What is the pH of 0.115 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3 )?.
What is the pH of 0.0750 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)? Express your answer to two decimal places.
What is the pH of 0.0950 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)? Express your answer to two decimal places.
what is the pH of 0.0750 M Fe(NO3)3 (Ka of Fe3+=300x10-3)?
What is the pH of 1.25 M Cu(NO3)2 (Ka = 3.00x10-8)?
Calculate the molarity of Fe3+ in solution A. Solution A: 10 mL of 0.0600 M Fe(No3)3 + 15 mL DI water.
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...
3. (a) Calculate the pH of a solution 0.145 M with respect to CH3CH2COOH and 0.115 M with respect to K+CH3CH2COO-. Ka = 1.3 x 10 – 5 ; pKa = 4.89 (b) Calculate the pH of the same solution after adding 0.015 M KOH. (c) Calculate the pH of the same solution as in part (a) but after addition of 0.015 M HBr.
15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is best explained by the equation: A) NO3-(aq) + H2O(1) + HNO3(aq) + OH(aq) B) Fe3+(aq) + 6 H2O(1) Fe(OH)3(aq) + 3 H30+(aq) C) [Fe(OH2)6]3+(aq) + H20(1) 3 H3O+(aq) + [Fe(OH2)5(OH)]2+(aq) D) H3O+(aq) + OH-(aq) + 2 H2O(1) E) HNO3(aq) + H2O() H30+(aq) + NO3-(aq)
Calculate the pH of a 2.55 M solution of FeCl3. (Fe(H2O)6^3+, Ka=6.3x10^-3)
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C. A student mixes 5.12 mL of 4.02 x 10...