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A 1.268 g sample of a metal carbonate (MCO3)was treated with 100.00 mL of 0.1083 M...

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Chemistry

A 1.268 g sample of a metal carbonate (MCO3)was treated with100.00 mL of 0.1083 M sulfuric acid (H2SO4), yielding CO2 gas andan aqueous solution of the metal sulfate (MSO4). The solution wasboiled to remove all the dissolved CO2 and was then titrated with1.241×10−2 MNaOH. A 91.86 mL volume of NaOH was requiredto neutralize the excess H2SO4.

A) What is the identity of the metal M?

B) How many liters of CO2 gas were produced if the density ofCO2 is 1.799 g/L?

Answer & Explanation Solved by verified expert
3.9 Ratings (406 Votes)
Total moles H2SO4 molarity H2SO4 volume H2SO4 in Liter Total moles H2SO4 01083 M 0100 L Total moles H2SO4 001083 mol moles NaOH used molarity NaOH volume NaOH in Liter moles NaOH used 1241 x 102 M 9186 x 103 L moles NaOH used 114 x    See Answer
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