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A 0.481 gram sample of an unknown acid (HX) required 28.95 mL of 0.2013 M NaOH for neutralization to a phenolphthalein endpoint. What is the molar mass of the acid?
Dissolving 4.69g of an impure sample of calcium carbonate in hydrochloric acid produced 1.07 L of carbon dioxide (measured at 20.0 degrees Celcius and 737mmHg). Calculate the percent by mass of calcium carbonate in the sample.
An equilibrium mixture contains .870 mol I2, and .290 mol H2 in a 1.00 L flask. I found the equilibruim constant to be .172 which is correct.
Chemists studied the formation of phosgene by sealing 0.73 atm of carbon monoxide and 0.98 atm of chlorine in a reactor at a certain temperature. The pressure dropped smoothly to 1.32 atm as the system reached equilbrium.
explain why the coupling of the diazonium salt with a phenol or an aromatic amine occurs at the para position.
Determine the value of pH of given solutions that are (a) a solution that is 0.40 M CH3CO2H, (b) a 0.40 M CH3CO2H solution, (c) 0.20 M NaCH3CO2. And explain your answer too?
a 50.0 g sample of water is cooled from 30 degrees Celsius to 15 degrees Celsius losing 3140 J of heat What is the change in enthalpy.
What is the difference between selectivity and sensitivity as these words pertain to sensors? Why or why not would you want a very sensitive sensor?
An atmospheric chemist studying the pollutant SO2, places a mixture of SO2 and O2 in a 2.00 L container at 800k and 1.90 atm. when the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.65 atm
What would be the wavelength of a photon that would be able to break the Cl-Cl bond in Cl2. The bond energy in Cl2 is 243 kJ/mol.
In an aqueous solution that contains 285 mg of trichloroacetic acid (HA), Cl3CCOOH (163.4 g/mol) in 10.0 ml. Calculate: 1) Analytical molar concentrations of HA species
Identify the oxidation-reduction reactions among the following.
There is a stock 6.00m solution of sodium chloride available in the lab. What volume of this solution would you need to prepare your solution?
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