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Calculate the amount (in mL) of a 1.520M NaOH that is required to add the following acetic acid solutions to prepare a buffer with the corresponding pH: pKa of acetic acid = 4.74 (a) 30.00mL of a 5.00% (w/v%) acetic acid; the resulting acetate buffer has a pH of 5.75 (b) 50.00mL of a 5.00% (w/v%) acetic acid; the resulting acetate buffer has a pH of 4.98 (c) 40.00mL of a 5.00% (w/v%) acetic acid; the resulting acetate buffer has a pH of 4.33 The mole of NaOH in the equilibrium table is a function of volume (i.e. MNaOH×V) and it will be the limiting reagent in the equilibrium table. I know I'm supposed to Set up an equilibrium table for a reaction between acetic acid and NaOH and then use the Henderson-Hasselbalch equation to determine the volume of NaOH (i.e. V) that is required to prepare the specific acetate buffer solution at the corresponding pH.
Show all the steps in the mechanism for the following reaction, When benzene is mixed with deuterated sulfuric acid, deuterium is slowly incorporated onto the ring. Show the mechanism for this reaction and explain how this relates the sulfonation of ..
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