Calculate the pH of an alkaline (or basic) buffer solution. You can rewrite the Henderson-Hasselbalch equation for bases: pOH = pKb + log ([B+]/[BOH]), where "pKb" is the base's dissociation constant, "[B+]" stands for the concentration of a base's conjugate acid and "[BOH]" i...
Chemistry question. Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 230 mg/L. A solution with a pH of 9 has EXACTLY how many H+ ions compared to a ...
Calculate the pH of a buffer that contains 0.60 M NaHCO3 and 0.72 M Na2CO3. Calculate the pH of a buffer that is 0.105 M in NaHCO_3 and 0.125 M in Na_2CO_3. (b) Calculate the pH of a solution formed by mixing 65 mL of 0.2...
Decide on the pH for your buffer. This pH should be within one pH unit from the pKa of the acid/conjugate base. So, you can prepare a buffer at pH 2 or pH 7, for example, but pH 9 would be pushing it. Use theHenderson-Hasselbachequation to calculate how much acid and base you ...
Carbonic acid is a weak acid in aqueous solution; Ka for the first acid ionization is equal to 4.2 x 10-7. Calculate pKb for the hydrogen carbonate ion HCO3-. a. 5.2 b. 8.9 c. 6.4 d. 4.2 e. 7.6When solutions of carbonic acid and sodium hydroxi...