23. What reagent solution might you use to separate the cations in the following mixtures, that is, with one ion appearing in solution and the other in a precipitate? (b) Mg(OH)2(s) and BaSO4(s) (c) PbCO3(s) and CaCO3(s) 24. What reagent solution might you use to separate the cations in each of the following mixtures? Hint: Refer to Exercise 23.] (a) PbSO4(s) and Cu(NO3)2(s)

23. What reagent solution might you use to separate the cations in the following mixtures, that is, with one ion appearing in solution and the other in a precipitate? (b) Mg(OH)2(s) and BaSO4(s) (c) PbCO3(s) and CaCO3(s) 24. What reagent solution might you use to separate the cations in each of the following mixtures? Hint: Refer to Exercise 23.] (a) PbSO4(s) and Cu(NO3)2(s)

General Chemistry - Standalone book (MindTap Course List)

11th Edition

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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

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Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.49QP: The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a...

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Similar questions

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
The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.
0.5 g mixture of (0.1 N KCI and 4 points KBr) is required to 58.03 mL of 0.1 N AGNO3 to precipitate both bromide and chloride as AgCl and AgBr. Calculate the weight percentage for each of the AgCl and AgBr in a mixture if you know that the molecular weight of KCI = 74.5 and of KBr = 119 * %3D
Group I (Ag2+, Pb2+, Hg2+) cations produce insoluble chlorides so they can be precipitated with dilute HCl.
Why is phthalic acid soluble in water and what type of IMFs are involved in the solubility of it in water?
24. What mass of precipitate is formed when 25.00 mL of 0.200 M BaCl2 and 35.00 mL of 0.123 M Na2 SO2 are mixed?
11) When sodium chloride (NaCl) is added to a saturated aqueous solution of silver nitrate (AgNO3), what is the precipitate that would be expected to appear?
2. Will a salt form in an aqueous solution if Na2S is added to a solution containing NH4Cl?3. Can adding sulfate ions to a solution containing Al3+ and Fe2+ be used to identify the components in the mixture?
Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3 (Ksp = 1.36 × 10–7).(b) If the NiCO3 were a contaminant in a sample of CoCO3 (Ksp = 1.0 × 10–12), what mass of CoCO3 would have been lost? Keep in mind that both NiCO3 and CoCO3 dissolve in the same solution.
The chloride in a sample containing approximately 3.5 % NaCl is to be determined gravimetrically as AgCl. What weight of sample must be taken to obtain a precipitate that will weigh about 0.10 g?
instead of dissolving Ag2SO4 (ksp = 7.8x10^-11) in water, you decide to dissolve it in a 2.0x10^-2 mol/L solution of AgNO3. What is it's solubility in this solution?
In which solution will 0.000015 M Pb(NO3)2 form a precipitate? 0.050 M NaF (Ksp of PbF2=3.6x10-8) 0.0040 M Na2SO4 (Ksp of PbSO4=6.3x10-7) 1.0 M NaCl (Ksp of PbCl2=1.7x10-5) 4.0x10-9 M Na2CO3 (Ksp of PbCO3=7.4x10-14

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