Please use the values in the resources listed below instead of the textbook values. Perform the following calkulations involving concentrations of iodate ions (a) The iodate ion concentration of a saturated solution of Ce(103)4 was found to be 7.35X 10 mol/L. Find the Kao (b) Find the concentration (in M) of iodate ions in a saturated solution of Ra(103)2- (Ksp - 1.16X 10)

The equilibrium concentration of sulfide ion in a saturated zinc sulfide solution is M. (Assume that Ksp (ZnS) = 2.0 × 10-25.)

It is determined that the equilibrium concentrations of Fe³+, SCN¯ and [F e SCN²+] are 5.50 x 10-4 M (5.50 times 10 to the minus 4th power M), 7.70 x 10-4 M (7.70 times 10 to the minus 4th power M) and 1.40 x 10-4 M (1.40 times 10 to the minus 4th power M) respectively. What is the value of Kc? No units, please.

What concentration of SO is in equilibrium with Ag,SO0,(s) and 6.90 x 10-3 M Ag+? The Kp of Ag, SO, can be found in this table. [(so = %3D M

When barium fluoride dissolves in water at 25 °C, the equilibrium concentration of Ba2+ is 3.6*10-3 M. Use this information to calculate Ksp for BaF2.

38. The organic compound 18-crown-6 (see preceding prob- lem) also binds strongly with the alkali metal ions in methanol. K* + 18-crown-6#[complex]* In methanol solution the equilibrium constant is 1.41 x 10. A similar reaction with Cst has an equilibrium con- stant of only 2.75 x 104. A solution is made (in methanol) containing 0.020 mol L each of K* and Cs*. It also contains 0.30 mol L' of 18-crown-6. Compute the equi- librium concentrations of both the uncomplexed K* and the uncomplexed Cs*.

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Can you help me calculate Keq from the reaction Cu2+ + 4NH3 = [Cu(NH3)4]2+ knowing that the initial concentration of Cu2+ is 0.0333M and the initial concentration of NH3 is 0.33M. Finally we also know that the final concentration of Cu2+ is 2.6x10^(-10)M.

a) Complete the reaction: Al(OH)3(s) D Al+3 + b) b)Calculate the Ksp for Al(OH)3, which is only slightly soluble in water, if a saturated solution contains [Al+3] = 0.110 M and [OH-1] = 0.330 M. (answer is 3.95 x 10-3)

The Ksp of Pb(OH)2 at 25 °C is 1.4 x 10-15.   What concentration of NaOH will commence precipitation of Pb(OH)2(s) from a solution that contains 0.025 mol L-1 Pb2+(aq) ion?