(Multi answers) Find soluble compounds using the solubility rules.TABLE 9.7 Solubility Rules for lonic Compounds in WaterAn ionic compound is soluble in water if it contains one of the following:Li'. Na, K, Rb, Cs, NH₂NO.C₂H₂O₂CI. Br.I except when combined with Ag", Pb, or Hg²+So except when combined with Ba, Pb, Ca, Sr, or Hg²+Ionic compounds that do not contain at least one of these ions are usually insoluble.Positive lonsNegative lonsSelect 5 correct answer(s)CuSKNO3OKCICaSO4Na₂SAgClAgNO3RbBrBaSO4

Answer: Solubility of ionic compounds in water depends upon their lattice energy.

(Multi answers) Find soluble compounds using the solubility rules. TABLE 9.7 Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Li". Na, K, Rb, Cs, NH₂ NO₂, C₂H₂O₂ CI. Br.I except when combined with Ag", Pb, or Hg, SO, except when combined with Ba, Pb, Ca. Sr, or Hg: lonic compounds that do not contain at least one of these ions are usually insoluble. Positive lons Negative lons Select 5 correct answer(s) CuS KNO3 KCI CaSO4 Na₂S AgCl AgNO3 RbBr BaSO4

(Multi answers) Find soluble compounds using the solubility rules. TABLE 9.7 Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Li". Na, K, Rb, Cs, NH₂ NO₂, C₂H₂O₂ CI. Br.I except when combined with Ag", Pb, or Hg, SO, except when combined with Ba, Pb, Ca. Sr, or Hg: lonic compounds that do not contain at least one of these ions are usually insoluble. Positive lons Negative lons Select 5 correct answer(s) CuS KNO3 KCI CaSO4 Na₂S AgCl AgNO3 RbBr BaSO4

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 140QRT

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Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. :math>PbSe. BaCO3 :math>Mg(OH)2f. AlPO4 :math>Na2SO4g. PbCl2 :math>(NH4)2Sh. CaSO4
three solutions are mixed together to form a single solution ; in the final solution, there are 0.2 mol Pb(CH3COO)2, 0.1 mol NA2S and 0.1 mol CACL2 present. which solid(s) will precipitate?
Examine the following solubility rules. Is Fe(OH)3 soluble in water? Salts containing K+, Na+ and NH4+ are soluble. Most salts containing Cl-, S2-, and NO3- are soluble. Most salts containing CrO42-, OH- and CO32- are insoluble So the answer is yes?
When 0.4 mol/L, 350 mL of Pb(NO3)2 is mixed with 0.3 mol/L, 450 mL of KCI, A. will a precipitate form? If so how much is it? B. at the end of the reaction, determine the concentration of all ions presented in the solution.
When HCl(aq) is added to calclum carbonate solid, carbon dioxide gas, liquid water and aqueous calcium chloride form: Caco,(s) + 2HCI(aq) - CO,lg) • CaCl, faq) + H,00) This reaction is used by geologists to confirm the presence of limestone (calcium carbonate) in minerals. In this experiment you are trying to determine the effect of concentration of HCI(aq) on the production of carbon dioxide. a. Based upon the information above, come up with a question to answer. (C:1) You can use the following equipment to answer this question: calcium carbonate chips, 1.90 molL HClaq). pH meter (measures hydrogen ion concentration), beaker, timer, apparatus to measure gas produced b. Based upon the equipment provided above, design a procedure to answer your question. Ensure you provide numbered steps. (1:3, C:2) c. Hypothesize an answer to your question. (I:1) Give reasons for your hypothesis. Ensure you are very specific. (A3) From your experiment, you collect the following data: Reactant…
7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s)  Sr2 (aq)  2F  (aq) 2

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