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Zinc sulfide reacts with nitric acid to give zinc sulfate and nitric oxide. Calculate the mass of zinc required to react with 110 mL of 0.15 M nitric acid.
Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.
The solubility of CO2 in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility under atmospheric conditions? (The partial pressure of CO2 in air is 0.0003 atm.) Assume that CO2 obeys Henry's law.
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ? CO(g) + H2O(g) The equilibrium concentrations of the reacting species.
calculate the number of moles of AgCrO4(Ksp=9.0x10^12) that will dissolve in 1.00L of 0.010 M K2CrO4 solution. what will be the ion concentrations at equilibrium?
what is the concentration of a nitric acid solution if a 10.00ml sample of the acid reqires 31.25ml of 0.135m koh for neutralization.
What is the molality of a solution that contains 2.93 grams of urea (molar mass = 60.0 g/mol) in 141 grams of benzene.
Multiple choice questions in Radioactive Decay - electron emitted from the nucleus during some kinds of radioactive decay is known
The products of the fastest inactivation process are as explain the mechanism is accountable for the making of the products.
The density of so-called "heavy water"=1.1053 g/mL at 20 0C. determine what would be the mass of the flask when filled with heavy water?
Assume that the wet limestone process requires 1 metric ton of calcium carbonate to remove + 85.0 % of the sulfur from 4 metric tons of coal containing + 10.0 % S Assume that the sulfur product is calcium sulfate.
A sample containing 4.80 g O2 of gas has a volume of 15.0 L. Pressure and temperature remain constant. What is the new voume if 0.500 mole O2 gas is added.
what mass of Na2SO4 is needed to prepare 350. ml of a solution having a sodium ion concentration of 0.125 M.
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