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A solid mixture weighing 5 gm consists of lead nitrate as well as sodium nitrate was heated below 600o C until weight of residue was constant. If the loss in weight is 28%, discover the amount of lead nitrate and sodium nitrate in mixture.
Strong, non-charged bases are useful in base-catalyzed reactions. Many non-charged nitrogen bases are commonly used in various reactions. Perhaps the strongest non-charged base is shown below
Explain why lattice energy calculations based on the born mayer equation reproduce the experimentally determined values to within 1 percent for LiCl but only 10 percent for AgCl given that both compounds have the rock salt structure
The pH of a 0.10 M nicotinic acid solution is 2.93. What is the approximate value of Ka for nicotinic acid, HC6H4NO2? Assume small percent dissociation. pH = ?log10[H+].
The conjugated system of a retinal consists of 11 carbons atoms and one oxygen atom. In the ground state of retinal. each level up to n=6 is occupied by 2 electrons.
explain why the carbonyl group co groupof methyl benzoate is a m-directing group. would you expect methylbenzoate to
The freezing point depression constant, Kf, for water is 1.86?C/m. Suppose that 5.00 g of mercury(I) nitrate was dissolved in 100.0 g of water
Five grams of the specified pure solvent is placed in a variable volume piston. What is the volume of the pure system when 50% and 75% have been evaporated at: (i) 30 deg C (ii) 50 deg C?
A microwave oven operates at 2.40 . What is the wavelength of the radiation produced by this appliance?
what is the mass percent of the helium in a mixture that has an equal number of He and CH4 molecules. 1.10%
Explain what is the heat released during reaction. Also what is the enthalpy of neutralization. Does doubling the volumes of acid and base double the amount of heat. Does doubling the concentration of acid base double the amount of heat released
How much ammonium hydroxide is needed to react completely with 75.0g of copper (2) nitrate in a double replacement reaction.
A 25.00 mL aliquot of iron solution was titrated to equivalence with 26.19 mL of 0.0215 M KMnO4. A procedure similar to the one in experiment 7 was followed. Calculate the moles of iron in the original volumetric flask.
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