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Explain why is it important to maintain a constant temperature in this experiment? electrophilic aromatic substitution lab
Calculate the molality of a hydrochloric acid solution that is 26.4% by mass and has a density of 1.19 g mL^-1
the pH of the solution is 9.15. After adding 16.55 mL of hydrochloric acid to your sample, the pH is 8.78. Calculate the first derivative of the function of the pH of your solution with respect to the volume of titrant added
Solutions of AgNO3 and KCl are combined and 0.683 g of a precipitate are formed. What is the precipitate and how many moles were formed.
If 36.6 grams of hydrogen sulfide gas (H2S; MM = 34.08 g/mol) react with 35.6 grams of oxygen gas (O2, MM = 32.00 g/mol), what is the mass of sulfur dioxide (SO2, MM = 64.06 g/mol) gas produced
a sample of fluorine has a volume of 2.88 l when the temperature is 11.6 degc and the pressure is 649 torr. what will
A solution of H2SO4 and KI is then added to conver the MnO2 to MN^2+, and the iodide is converted to I2. The I2 is then titrated with standardized Na2S2O3. Calculate the amount of O2 in 25.0mL of water if the titration requires 2.45ml of 0.0112 M N..
1.2 mole of a monoatomic ideal gas that occupies a volume of 13L at 248K spontaneously and isothermically expands until its voulme is doubled.
An aqueous solution containing 5.85g of an optically pure compound was diluted to 800.0mL with water and placed in a polarimeter tube 10.0cm long. The measured rotation was -5.93degrees at 25degrees C. Calculate the specific rotation of the compou..
A balloon contains 0.120 of gas and has a volume of 2.83 .If an additional 7.2×10?2 of gas is added to the balloon, what will its final volume be
Ionization energy is the energy needed to eject an electron from an atom. Compute the ionization energy of a hydrogen atom in its third excited state (n = 4).
If the washes totaled 46.4 ml. how many grams of KAI(SO4)2 would be dissolved in the solution? consider the solubility begin 3.00 g/ml.
Under what conditions would you expect a real gas to be (a) more compressible than an ideal gas; (b) less compressible than an ideal gas
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