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You titrate a 0.1000 M solution of a strong base (NaOH) with a 100.00 mL solution of 0.1000 M Formic acid (Ka = 1.80 x 10^-4). Calculate the pH at the following points 100.0 mL of NaOH added
What is the approximate pH of a solution of the salt NH4(O2CCH3) (ammonium acetate)? No calculations -- only reasoning needed. pKa/pKb values in your notes
A reaction has a rate constant of 7.69 M^-1s^-1 at 219 K and a rate constant of 3.36 *10^4 M^-1s^-1 at 344K. what is the activation energy for this reaction
Calculate the average bond energy of one O3 bond. What wavelength has just the right amount of energy to break the bond
If the solution is 40.0% K2CO3 by mass, what is the predicted freezing point of this solution in °C, assuming full ionization.
Compound A has a parent peak of M+ = 95 m/z in its mass spectrum and shows a medium intensity sharp infrared absorption band at 2280 cm. The HNMR of compound A shows 3 signals in a 4:4:1 ratio.
The piston is then moved in and the heat rejected by the air reversibly at constant pressure until the volume is= initial volume. compute The net heat flow and the overall change in entropy?
What is the pH of the solution formed by mixing 45.0 mL of 0.183 M potassium hydroxide and 65.0 mL of 0.145 M hydrochloric acid?
Find the number of moles of water that can be formed if you have 150mol of hydrogen gas and 70mol
Compare the electrical conductibities of Sodium Chloride (NaCl), ammonium nitrate (NH4NO3), calcium sulfate (CaSO4), and distilled water. Account for any differences noted in the electrical conductivities of these compounds.
A sample of gas occupies 7 ml at stp. at what pressure would this sample occupy 500 ml if the pressure was changed to 525 degrees c?
Using Wien's law, calculate the temperature a star must have for the peak wavelength of its blackbody curve to equal this value.
At this temperature, calculate the number of moles of NO2(g) that must be added to 3.12 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.
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