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A 0.8500 gram sample containing KHC8H4O4 was dissolved in approximately 50 ml of water. This resulting solution required 28.50 ml of the NaOH solution that was morality from where the answer was 0.095M to neutralize it. Explain what percentage of the solid sample was pure KHC8H4O4? The formula weight of KHP is 204.22 g/mol.
Two flasks are connected with a stopclock. The first flask has a volume of 5 liters and contains nitrogen gas at a pressure of 0.75 atm. The second flask has a volume of 8 L and contains oxygen gas at a pressure of 1.25 atm.
The vapor pressure of water at this temp is 22.4 torr. How many grams of each product were formed and how many grams of 2-heptene and oxygen did you start? R= 0.0820578 L*atm/K*mol.
Draw the structure of the compound you would expect from E2 reaction of 2-chloro-3methylhexane with NaOH.
Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag+ in the balanced reaction. Cd(s) + Ag+(aq) ? Ag(s) + Cd2+(aq)
based on the synthesis chart provided in the organic course noteswhat is the smallest number of synthetic steps needed
What is the approximate ratio of the molar concentrations of CO_2(aq) in the soda before it is opened to that in the soda after it has been opened and reached equilibrium with the surrounding atmosphere
the nahco3nbspis the limiting reactant and the hcl is the excess reactant in this experiment. determine the theoretical
Calculate the concentrations of all species in a 1.66 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1=1.4x10^-2 and Ka2=6.3x10^-8.
Compute the molar concentrations of these gases under conditions typical of (a) the mid-latitude troposphere (10°C and 1.0 atm) and (b) the Antarctic stratosphere (200 K and 0.050 atm).
When 2.05 grams of aluminum metal are dropped in 650. mL of 6.0 M hydrochloric acid, how many liters of gas are evolved at 20°C, 1.07 atm
Chlorine gas will react with nitrogen gas when dissolved in water to yield NCl (aq). At 298 K, the equilibrium constant for this reaction is 1.817x10-4. If I mix 1.0 g of chlorine and 1.0 g of nitrogen in a 2 L flask, what would be the equilibrium..
Can someone please help me I need to A. Write the complete equation for each reaction that produced a precipitate
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