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Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8x10-5)
Determine the molecular formula of the oxide of phosphorous when it is in its gaseous state.
Use the table of standard reduction potentials to calculate the equilibrium constant at a standard temperature (25 degrees C) for the following reactions:
Qualitatively, describe how an acid-base indicator works. Why do we want to use a minimum amount of indicator in a titration? Select all that apply.
If 2.45 g of N2H4 reacts and produces 0.650 L of N2, at 295 K and 1.00 atm, what is the percent yield of the reaction?
Calculate the mass of silver chloride in grams required to make 4.4g of silver plating.
Up to Iron "Fe", the number of proton and neutron are about equal, after Fe the number of neutron began to rapidly increase, with respect to the number of proton, why?
certain temperature and pressure, one liter of CO2 gas weighs 1.85 g. What is the mass of one liter of CH4 gas at the same temperature and pressure?
How many kJ of energy are required to convert 747 grams of water (liquid) at 23.4°C to steam at 100°C? The following information is given for H2O:
In which compound does sulfur have the highest oxidation number a)Na2S2O3 b)NaHS c)H2S d)KHSO3 e) CuSO4
Explain how to purify a product using each of the 3 different techniques, elaborate on what these techniques achieve at the molecular level.
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K.
What is the final temperature of a 123.5 g of silver if the initial temperature was 25.5C and 31 kJ of heat was added
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