What is the pH of a 0.200 M solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8
What is the pH of a 0.200 M solution of sulfurous acid? Given: Ka1 = 1.70×10–2,...
What is the pH of a 0.180 M solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8
What is the pH of a 0.148 M solution of sulfurous acid? (Ka1 = 1.7 x 10-2 and Ka2 = 6.2 x 10-8).
Calculate the pH and the equilibrium concentrations of HSO3- and SO32- in a 0.1770 M sulfurous acid solution, H2SO3 (aq). For H2SO3, Ka1 = 1.7×10-2 and Ka2 = 6.4×10-8 pH = [HSO3-] = _______ M [SO32-] = ______ M
Consider a the titration of 2.5 M sulfurous acid (H2SO3, Ka1 = 1.5e-2, Ka2 = 1.0e-7) with 2.0 M NaOH. What is the pH at the first halfway point of the titration? What is the pH at the second halfway point of the titration? What is the pH at the equivalence point of the titration?
In the titration of 50.0 ml of 0.200 M Sulfurous Acid (H2SO3) with 0.120 M LiOH and given the information below, answer the following questions. 1. Ka,-1.7 x 10-2 Ka2- 6.4x 10-8 SO32- H+(aq) ← → HISO3_ (ag) + (ag) What is the initial pH of the analyte (sulfurous acid)? a. or What is the pH at the first equivalence point of the titration? b. What is the pH at the first half-way point of the titration? c. What volume...
a)What is the percent ionization of a 0.493 M aqueous solution of hydrosulfuric acid? Ka1 = 9.5x10-8; Ka2 = 1x10-19 b)What is the pH of a 0.400 M aqueous solution of NaCH3COO? Ka (CH3COOH) = 1.8x10-5 c)What is the pH of a 0.437 M aqueous solution of NaHCO3? Ka1 (H2CO3) = 4.2x10-7 Ka2 (H2CO3) = 4.8x10-11 d)What is the pH of an aqueous solution made by combining 14.04 mL of a 0.1614 M hydrochloric acid with 35.78 mL of a...
a)What is the percent ionization of a 0.493 M aqueous solution of hydrosulfuric acid? Ka1 = 9.5x10-8; Ka2 = 1x10-19 b)What is the pH of a 0.400 M aqueous solution of NaCH3COO? Ka (CH3COOH) = 1.8x10-5 c)What is the pH of a 0.437 M aqueous solution of NaHCO3? Ka1 (H2CO3) = 4.2x10-7 Ka2 (H2CO3) = 4.8x10-11 d)What is the pH of an aqueous solution made by combining 14.04 mL of a 0.1614 M hydrochloric acid with 35.78 mL of a...
Sulfurous acid (H2SO3) is a diprotic acid, (Ka1 - 17 10-2 and Ka2 - 6,0 x 10-8 what is the equilibrium concentration of SO3? if the initial concentration of H2SO3 is 1.2 M? O 6.0 x 10-8 M O2.0 x 10-2 M O 1.7 x 10-8 M O 17 x 10-2M 7.2 x 10-8 Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4l(s) = NH3(g) + HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at...
What is the pH of a 0.010-M solution of phthalic acid, C6H4(CO2H)2? (Ka1 = 1.29 x 10-3 and Ka2 = 3.01 x 10‑9) Please write everything out if possible, I'm pretty confused on these problems so any help would be nice.
What is the pH of a 1.13M solution of ascorbic acid? Ka1 = 8.0 x 10-5 Ka2 = 1.6 x 10-12