Calculate the in a solution that is in and in . ()
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Use the Henderson-Hasselbalch equation to calculate the pH of each solution:
a solution that is 0.165M in HC2H3O2 and 0.120M in KC2H3O2
a solution that is 0.225M in CH3NH2 and 0.120M in CH3NH3Br
Acetonitrile CH3CN is a polar organic solvent that dissolves a widerange of solutes, including many salts. The density of a 1.90 MLiBr solution in acetonitrile is 0.827 g/cm3a)Calculate the concentration of the solution in molality.b)Calculate the concentration of the solution in mole fraction ofLiBrc)Calculate the concentration of the solution in mass percentage ofCH3CN .
Part A:
Calculate the pH of a solution that is 0.250 M in sodium formate (HCOONa) and 0.110 M in formic acid (HCOOH).
Part B:
Calculate the pH of a solution that is 0.520 M in pyridine (C5H5N) and 0.470 M in pyridinium chloride (C5H5NHCl).
Part C:
Calculate the pH of a solution that is made by combining 55 mL of 0.040 M hydrofluoric acid with 125 mL of 0.120 M sodium fluoride.