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Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 8.0×10-2 M NaOH.
A:lactic acid
B:sodium hydrogen chromate
A piece of silver of mass 362 g has a heat capacity of 85.7 J/C (celsius degrees). What is the specific heat of silver?
The precipitate was filtered, dried, and weighed. A total of 2.10 g calcium fluoride was collected. What was the percentage of CsF in the original sample?
what is the wavelength of a photon that has three times as much energy as that of a photon whose wavelength is 779 nm.
What is the half-life? b) How long would it take for the concentration of CH3CN to decrease to 25% of its initial value? c) To 12.5% of its initial value?
Determine the absolute error and relative error in ppm CaCO3 associated with a single standardization and titration of an unknown CaCO3 solution
what is the density of a piece of metal if it's mass is 201 g and its volume is 18.9 cm3
the electron configuration [Kr]4d10 5s2? How many unpaired electrons are there in the ground state of this ion?
If the initial concentration of cyclopropane is 0.150 M, what will the concentration of cyclopropane be after 22.0 hours? b) What is the half-life for the conversion process?
Reactions of Alcohols, Show how ethanol and cyclohexanol may be used to synthesize cyclohexyl ethyl ether using tosylation followed by Williamson ether synthesis.
The atomic mass of element X is 22.99 amu. A 19.98-g sample of X combines with 16.51 g of another element Y to form a compound XY. Calculate the atomic mass of Y.
Devise tests which allow you to distinguish between the ions in each case.
Express the concentration of a 0.0460 M aqueous solution of fluoride, F-, in mass percentage and in parts per million. Assume the density of the solution is 1.00g/mL.
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