Aniline, C6H5NH2 is a weak base important in the dye industry.  It has a Kb= 4.0 x 10-10. What is the pH of a solution containing 0.45 M aniline?

Ammonia, NH3, has a K, of 1.8 x 10. If a solution is prepared in pure water containing an initial concentration of NH3 of 0.20 M, what would be the pH at equilibrium?Select two answers (one for pH and one for % ionization) NH3 (aq) + H2O (1) OH (aq) + NH (aq) Select one or more: O a. pH = 10.26 O b. pH = 11.28 С. pH %3D9.26 O d. % ionization = 0.95% %3D e. % ionization = 0.0090 % %3D Of. % ionization = 2.6 %

A diprotic acid (H₂A) has Kal = 4.54 x 10-7 and K₁2 = 5.59 x 10-¹1. What is the pH of a 0.396 M H₂A solution? pH =

What is the pH of a 0.00105 M  solution of nicotine (C10H14N2)? (Kb1 = 1.0 × 10–6)

What is the pH of a 0.1 M solution of HF? (Hydrofluoric acid K₂ = 7.1 x 10-4)

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Calculate the pH of a solution that has an ammonium chloride concentration of 0.058 M and an ammonia concentration of 0.052 M.  Kb= 1.8 x 10^-5

10a. The Kb of the base B is 1.8 x 10-5. What is the Ka of its conjugate acid, BH^+?  10b. What is the pH of a 1.00 M solution of base B?

A diprotic acid, H₂A, has Ka1 = 3.4 × 10-4 and Ka2 = 6.7 x 10-⁹. What is the pH of a 0.64 M solution of H₂A?

1.00 mL of 0.345 M HCI -Solution A. To this solution you add 123.00 mL of H2O -Solution B. i) Solution A, determine the hydronium (H^ + ) and hydroxide (OH^-) concentrations And the pH and pOH ii) Solution B determine the hydronium (H ^+ ) and hydroxide (OH) concentrations and the pH and pOH