Liquid ammonia (anhydrous NH3(0)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 = NH4+ + NH2" K = 1x10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.

The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10¬1º. Calculate the pH of a 3.0 M solution of hydrocyanic acid. Round your answer to 1 decimal place. pH = ?

Write the expressions for the acid dissociation constants for the three successive dissociations of phosphoric acid, H3PO4, in water.

Chlorobenzene, C₆H₅Cl, is a key intermediate in the manu-facture of dyes and pesticides. It is made by the chlorination ofbenzene, catalyzed by FeCl₃, in this series of steps:(a) Which of the step(s) is (are) Lewis acid-base reactions?(b) Identify the Lewis acids and bases in each of those steps.(a) Which of the step(s) is (are) Lewis acid-base reactions?(b) Identify the Lewis acids and bases in each of those steps.

Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K=1.8 × 10-4. HCOOH(aq) + H,O(D) — HCOO¯(aq) + H₂O + (aq) Calculate the equilibrium concentration of H3O+ in a 0.985 Msolution. M

Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as antioxidants in soaps. Hydroxylamine has Kb of 9.1 × 10–9. What is the pH of a 0.054 M HONH2 solution? Please report 2 decimal places.

18). The formulas and the structures of two acids are shown below. Which acid is a stronger acid? If the acid strength of the two acids is equal, say so. Cl2CHCOOH CH3COOH но но CI-C-C-OH н-с-с-он ČI Ką = 0.0324 Ką = 1.82 x 10-5 %3D a. Cl¿CHCOOH is a stronger acid than CH;COOH. b. CH;COOH is a stronger acid than CI½CHCOOH c. The two have equal acid strength. d. none of the above

(a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: ethanoic acid (CH3COOH)   ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.   (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak base