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What is the molar solubility of AuCl (Ksp=2.0 x 10^-13) in pure water at 25 degrees Celcius?
A galvanic cell is produced as follows: Left half-cell has a Pt wire dipping into a beaker containing an equimolar mixture of Cr+2 and Cr+3 . [Cr3+ + e-??Cr+2 E°-= -0.42 V] Right hand cell has a Tl rod immersed in 1.00 M TlClO4.
A person ate 0.919 pound of cheese (an energy intake of 7350 kJ). Suppose that none of the energy was stored in his body. What mass (in grams) of water would he need to perspire in order to maintain his original temperature? (It takes 44.0 kJ to v..
For the reaction, calculate how many moles of the product form when 0.048 moles of O2 completely reacts. Assume that there is more than enough of the other reactant. 4Fe + 3O2 ---> 2Fe2O3
A 10.0 mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization.
Calculate the pH of a buffer solution obtained by mixing 400.0 mL of 0.200 M acetic acid solution and 100.0 mL of a 0.300 M sodium hydroxide solution.(The pKa of Acitic Acid, CH3OOH is 4.74)
Use simple structure and bonding models to account for why xenon is capable of forming compounds like XeF4 while argon is not.
Two liters of argon gas at 300 K and 5 atm are expanded against a constant opposing pressure of 1 atm until mechanical equilibrium is achieved.
If the alkalinity of the spring water is due only to the presence of carbonate and bicrabonate, what are the concentrations of each of them
As part of an internship in a petrochemical company you are given the task of identifying the fractions coming off the distillation tower. The current fraction shows a 1H NMR with only peaks for methyl (CH3) and methylene (CH2) groups
When a 0.6333-g sample of a compound of carbon, hydrogen and sulfur was burned in excess oxygen, 0.9272 g CO2, 0.3795 g H2O and 0.6749 g SO2 were obtained. In a separate experiment, it was found that, for fixed temperature and pressure
Calculate the volume of ammonia required to bring the pH to 3.00 and to 8.00. Kb (NH3) = 1.8 x 10^-5.
The molar solubility of calcium phosphate. b) The molar concentration of calcium ions at equilibrium. c) The molar concentration of phosphate ions at equilibrium.
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