The Ksp of La(OH) 3 is 2.0x10-21 When activities are considered, what is the concentration of La3+ in a saturated solution with an ionic strength of 0.054 M? .3+ (aq) La(OH)3 (s) = La²) + 3OH(aq KS = 2.0x10-21 sp For La³+ with a charge of +3 and a hydrated radius of 900 pm, the activity coefficient from the extended Debye Hückle equation is 0.233 when the ionic strength is 0.054 M. For OH with a charge of -1 and a hydrated radius of 350 pm, the activity coefficient from the extended Debye Hückle equation is 0.806 when the ionic strength is 0.054 M. Answer using scientific notation with 3 significant digits. For example typing "3.14E-6 M"

The Ksp of La(OH) 3 is 2.0x10-21 When activities are considered, what is the concentration of La3+ in a saturated solution with an ionic strength of 0.054 M? .3+ (aq) La(OH)3 (s) = La²) + 3OH(aq KS = 2.0x10-21 sp For La³+ with a charge of +3 and a hydrated radius of 900 pm, the activity coefficient from the extended Debye Hückle equation is 0.233 when the ionic strength is 0.054 M. For OH with a charge of -1 and a hydrated radius of 350 pm, the activity coefficient from the extended Debye Hückle equation is 0.806 when the ionic strength is 0.054 M. Answer using scientific notation with 3 significant digits. For example typing "3.14E-6 M"

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 16E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...

See similar textbooks

Similar questions

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995
At 25 °C, for Lead (II) sulphate (PbSO4), Ksp = 2.53×10-8 and for Barium sulphate (BaSO4) Ksp = 1.08×10-10. Suppose that Na2SO4 is added gradually to 500 mL of a solution that contains both Pb2+ ion and Ba2+ ion. (i) What will the Ba2+ concentration be (in mol/l) when Pb just begins to precipitate if the initial solution contains 0.40 M Pb2+ and 0.52 M Ba2+? (ii) What percentage of the strontium ion has precipitated when PbSO4 just begins to precipitate if the initial solution contains 0.28 M Pb2+ and 0.32 M Ba2+?
Calculate the solubility of La(IO3)3 in a 0.03 M solution of Mg(ClO4)2 using (a) activities and (b) molar concentrations when its Ksp is 1.0x10^-11
Please use the values in the resources listed below instead of the textbook values. Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a saturated solution of Ce(IO3)4 was found to be 7.35X10 mol/L. Find the Ksp: 4.0 (b) Find the concentration (in M) of iodate ions in a saturated solution of Ra(IO3)2. (Ksp = 1.16X 10-9) 4.0) M
a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksp. = 1.4 x 107 at 25 °C %3D b) Will the solubility of Cu(IO3)2 (s) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (a0), react with aqueous ammonia to form a complex according Cu2+, (a0+ 4NH3 (a) [Cu(NH3)4]* (aq) with a formation constant, Ke= 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)
Chemistry (Part -4) =============
The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molar solubility of Mg3(AsO4)2 in water.
19" 0.00014 m Na2 Coz are combined? Determine the solubility of Cul (s) (Ksp.= 1.1x1013 In 0.15m Cu₂ (03 (aq) Solution,
Calculate the solubility of FeCO3 (in mol/L) in the following. Assume the Ksp of FeCO3 = 3.5 x 10-1". (a) water mol/L (b) 0.0415 M Fe(NO3), ] mol/L (с) 0.0415 М K,СОз mol/L
Given the equilibria below, determine the mass of AgBr that will dissolve in 200 mL of 0.100 M NaCN. AgBr(s) Ag*(aq) +Br (aq) Ksp = 5.0 x 10-13 Ag"(aq) + 2 CN (aq) Ag(CN)2 (aq) Kr= 1.3 x 1021
7. The Ksp for copper(I) sulfide, Cu2S(s), is 2.5 x 10-48. Cu2S (s) 2 Cu'(aq) + S²(aq) (a) Write a solubility constant expression for Cu2S(s). [2] (b) Calculate its molar solubility in water at 25 degrees Celsius. [6]
Q2) Q1) what is the concentration of Sr2* in PPm for the solution in equilibrium with the precipitate of SrSO4 ? PKSP(SrOa) =6.55 PKa( HSO4) 1.92 Mw(Sr)=87.6