C5H5N (ethylamine) is a weak base. Kb=1.7x10-9. Write an acid dissociation reaction for its conjugate acid. Then, calculate its Ka.
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
A 0.162 molar C5H5N solution has been prepared (Kb= 1.7×10^-9). what is [C5H5N] after equilibrium occurs?
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
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
Pyridine, C5H5N, is a weak base; its conjugate acid has Ka = 6.3 × 10-6. A 0.5-M solution of pyridine has a pH of 9.4. Calculate the concentration of the unreacted pyridine in this solution. [C5H5N(aq)] = M
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.
Design a buffer that has a pH of 9.76 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pKa CH3NH2 4.2 x 10-4 CH3NH3+ 2.4 x 10-11 10.62 C6H15O3N 5.9 x 10-7 C6H15O3NH+ 1.7 x 10-8 7.77 C5H5N 1.5 x 10-9 C5H5NH+ 6.7 x 10-6 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of...
If a base has Kb = 4.09 x 10-8, the value of Ka for the conjugate acid is___________________
Calculate the Kb of the conjugate base of a weak acid with a Ka = 5.28 × 10−5. - report answer in three significant figures - answer should be written in scientific notation (ex. 4.67E-7 or 4.67E7 be sure to use a CAPITAL E not lower case 'e')