A 0.162 molar C5H5N solution has been prepared (Kb= 1.7×10^-9). what is [C5H5N] after equilibrium occurs?
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
Consider a solution of 0.31 M C5H5N (Kb = 1.7×10-9). Decide if each of the following is a major or minor species in the solution. Calculate 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
What is Ka for the conjugate acid of C5H5N (Kb = 1.7 x 10 9)? 7 3 LO 89 +/- X 100
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.
30.0 mL of 0.340M C5H5N (Pyridine Kb = 1.7 x 10-9) is titrated with 0.190M HBr (hydrobromic acid). Determine the pH at each of the following points. a. Before any HBr is added b. After 3.00mL of HBr is added c. at half titration d. at equivalence e. After 0.50 mL of HBr added after the equivalence point
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]
Kb = 1.7x10–9 for C5H5N (pyridine). What would be the pH of an aqueous solution containing 0.093 M C5H5N and 0.18 M C5H5NH+?
You have 15.00 mL of a 0.100 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
What is the pH of a buffer made by combining 0.55 mol of C5H5N with 0.86 mol of C5H5NHBr in 100.0 mL of solution? Kb C5H5N = 1.7 x 10-9