5. A buffer solution contains 10.0 mmol of formic acid (HCOOH) and 15.0 mmol of formate (HCO0). If the solution pH is 3.95, then what is the Ka of formic acid? (а) 7.5 х 10-5 (b) 1.1 х 104 (c) 4.1 x 102 (d) 1.7 x 10-4
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Q: 3. What is the value of k"?
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- What is the pH of a of 0.450 M NaCN? The Ka for hydrocyanic acid is 4.9 × 10-10?Can someone help me with the problem below? CH3NH2 is a weak base (Kb=5.0×10−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a solution that is 0.0490 M in CH3NH3NO3 at 25 ∘C?A solution that is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2 ) and 8.0×10−2 M in propionic acid (C2H5COOH or HC3H5O2 ). The Ka of propionic acid is 1.3×10-5. What is the PH?
- If acetic acid has a Ka of 1.8 x 10-5, what would be pH corresponding to the half-equivalence point in the pH curve of acetic acid? Please round your answer to 3 sig figs. pH has no unit.NH3 is a weak base (?b=1.8×10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.061 M in NH4Cl at 25 °C?Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as antioxidants in soaps. Hydroxylamine has Kb of 9.1 × 10–9. What is the pH of a 0.054 M HONH2 solution? Please report 2 decimal places.
- The pKa of acetic acid is 4.74. The conjugate base of acetic acid (CH3COOH) is sodium acetate (CH3COONa). One has two stock solutions. One is 0.10 M in acetic acid and the other is 0.2M in sodium acetate. If one mixes 200 Ml of the acetic acid solution with 100 mL of the sodium acetate solution, what would be the final pH?What is the pH of a solution that is 0.29 M KOCN and 0.14 M HOCN (cyanic acid)? (Ka for HOCN is 3.5*10^-4.)What is the pH of a vinegar with 25.65 % (w/v) acetic acid in water? The pKa of acetic acid is 4.497. Record your answer with 2 decimals.
- A 0.250M solution of an unknown acid has a pH of 5.473. What is the Ka Answer: of this acid?A solution of acetic acid CH3COOH, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.68, what was the initial concentration of the acid? Ka=1.7x10-5 Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonia-like odour used to remove hydrogen sulphide from natural gas. A 0.15 mol dm-3 aqueous solution of ethanolamine has a pH of 11.34. What is kb for ethanolamine? What is the concentration of hydroxide ion in a 0.060 mol dm-3 aqueous solution of methylamine, CH3NH2? What is the pH? Kb=4.4x10-4Determine the pH of the following solutions, given that Ka (HF) = 6.8 x 10-4.Hint: 1. Diagnose the scenario (i.e. strong acid + weak base, etc.), 2. If buffer solution, make useof Henderson-Hasselback eqn and 3. If strong acid/base added to buffer, write out reaction withstrong acid or base on the left hand side, then calculate ICE change. a. 0.5 moles of NaF b. A solution with 0.5 moles HF (Ka = 6.8 x 10^-4) and 0.5 moles NaF, to which 0.1 moles HClis added.