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have been hired by a farmer to help her understand an observation she made. While trying to prepare a copper supplement for use on her farm, she observed the formation of a large volume of precipitant while trying to dissolve copper sulfate in the irrigation water from the well on her farm (which contains high levels of hydrogen sulfide). What explanation can you provide for this observation
The element lanthanum has two stable isotopes, lanthanum-138 with an atomic mass of 137.9 amu and lanthanum-139 with an atomic mass of 138.9 amu
Determine which of the following reactions are oxidation-reduction reactions and which are not. what type of reaction do you have if it is not an oxidation-reduction reaction?
what is the density of a piece of metal if it's mass is 201 g and its volume is 18.9 cm3
Calculate the hydrogen-ion concentration [H+] for the aqueous solution in which [OH-] is 1 x 10-11 mol/L. Is this solution acididc, basic, or neutral?
The acid-dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, 25) and Ka3 = 4.2 × 10-13 at 25.0 °C.
What would be the equilibrium pH value of rainwater if atmospheric SO2 gas were its only dissolved constituent? Assume that the fugacity (activity) of SO2 gas in the atmosphere is 5 x 10-9 bar
What volume of hydrogen gas is produced when 83.8 g of iron reacts completely according to the following reaction at 25oC and 1 atm.
Distilled water in the same tube gave a reading of +0.016 degrees. Calculate the specific rotation for the compound.
If aluminum is diffused into a thick slice of silicon with no previous aluminum in it at a temperature of 1100?C for 8 hours, what is the depth below the surface at which the concentration is 1016 atoms/cm3 if the surface concentration is maintain..
Describe at least four methods that could be used to attempt to separate the oil and water at home. Based on the four methods postulate which method would work better than the others.
A 44.2 L sample of a gaseous hydrocarbon, measured at 1.00 atm pressure and 25 C is burned in excess oxygen, liberating 2.55x10^3 kj of heat at constant pressure.
The density of lead is 11.4 g/cm3 at 25°C. Calculate the volume occupied by 25.0 g of lead.
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