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Calculate the number of moles in each of the following: a) 85.2 g of Ni, b) 144 g of K, c) 6.4 g of H2O, d) 308 g of BaSO4, e) 252.8 g of fructose C6H12O6
When determining the pressure of dry hydrogen gas, explain how the measured atmospheric pressure is corrected for the presence
What mass of sucrose should be combined with 488 of water to make a solution with an osmotic pressure of 8.25 at 280.
why metal sulfide compounds can only form after the hydrothermal fluids escape into the open seawater.
Calculate the mass of nitrogen dissolved at room temperature in an 96.0 home aquarium. Assume a total pressure of 1.0 and a mole fraction for nitrogen of 0.78.
Choose the stronger of each pair of acids, respectively, and explain why: a) HBrO3 or HBrO b) HBrO2 or HIO2 A. a) HBrO because Br has a lower oxidation state (fewer number of O atoms around it) in HBrO than in HBrO3
Calculate the vapor pressure (in torr) at 298 K in a solution prepared by dissolving 19.1 g of the non-volatile non-electrolye urea {CO(NH2)2} in 108 g of water.
In 0.1592 M solution, a weak acid, HA, is 7.11% ionized. Calculate the ionization constant for the weak acid.
If 18.2 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia.
306 mL of a .208 M solution of silver nitrate will react with 146mL of a .170 M solution of sodium phosphate to produce how many grams of silver phosphate precipitate?
How many liters of NO(g) can be made from 17.57 L of O2(g) and 16.55 L of N2(g) at STP?
Using standard free energy of formation values given below, calculate the equilibrium constant K_p of the reaction
A solution is prepared by adding 0.14 mole Na2HPO4 and 8.2 grams of NaH2PO4 to sufficient water to prepare a 1.00 L solution. What is the pH of the solution?
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