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).
What is the pH of a 0.148 M solution of sulfurous acid? (Ka1 = 1.7 x...
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 0.200 M solution of sulfurous acid? Given: Ka1 = 1.70×10–2, Ka2 = 6.20×10–8
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
What is the pH of a 1.48M solution of citric acid? Ka1 = 7.4 x 10-4 Ka2 = 1.7 x 10-5 Ka3 = 4.0 x 10-7
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...
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?
The acid-dissociation constants of sulfurous acid (H2SO3) are Ka1= 1.7 x 10^-2 and Ka2 = 6.4 x 10^-8 at 25 degrees celcius. Calculate the pH of a 0.163 M aqueoussolution of sulfurous acid.
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
What is the equilibrium pH of a 0.515 M solution of H3PO4 (aq)? (Ka1 = 7.5 × 10–3 , Ka2 = 6.2 × 10–8 , Ka3 = 4.8 × 10–13) a. 1.23 b. 3.75 c. 12.32 d. 6.30 e. 7.21