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Consider a saturated solution of Zinc arsenate, Zn3(AsO4)2, in which the following reactions can occur: Zn3(AsO4)s (s) --> 3Zn+2 + 2AsO4 -3 Ksp=1.0e-27 AsO4 -3 + H2O ---> HAsO4 -2 + OH- Kb1=3.1e-3 HAsO4 -2 + H2O ---> H2AsO4- + OH- Kb2=9.1e-8 H2AsO4- + H2O ---> H3AsO4 + OH- Kb3=1.7e-12
A first order decomposition reaction is observed to have the following rate constants at the indicated temperatures. using an Arrhenious plot, find the activation energy
Calculate the final temperature when a 20.4 gram sample of ice at 0oC is placed into a styrofoam cup containing 111 grams of water at 72.7 oC. Assume that there is no loss or gain of heat from the surroundings.
a block of aluminum with the volume of 96.5 g absorbs 65.3 J of heat. If the initial temperature is 31.2 degrees celcius, what is the final temperature.
A mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] 5.0 x10-3 M [O2] 1.9 x10-3 M [SO3] 6.9 x 10-3 M Is the reaction at equilibrium
Calculate the pH of a solution that is 0.20 M HOCl and 0.90 M KOCl. In order for this buffer to have pH=pKa, would you add HCl or NaOH?
Given your knowledge of complex ion formation, what do you expect to happen to the solubility of ZnS(s) in a solution containing excess NH3?
For the reaction, A = B + C, the rate law is k[A]. If it takes 80.0 seconds for 70.0% of a 10.0 gram sample of A to be transformed into products, what is the value of the rate constant.
Ferrocene cannot be nitrated using the conventional HNO3-H2SO4 mixed acid conditions, even though nitration is an electrophilic
A multiple stage evaporate process concentrates a weak solution of LiOH from 4.48 wt% to 26.78wt%. This evaporator processes 10 metric tonnes of solution each day.
if a 1.00 g piece of gold (density = 19.32 g/cm^3) is hammered into a sheet 8.0 x 5.0 ft what is the average thickness of the sheet in meters?
Calculate the number of millimoles of HCl needed to reach the methyl orange end point. b. How many millimoles of Na2CO3 reacted with the HCl?
Determine the amount of heat (in kJ) given off when 1.89 104 g of ammonia are produced according to the following equation. Assume that the reaction takes place under standard-state conditions at 25.0°C.
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