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Student prepared .10M solution of formic acid and found it's pH at 25 Celsius to be 2.38. What is the pKa of formic acid at this temperature?
If a 1.00 L flask is set up with an initial concentration of 0.391 mol/L COCl2, calculate the equilibrium concentration of carbon monoxide in mol/L.
A compound is 40.0% C , 6.70% H, and 53.3% O by mass. Assume that we have a 100.-g sample of this compound. The molecular formula mass of this compound is 240 amu. What are the subscripts in the actual molecular formula?
Ozonolysis of A followed by dimethyl sulfide reduction produces a single optically active compound C, C5H8O2. Reduction of C with ethereal LiAlH4 affords optically active compound D (C5H12O2) of the (S)-configuration. The 13C NMR spectrum of D is ..
A solution of malonic acid, H2C3H2O4 was standardized by titration w.1000M NaOH solution. If 20.76 mL of the NaOH solution were required to neutralize completely 13.15 mL of the malonic acid solution
calibrated manufacturing makes an electronic component that is in great demand.nbspnbspthe component sells for 20
circle the correct choices to indicate how many electrons each element must gain or lose to form an octet
Calculate the atomic mass of neon (Ne) which is composed of three naturally occurring isotopes with the following natural abundances and masses
A fixed amount of gas at 25.0 °C occupies a volume of 8.66 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 155 °C while maintaining the pressure at 629 torr.
How many mL of a .1 N solution of NaOH must be added to a 25 mL solution of .1 N HAc to obtain a pH of 9.75? What is the concentration of HAc at this pH
calculate the ph that results when 100 mL a liquot of 0.0500 M is added to 400 M of a NH3/NH4+ buffer that is 0.200 M in NH3 and 0.300 M in NH4Cl
how many milliliters of .100 M NaOH are required to neutralize 50.00 mL of .215 moles of H2SO4
The freezing point of the solution decreases by 0.905 ° C compared to that of the pure solvent. What is the molar mass of the unknown solid. The freezing point depression constant for benzene is 5.46° C/m.
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