Calculate the pH and the equilibrium concentrations of HC2O4- and C2O42- in a 0.1160 M oxalic acid solution, H2C2O4 (aq). For H2C2O4, Ka1 = 5.9×10-2 and Ka2 = 6.4×10-5
pH =
[HC2O4-] = M
[C2O42-] = M
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Calculate the pH and the equilibrium concentrations of HC2O4- and C2O42- in a 0.1160 M oxalic...
Calculate the pH and the equilibrium concentrations of HC2O4- and C2O42- in a 0.0782 M oxalic acid solution, H2C2O4 (aq). For H2C2O4, Ka1 = 5.9×10-2 and Ka2 = 6.4×10-5 pH =_______ [HC2O4-] =___________ M [C2O42-] =___________ M
Oxalic acid (HOOC-COOH) is a simple diprotic acid. It is used commercially in bleaching straw and leather and removing rust and ink stains. a. Write each dissociation step for the acid including the K values from appendix C. b. What are the equilibrium concentrations of [H2C2O4], [HC2O4- ], and [C2O42- ] in a 0.150M H2C2O4 solution. (Hint: the concentrations of [H2C2O4], [HC2O4- ] are found together and used to find concentration of [C2O42- ].) c. What is the pH of...
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
calculate the pH and pOH for a 0.15 M oxalic acid H2C2O4 solution. (ka1-6.0x10^-2, Ka2-6.1x10^-5)
The pH of a 0.20-M solution of oxalic acid (H2C2O4) is measured to be 1.10. Use this information to determine a value of Ka for oxalic acid. H2C2O4(aq) + H2O(l) HC2O4-(aq) + H3O+(aq) Ka =
Calculate the pH of 1.00 x 10^-2 M oxalic acid solution. Calculate the pH of 1 x 10^-2 M solution of sodium oxalate. Ka1 = 5.62 x 10^-2, Ka2 = 5.42 x 10^-5
Calculate the pH and the equilibrium concentrations of H2C6H5O7-, HC6H5O72- and C6H5O73- in a 0.1840 M aqueous citric acid solution. For H3C6H5O7, Ka1 = 7.4×10-3, Ka2 = 1.7×10-5, and Ka3 = 4.0×10-7 pH = [H2C6H5O7-] = __M [HC6H5O72-] =__ M [C6H5O73-] = __M
A titration is carried out for 20.0mL of 0.10 M Oxalic Acid (weak acid) with 0.10 M of a strong base NaOH. Calculate the pH at these volumes of added base solution: (a) 0.0 mL (b) 5.0 mL (c) 10.0 mL (d) 15.0 mL (e) 20.0 mL (f) 25.0 mL (g) 30.0 mL Oxalic acid Ka1 = 5.9 x 10-2 Ka2 = 6.4 x 10-5
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2620 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2380 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M