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An aqueous solution is 13.0% by mass ethanol, CH3CH2OH, and has a density of 0.978 g/mL. The molality of ethanol in the solution is?
Lethality of Carbon Monoxide, Sulfur Dioxide and TNT, Air monitoring provides the following contaminant concentrations at the approximate center of a fire scene in which acres of automobile tires are burning
Determine the molecular weight of a compound given the gas phase data: mass of 11.8 g, temperature of 39.1 C, pressure of 630 torr, volume of 1.31 L.
Metallic aluminum reacts with MnO_2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al.
She weighed an empty 4.3 L bulb, then filled it with the gas at 1.60atm and 23.0 C and weighed it again. The difference in mass was 7.9g . Identify the gas.
Calculate the solubility of zinc hydroxide, Zn(OH)2, in 1.00 M NaOH. Ksp = 3.0 × 10-16 for Zn(OH)2, Kf = 3.0 × 1015 for Zn(OH)42-
2 NH3 + CH3OH → products . How much NH3 is needed to react exactly with 21 grams of CH3OH
Calculate the wavelength () of the light in nanometers () corresponding to the energy change () value of this transition. You can use the following values for your calculations
A solution is 40% acetic acid by mass. The density of this solution is 1.049 g/mL. Calcu late the mass of pure acetic acid in 480 mL of this solution at 20 C
Q 3: The salt NaBrO(3) oxides Sn^2+ to SnCl(6)^2- in the presence of hydrochloric acid according to the equation
A weak acid HX has Ka = 1.00×10-6. What would be the pH of a 0.10 M solution of HX in water?
Show why this chemical is dangerous, by showing chemical reactions for its formation in the environment and its reactions in the atmosphere.
A .10M solution of the weak acid HCN has an equilibrium constant of 4.9 X 10^-10. Calculate the percent dissociation of the acid
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