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Presume you desire to prepare an acetic buffer at pH = 3.95 by adding 0.200 M KOH to 200.00mL of 0.300 M acetic acid CH3COOH. Explain how much volume of the base do you need in order to prepare such a buffer solution?
Two different solutions were prepared. Solution A was prepared by dissolving sodium acetate in methanol and solution B was prepared by adding potassium methoxide to acetic acid.
Consider the following electrochemical cell at 298 K. One compartment contains a 1.00-M solution of silver nitrate. The other compartment contains a saturated solution of silver iodide
Draw the phase diagram of water and put a on the phase diagram to show the pressure and temperature conditions in the day and at night on the moon.
a man with a mass of 60 kg steps into powdery snow and sinks to his waist. the area of each mans feet is 250
Your friend brings you a 1.50 M sample of HONH3Cl and wants yo know the pH. You politely ask for the Ka of the acid and she responds that she only knows that the Kb for HONH2 = 3.0 x 10^-6
Why do I add strong acid (e.g. HCl) to the salt of a weak acid (ammonium acetate) to bring UP the pH of the buffer solution from the pKa
draw the shape of the molecules and give the orbital geometry around the central atom; the molecular geometry; and give the hybridization state
What is the millimolar solubility of oxygen gas, in water at 16 , if the pressure of oxygen is 1.00 ?
what is the maximum mass of sucralose (C12H19Cl3O8) you can add to 3.0 kg of pure water and still have the solution freeze? Assume that sucralose is a molecular solid and does not ionize when it dissolves in water
Three moles of C(s) are heated from 300K to 600 K at constant P. Over the temperature range, Cp = -12.19 + 0.1126 T/K - 1.947 x 10-4 T^2/K^2. Find delta H and delta S.
How much heat (in kJ) is evolved in converting 1.20 mol of steam at 134.0°C to ice at -55.0°C.
The normal boiling point of ethanol is 78.4 C, and the heat of vaporization is Delta H vap = 38.6 kJ / mol.
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