What is the pH of a 0.30 M pyridine solution that has a Kb 1.9 x 10 2 The equation for the dissociation of pyridine is C 5H 5N( aq) + H 20() C5H 5NH *(aq) + OH "(aq). 9.38 10.38 8.72 4.62

Calculate the pH of a solution containing 0.45 M HCN(aq) and 0.65 M NaCN. The Ka of HCN(aq) is 4.9 × 10–10.

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

The strongest known acid is fluoroantimonic acid, [H₂F][SbF6]. It is 1016 times more acidic than concentrated sulfuric acid and has a pH of -31.3; it is strong enough to protonate both xenon and molecular hydrogen. It is an ionic liquid made by reacting hydrogen fluoride with antimony(V) fluoride: 2 HF + SbF5 → H₂F+ + SbF6 Explain why this acid is so strong.

What is the pH of a 0.652 M solution of hydroxylammonium, a weak acid with a K, of 1.1 x 10-6? Oa. 0.19 Ob. 3.07 Ос. 7.2 х 10-7 Od. 5.96 Oe. 6.14

Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M HCl(aq) solution. Calculate the pH at 10.0 mL intervals of added HCl(aq), up to 50.0 mL, and plot the titration curve. Assume that the volumes are additive. Use pKb = 3.34 for methylamine.

Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (a) Write out the reaction that leads to this acidic pH.

Calculate the pH of a solution that is 3.67×10−53.67×10-5 M NH3 and 2.41×10−52.41×10-5 M NH4Cl.Kb=1.821.82 x 10−510-5NH4+1 (aq) + H2O(l) <----> NH3(aq) + H3O+1(aq)

Codeine,C18H21NO3 is an alkaloid (Kb=6.2 * 10^-9) a painkiller and a cough suppressant. its solution is acidified with hydrochloric acid to pH=4.50. what is the ratio of the conjugate acid to codeine to that of codeine? (use Handerssen Hasalbalch equation).

A solution is prepared at 25 °C that is initially 0.27M in chlorous acid (HCI0,), 2 a weak acid with K,=1.1 × 10 and 0.29M in potassium chlorite (KCIO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = U ? olo Ar