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The solubility of CaSO4 in pure water at 0.0 C is 1.13 gram per liter; what is the value of solubility product?
Determine the wavelength, of an alpha particle with a(KE) kinetic energy of 8.0 10-13 Joules
What is the molarity of an NaCl solution prepared by dissolving 9.3g NaCl in sufficient water to give 350mL of solution.
Find delta H for the solution of one mole of NaOH in H2O If calorimeter constant is 11 cal/deg C
What is the complete wavefunction for n=2, L=0, and m(sub L)= 0? What radius of the orbital specified is required to contain 95% probability of finding an electron?
how many grams of potassium bromide are required to prepare 350 mL of a .200 M solution.
what is the mass, in kilograms, of Avogadro's number of olympic shot put balls if each one has a mass of 16lb? How does this compare with the mass of Earth, 5.98x10^25 kg.
The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust and other resources is about 26 million tons. the equation for the reaction is S + O2= SO2.
Find the volume of a molar solution and What volume of a 2.00 molar solution of sulfuric acid, H 2 SO 4 , is required to react with 250.0g of magnesium carbonate, MgCO 3 , according to the following equation?
Iincreasing the total pressure on the system by decreasing its volume, (c) adding gaseous I2 to the reaction mixture?
A student analyzed and recorded two potassium emission spectra: 1) one using 0.10 M Potassium sulfate solution; 2) one using 0.10M Potassium nitrate solution;. Determine why will significant differences be observed in the two emission spectra.
What scientific principle or law is used in the process of balancing chemical equations. Define the terms limiting reactant and excess reactant.
Green light of a wavelength 516 nm is absorbed by an atomic gas. What is the energy difference between the two quantum states involved in the transition.
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