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When aqueous solutions of lead( II) ion are treated with potassium chromate solution, a bright yellow precipitate of lead( II) chromate, PbCrO4, forms. How many grams of lead chromate form when a 1.00- g sample of Pb( NO3) 2 is added to 25.0 mL of 1.00 M K2CrO4 solution?
Compute the heat capacity of the calorimeter in J/K assuming that no heat leaks or out of the calorimeter.
If the water in a well has 1000.0 mg/L of CaCO3 dissolved in it, How many grams of Na2C2O4 could you mix with 100.0 mL of that water before a precipitate would form
Calculate the change in internal energy of the gas in each case of these processes.
Experimental solid-oxide fuel cells that use butane (C4H10) as the fuel have been reported recently. These cells contain composite metal/metal oxide electrodes and a solid metal oxide electrolyte. Consider the following unbalanced half-reactions:
Calculate the mass of sodium hydroxide that must be added to 1.00 L of 1.00 M HC2H3O2 to double the pH of the solution (assume that the added NaOH does not change the volume of the solution). Ka of HC2H3O2 = 1.8 x 10 ^-5
A titration is performed by adding 0.400 M KOH to 40.0 mL of 0.300 M HCl. What is the pH after addition of 5.0 mL of the base?
The H2O molecule has a bond angle of 105. What type of atomic orbitals does oxygen use to form the two equivalent sigma bonds with H
A 0.9161 g sample which contained monoprotic lactic acid, was dissolved in 75.0 ml of water and titrated to the equivalence point with 32.25 ml of a 0.1057 m NaOH solution.
What mass of copper would you expect to be deposited from a copper (II) sulphate solution using a current
What is the pressure in a 10.0L cylinder filled with .448 mol of nitrogen gas at a temperature of 315k
Draw the atomic orbital diagram for the valence electron in Selenium (S) and then indicate the quantum numbers?
Calculate the number of moles of liquid propane that can be stored in the same volume if the density of the liquid is 0.590 {rm{g}}/{{rm{mL}}}.
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