$ (d) $100 \mathrm{ppm}$
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A sample of dolomitic limestone, with a mass of 0.9142 g, is reacted with hydrochloric acid. The mass of carbon dioxide released is 0.4373 g. Assuming the sample has a 1:1 mole ratio of MgCO3 to CaCO3, where the mass of MgCO3 is 0.4190 g and the mass of CaCO3 is 0.4974 g. A 25.00 mL sample of water, buffered at a pH of 10, is titrated with 0.008989 M EDTA using the Calmagite indicator. A volume of 8.15 mL of EDTA is required. Determine the hardness of the water sample in ppm.
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1 gram sample taken from dolomite limestone was dissolved in acid and neutralized and taken into a 250 mL solution. 50 mL of this was adjusted to pH 10 with NH4+ / NH3 buffer and titrated with 20 mL 0.1 N EDTA solution with Eriochrome T indicator. Mg(OH)2 precipitate was removed by filtration and the filtrate was titrated with 7 mL of 0.1 N EDTA solution using the murexide indicator. (Only Ca2+ is titrated with the Murexide indicator). What is the MgCO3 and CaCO3% of dolomite? (Mw MgCO3: 84.32 g/mol, Mw CaCO3: 100.09 g/mol)
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