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You have a 0.776 M solution of the base pyridine. Kb = 1.7 x 10" Find...
Pyridine is a weak base with a Kb=1.7 x 10^-9. If 0.300 moles of pyridine is added to 1.00 L of water, what will be the equilibrium concentrations of the species below? a. [Pyridine] b.[Pyridine-H+] (the Pyridium ion) c.[OH-] 2. what is the pH of the solution in problem 4 above?
Calculate the pH of a 0.20 M solution of the weak base pyridine. (C5H5N; Kb = 1.7 x 10-9). What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 ´ 10–5]
Find the [OH−] of a 0.40 M pyridine (C5H5N) solution. (The value of Kb for pyridine (C5H5N) is 1.7×10−9.) Find the pH of a 0.40 M pyridine (C5H5N) solution.
A 250.0 mL solution contains two weak bases, pyridine (Kb = 1.7 x 10^-9) and caffeine (Kb = 4.1 x 10^-4). This solution contains 1.00 x 10^-3 mol of each of the bases. What's the pH of this solution?
16 What is the pH of a 1.63 M solution of pyridine (C5H5N; Kb = 1.7 x 10-9)? [ (4 Puan) 9.72 10.07 9.07 5.23 8.77
1))))Weak Base Titration: At the Equivalence Point a))A 11.30 mL solution of 2.47 M pyridine (C5H5N, a weak base) is titrated to the equivalence point with 22.4 mL of HNO3. What is the pH at the equivalence point? Kb for pyridine is 1.7 X 10-9. b))))Click on all of the dominant species that you would expect to find in solution at the equivalence point. Do not include H3O+ and OH-ions unless they are coming from another source other than the...
Ammonia, NH3, is a weak monoprotic base with Kb = 1.76 × 10−5. Calculate the pH of a 0.00779 M solution of this base. Report your answer to TWO places past the decimal.
If the Kb of a weak base is 5.6 x 10-4, what is the pH of a 0.450 M solution of this base? Give your answer to 2 decimal places
What is the pH of a .62 M [C5H5NH]NO3 solution? Kb(C5H5N) = 1.7 x 10-9 Kb(NH3) = 1.8 x 10-5
Find the pH of a 0.0015 M morphine solution (weak base), Kb= 1.6 x 10−6.