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Find the approximate pH range suitable for the separation of Fe3+ and Zn2+ ions by precipitation of Fe(OH)3from a solution that is initially 0.015 M in both the ions. Assume a 99% precipitation of Fe(OH)3.
Calculate the pH of the following aqueus solution: 0.61 M NH4Cl (pKb for NH3=4.74)
When heated, ammonium carbonate decomposes as follows. NH4CO2NH2(s) ->2 NH3(g) + CO2(g) At a certain temperature the equilibrium pressure of the system is 0.318 atm. Calculate KP for the reaction.
What are some reasons why there would be a difference between the expected and actual values for the moles of copper oxide produced from heating copper in the air.
A piece of a newly synthesized material of mass 25.0 g at 80.0C is placed in a calorimeter containing 100.0 g of water at 20.0C. If the final temperature of the system is 24 0C
Write and balance the equation for the complete combustion of ethane, C2H6. You do not need to include any phase symbols
A voltaic cell consists of Pb/Pb2+a half-cell and a Cu/Cu2+ half-cell at 25 . The initial concentrations of and are 5.10×10?2 and 1.60 , respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.360 V?
The flask was then shaken until the solution was uniform. A 40.0-mL sample of this glucose solution was diluted to 0.500 L. How many grams of glucose are in 100 mL. of the final solution?
Which one of the following salts, when dissolved in water, produces the solution with the lowest pH
Calculate the equilibrium concentration of each compound if 3.10 moles of COBr2 are placed in a 3.00 liter flask at a certain temperature. Kc = 0.140 for the reaction at this temperature.
determine the numerical values for them the subscript hot, cold, and total stands for the hot brick, the cold brick and the sum of the two.
Calculate the molality of the unknown compound (m). m=mol of solute X particles per formation / mass of solvent , kg Data given: Mass of test tube , flask, t-butyl alcohol and unknown
What are the equilibrium concentrations of monomer and dimer at 25?C in a solution prepared by dissolving 3.4×10?2mol of pure acetic acid in enough benzene to make
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