Part A: Unknown Acid use 1gram and mix with 120 mL of distilled water Determine the concentration of the acid by titrating with 0.0998 M of NaOH Concentration of NaOH= 0.0998M Volume of NaOH= 3.5 mL # moles of NaOH= Initial
You need to determine the pKa of a weak, monoprotic acid. You add 0.500 moles of the acid to 1.00 L of water. The resulting pH was 1.87. What is the pKa of this weak acid? You may ignore the autoionization of water. 2.74 3.43 5.38
. Use the Henderson-Hasselbach equation: pH = pKa + log [A-]/[AH], where A- is the conjugate base and AH is the weak acid. Calculate the pH of an acetate buffer in which the acetate concentration [CH3COO-] is 3.5 times greater
Please someone Help!! Acetic acid, CH3COOH, is a weak organic acid, pKa 4.47. Determine the position of the equilibrium for the reaction of acetic acid with NaHCO3, and draw the species that predominates at equilibrium.