Ephedrine is a weak base. A 0.035 M solution of ephedrine has a pH of 11.33. What is the base ionization constant (Kb) for ephedrine?
() 7.8 x 10-10
() 1.5 x 10-9
() 9.8 x 10-5
() 1.4 x 10-4
Ephedrine is a weak base. A 0.035 M solution of ephedrine has a pH of 11.33....
A 0.200 M solution of a weak base has a pH of 9.95 . What is the base hydrolysis constant, Kb, for the weak base?
A solution of ephedrine has a pH of 11.8. What is its initial concentration and the percent ionization? Kb=1.4x10^-4. Ephedrine = C10H15ON
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]
A 0.314 M solution of a weak base has a pH of 10.70. What is the base hydrolysis constant, K, for the weak base? Kb =
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
6. A 0.200 M solution of a weak base in water has a pH = 10.40. Calculate the value of K, for this base a 1.0 x 10 b. 3.2 x 10 c. 2.2 x 10 d. 4.0 x 1011 e. 5.0 x 10 7. The ionization constant, K, for dichloroacetic acid, HC,HO_Cl, is 5.0 x 10? What is the pH of a 0.15 molar solution of this acid? a. 1.06 b. 1.19 c. 1.30 d. 1.56 e. 1.82
Butylamine, , is a weak base. A 0.77 M aqueous solution of butylamine has a pH of 12.20. What is Kb for butylamine? Calculate the pH of a 0.88 M aqueous solution of butylamine. Kb? pH?
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....
A weak base has a base hydrolysis constant, Kb, of 2.5 x 10-6. What is the pH of a 0.15 M solution of the weak base? pH =