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Problem: What is the pressure of a gas in millimeters of mercury in a sample container connected to a mercury-filled, open-ended manometer if the level of mercury in the arm connected to the atmosphere is 3.41 cm lower than the arm connected to the sample container and if atmospheric pressure is 99.54 kPa (101.325 kPa/1 atm)? Please explain the complete solution of this problem.
A peptide with the amino acid sequence C-P=T-Y-R-L-D-Q (MW = 995.12 g/mol) is dissolved in this solution at a concentration of 5 micromol.
At 22C(Celsius) an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.14. What is the Ksp of the salt at 22C
how many grams of dry nh4cl need to be added to 1.60 l of a 0.800 it m solution of ammonia nh3 to prepare a buffer
If 22 mL of 5.8 M H_2SO_4 was spilled, what is the minimum mass of NaHCO_3 that must be added to the spill to neutralize the acid.
The reactant concentration in a zero-order reaction was 9.00×10?2{\it M} after 100s and 2.50×10?2{\it M} after 390s . What is the rate constant for this reaction
Molecular equation reaction for copper sulfate penta-hydrate with heat (state of reactants and products must be shown) then when the anhydrous copper sulfates with water
imagine that you have a 5.00 gas tank and a 4.00 gas tank. you need to fill one tank with oxygen and the other with
a gas mixture consists of 320 mg of methane , 175 mg of ar and 225 mg of neon. The partial pressure of neon at 300 k is 8.87 kPa. Calculate the volume and the total pressure of the mixture
calculate the ph of a buffer made with 0.50m phosphoric acid and 0.75m sodium dihydrogenphosphate. ka 7.5 x
calculate the volume of water needed to dilute the anti-freeze from 0.20M in 0.260 litres to 0.13M.
Consider the titration of 25.0 mL or 0.010 M Sn^2+ by 0.050 M TI^3+ in 1 M HCL, using pt and saturated calomel electrodes to find the endpoint.
Express this mass of CO2 in grams without exponential notation, using an appropriate metric prefix.
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