CrO2, Zn(NH3)4²+ (10) | BaCl, BaCrO4 Zn(NH3)42 In step 10 of the "GREEN" flow chart BaCl₂ is added to the colorless solution resulting in a clear colorless solution with no solid. The observations thus far likely indicate... 2+ Select the best answer for each element. (Hint choose one answer from the 1st set of three boxes and one answer from the 2nd set of three boxes.) The element Cr is present in the original sample The element Cr is absent in the original sample It is inconclusive whether Cr is present in the original sample The element Zn is present in the original sample The element Zn is absent in the original sample It is inconclusive whether Zn is present in the original sample

CrO2, Zn(NH3)4²+ (10) | BaCl, BaCrO4 Zn(NH3)42 In step 10 of the "GREEN" flow chart BaCl₂ is added to the colorless solution resulting in a clear colorless solution with no solid. The observations thus far likely indicate... 2+ Select the best answer for each element. (Hint choose one answer from the 1st set of three boxes and one answer from the 2nd set of three boxes.) The element Cr is present in the original sample The element Cr is absent in the original sample It is inconclusive whether Cr is present in the original sample The element Zn is present in the original sample The element Zn is absent in the original sample It is inconclusive whether Zn is present in the original sample

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...

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
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
32). Determine the molar solubility of Cu(IO4)2 in 0.20 M NaIO4? ((Ksp of Cu(IO4)2 = 1.4 x 10−7) (a) Show the reaction of dissociation of Cu(IO4)2. (b) Draw and fill the ICE table. (c) Show the Ksp expression for Cu(IO4)2. (d) Calculate the molar solubility of Cu(IO4)2 in 0.20 M NaIO4.
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
(b) 13. Calculate the Ni+2 concentration of a solution made by mixing 0.020 mole of solid Ni(NO3)2 into 1.0 liter of 0.22 M NH4OH. Kd for NI(NH3)²+ = 1.1 x 10-8. N ) ₁) (NO3)₂ + 4) O
You look at the solubility of Ca(OH)2 in water (Ksp = 4 x 10–10). You wait until the system reaches equilibrium and then add Cr(C2H3O2)3. (Ksp = 6.7 x 10–31 for Cr(OH)3). Would affect do you think would occur to the solubility? (increase, decrease, stay the same) Show this through a calculation (Note: Two equilibria must be considered).
Q2: Use activities to calculate the molar solubility of Zn(OH)2 in (Ksp 3*10-16) (a) 0.0100 M KCl. (b) 0.0330 M K2SO4.
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)
At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?
What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mg
Lead (II) bromide, PbBr2, has Ksp= 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+and Br–at equilibrium.)
The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce3+ concentration in asolution prepared by mixing 50.0 mL of 0.0250 M Ce3+ with 50.00 mL of

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