Although KOH, R6OH, and CSOH have little association between metal and hydroxide in aqueous solution, Lit and Na+do form complexes with OH :[LIOH(aq)]Lit + OH- = LIOH(aq)K1[Li* ][OH¯]= 0.83[NAOH(aq)]Na+ + OH = NaOH(aq)K1 =[Na+ ][OH ]= 0.20Prepare a table showing initial and final concentrations of Lit, OH, and LIOH(aq) in 1.00 F LIOH solution. Calculatethe fraction of lithium in the form LİOH(aq) at equilibrium.fraction as LIOH(aq):

Although KOH, RÜOH, and CSOH have little association between metal and hydroxide in aqueous solution, Lit and Na+ do form complexes with OH: [LİOH(aq)] Lit + OH- 2 LİOH(aq) K = = 0.83 [Li* ][OH¯] [NAOH(aq)] Na+ + OH- = NAOH(aq) K = [Na+][OH¯] = 0.20 Prepare a table showing initial and final concentrations of Lit, OH , and LIOH(aq) in 1.00 F LIOH solution. Calculate the fraction of lithium in the form LIOH(aq) at equilibrium.

Although KOH, RÜOH, and CSOH have little association between metal and hydroxide in aqueous solution, Lit and Na+ do form complexes with OH: [LİOH(aq)] Lit + OH- 2 LİOH(aq) K = = 0.83 [Li* ][OH¯] [NAOH(aq)] Na+ + OH- = NAOH(aq) K = [Na+][OH¯] = 0.20 Prepare a table showing initial and final concentrations of Lit, OH , and LIOH(aq) in 1.00 F LIOH solution. Calculate the fraction of lithium in the form LIOH(aq) at equilibrium.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the insoluble compound cobalt(II) carbonate, CoCO3. The cobalt(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)2+, K = 7.7x104. Be sure to specify states such as (aq) or (s). K= Submit Answer Retry Entire Group 3 more group attempts remaining
Write the chemical equation for the disproportionation of Cr(OH)3Cr(OH)3 in basic solution. Chromium(III) hydroxide and chromium(II) hydroxide are poorly soluble salts.
Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) in presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42, K₁= 2.9x1015. Be sure to specify states such as (aq) or (s). K=
Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the equilibrium constant for the following reaction: Ni2+(aq) + NH4+(aq) --> [Ni(H2O)5(NH3)]2+ + H+(aq) In a solution of 0.010 M Ni2+ and 0.010 M NH4+, will this reaction favor products or reactants at pH=1? pH=7? pH=12? how do you find the concentration of [Ni(H2O)5(NH3)]2+?
determine the equilibrium constant Keq if the concentration of iron(III) thiocynate is 0.322 M and the concentration of the thicyante ion is 0.013 M and the concentration of iron is 0.13 M.
bot 3. Iron(II) ion (Fe°*) reacts with thiocyanate ion (SCN¯) to form a red complex ion with the formula [FESCN]2+. The net ionic equation describing this reaction is given in Equation 10. eH MC () Fe+ (aq, It. yellow) + SCN (aq, colorless)=[FESCN]²+ (aq, red) 12+ (Eq. 10) A student studying this equilibrium begins with an equilibrium mixture that is light pink. (1) What change will the student observe when a solution containing Fe³+ ion is added to this mixture?
The metal ion M2+ in ammonia, NH3 forms the complex ion M(NH3)62+ (Kf = 5.1x108). Calculate the M2+ concentration when the equilibrium concentrations of NH3 and M(NH3)62+ are 0.046 and 0.15 M respectively.
In the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+. Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+ + 3H2O ↔ [Al(H2O)3(OH)3]2+ + 3H3O+
Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH", the Al³+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.20x10-2 mol AI(CH3COO) 3(S) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.90). For Al(OH)4, Kf = 1.1x1033. [A1³+] = Check & Submit Answer Show Approach M
7.00 grams of Cobalt (II) nitrate are dissolved in 1.00 liter of water. What is the initial concentration of CO (2+) in moles per liter? Then, 0.22 moles of solid KOH are added to this solution. The solution volume remains 1.00 liter. Given that Kf = 5.0 x 10^9 for the complex ion, Co(OH)4 (2-) find the final concentrations of Co (2+), Co(OH)4 (2-), and OH-. Also find the pH of this final solution.
Calculate the equilibrium concentration of Ni2+ in a 1.0-M solution [Ni(NH3)6](NO3)2.
Consider the insoluble compound nickel (II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³¹ . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group No more group attempts remain