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17 Nov 2019
Plusminus Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H_3O^+], pK_a is the negative logarithm of K_a, pK_a = - log K_a The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: PH = pK_a + log [base/acid] Notice that the pH of a buffer has a value close to the pK_a of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and pK_b is similar. POH = pk_b + log[acid]/[base] Part B How many grams of dry NH_4 Cl need to be added to 1.90 L of a 0.500 M solution of ammonia, NH_3, to prepare a buffer solution that has a pH of 8.99? K_b for ammonia is 1.8 times 10^-5. Express your answer with the appropriate units. mass of NH_4Cl = 68.57 g
Plusminus Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H_3O^+], pK_a is the negative logarithm of K_a, pK_a = - log K_a The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: PH = pK_a + log [base/acid] Notice that the pH of a buffer has a value close to the pK_a of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and pK_b is similar. POH = pk_b + log[acid]/[base] Part B How many grams of dry NH_4 Cl need to be added to 1.90 L of a 0.500 M solution of ammonia, NH_3, to prepare a buffer solution that has a pH of 8.99? K_b for ammonia is 1.8 times 10^-5. Express your answer with the appropriate units. mass of NH_4Cl = 68.57 g
Trinidad TremblayLv2
12 Jan 2019