The ionization constant for NH4+ is K = 5.8 x 10-10 at 25°C. It is in a reversible equilibrium with ammonia and H+. NH4+ --> NH3 + H+ where, H+ + NH3 --> NH4* with a k₁ = 4.000 x 1010 M-1 S-1 A temperature jump from 20°C to 25°C is made on a 0.1 M NH4Cl solution at pH 6. Calculate the relaxation time in microseconds for the reaction, assuming that the mechanism is given by the ionization equation shown. Assume that the pH is buffered.

2. Determine [H3O+] and [OH] concentrations (in M to two decimal places) for each: (a) Pure water at 10 °C (K = 0.293 x 10-14) W (b) An aqueous solution with a pH of 3.23 A: 5.41x108; 5.41×10-8 A: 5.89x104; 1.70×10-11

Use the 5% rule to determine whether or not the equilibrium concentration of the acid can be approximated by its makeup concentration. (a) 0.49 M cyanic acid (HCNO, PKa = 3.46) 0.02 * % O The approximation is valid. O The approximation is not valid. (b) 0.0014 M hydrazoic acid (HN3, PK₂ = 4.6) % O The approximation is valid. O The approximation is not valid. (c) 5.7 M arsenic acid (H3ASO4, Pka = 2.26) % O The approximation is valid. O The approximation is not valid.

Salts containing the phosphate ion are added to municipalwater supplies to prevent the corrosion of lead pipes. (a) Basedon the pKa values for phosphoric acid (pKa1 = 7.5 x 10 - 3,pKa2 = 6.2 x 10 - 8, pKa3 = 4.2 x 10 - 13) what is the Kbvalue for the PO43 - ion? (b) What is the pH of a 1 x 10 -3 M solution of Na3PO4 (you can ignore the formation ofH2PO4- and H3PO4)?

7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- (ct = Cha + cx-) pH (A"] Acid (HA] Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 0.145 0.221 Hydrogen cyanide Sulfamic 0.250 1.20

Calculate Ka from Equilibrium Concentrations At equilibrium a solution contains [HC2H3O2] = 0.0787 M and [H3O+] = [C2H3O2-] = 0.00118 M.

α A solution is prepared at 25 °C that is initially 0.90M in chloroacetic acid (HCH2CICO2), a weak acid with K = 1.3 × 10¯ chloroacetate (KCH2 CICO2). Calculate the pH of the solution. Round your answer to 2 decimal places. and 0.75M in potassium pH = ☐ ☑ o0o 18 Ar hers ne, and...

(c) Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3, is 4.3 x 10-7. Нансез END

The acid-dissociation constant for chlorous acid (HClO2) is1.1 x 10-2. Calculate the concentrations of H3O+, ClO2-,and HClO2 at equilibrium if the initial concentration ofHClO2 is 0.0125 M.

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