Empirical formula for acetic acid
The empirical formula for acetic acid is CH2O. Its molar mass is 60 g/mol. The molecular formula is
A. C2H4O2
B. C2HO2
C. none of the above
D. CH2O
E. C2H6O
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Carbon monoxide and water vapor, each at 200. Torr, were introduced into a 250. mL container. When the mixture reached equilibrium at 700.°C, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the following equilibrium.
The filtrate after the removal of the black precipitate was basified with 6M ammonia. This when treated with 3M ammonium carbonate, it gave a white precipitate. This white precipitate was dissolved in 6M acetic acid and basified with ammonia(6M).
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The average pH of precipitation in rural areas is 7.00. Assuming that the pH is controlled by the carbonate system, i.e., no anthropogenic acid gases are present in the atmosphere.
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In the reaction between potassium carbonate and calcium nitrate (balanced eq: K2CO3 + Ca(NO3)2--> K2(NO3)2 + CaCO3), why wouldn't ...--->2KNO3 +CaCO3 be right?
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