The cyanide ion is the conjugate base of the weak acid hydrocyanic acid. The value of Kb for CN-, is 2.50×10-5. Write the equation for the reaction that goes with this equilibrium constant.   ____ + _____ --> ____ + _____

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Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).

Benzoic acid (Ka = 6.6 X 10^-5) is present in many berries. Calculate the pH and % ionization of a 948 mL solution that contains 0.116 mol of benzoic acid. pH = ______ % ionization = ______ %

Ascorbic acid (H,C,H,O,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and Ka2 = 1.60 x 10-12. Determine the pH of a 0.118 M solution of ascorbic acid. 4.09 pH Incorrect Determine the equilibrium concentrations of all species in the solution. [H,C,H,O.] M %3D Incorrect [HC,H,0;] = M Incorrect (C,H,0;-] =| M Incorrect

Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+ (aq) a.Suppose a strong base (OH-) is added to the buffer system above. Which two species could react and why? b.Write the chemical reaction for the reaction of hydroxide ion (OH-) being neutralized by reacting with the hydrofluoric acid. c.Explain why the addition of a small amount of strong base will not cause a significant change in the pH of the solution as long as the HF is not used up. d. Suppose a strong acid (H3O+) is added to the buffer system above. Which species could react and why? e.Write the chemical reaction for the reaction of hydronium ion (H3O+) being neutralized by reacting with the fluoride ion. f.Explain why the addition of a small amount of strong acid will not cause a significant change in the pH of the solution as long as the fluoride ion (F ̄) is not used up.