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- We titrate a solution containing 10 mL of CH3COOH 0.1095 mol/L and 90 mL of distilled water, with NaOH 0.09220 mol/L, a strong base. What is, at equilibrium, the concentration of H3O+, CH3COO-, CH3COOH and the initial pH (using -log[ ])?Why must we prepare a buffer solution for a specific pH? Explain.If a buffer solution is 0.280 M in a weak acid (?a=1.6×10−5) and 0.510 M in its conjugate base, what is the pH?
- If a buffer solution is 0.180 M in a weak base (Kb=7.5×10−5) and 0.400 M in its conjugate acid, what is the pH?With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8x10-4. You add 60.7g hydrobromic acid to this solution, what is the new pH?Sample solution in the image. Compute for the pH, pOH, and [OH-] of a buffer solution that is 0.20 M in acetic acid and contains sufficient sodium acetate to make the acetate ion equal to 0.05 M. Ka = 1.85 x 10^-5.
- If a buffer solution is 0.230 M in a weak base (Kb = 4.7 × 10 − 5 ) and 0.540 M in its conjugate acid, what is the pH?An acid has a Ka= 1x10^-6 at what pH would this acid and it's corresponding salt make a good buffer?The addition of an acidic solution to a buffer solution with a pH of 8.3 would most likely result in the mixture having a PH close to ?
- The pOH of an acidic buffer is 9.725. What is the Ka of the acid if the ratio of [ionized] to [unionized] is 1380?Please help with the last question qhich i keep getting wrong Calculate the pH of the solution at the equivalence point with 0.2680.268 M HClHCl.The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with 56.8 mL of 0.106 M sodium acetate is ?