For the reaction that occurs when aqueous solutions of Mg(C10:)) and K,S are mixed; which of the following is correct?I. s- is a spectator ionII. KC103 precipitatesIII. MgS precipitatesIV. CIO; is a spectator ion(Solubility Rules are given as below). All salts of ammonium (NH4) and Group I metals (Li, Na, K, Rb, Cs) are soluble in water.. All Chlorides (CIF), Bromides (Br) and Iodides (I) are soluble in water; except those of silver (Ag), mercury) (Hg"), and lead(II) (Pb2).. All Nitrates (NO;), Chlorates (ClO;"), Perchlorates (CIO,) and Acetates (C,H;0,) are soluble in water.· All Sulfates (SO42-) are soluble in water; except those of mercury(I) (Hg"), lead(I) (Pb2) strontium (Sr2*) and barium (Ba2).. All Oxides (O):), Carbonates (CO;2-), Phosphates (PO43-) and Oxalates (C2042-) are insoluble in water; except those of Group I and NH,* aresoluble• All Hydroxides (OH-) and Sulfides (S2-) are insoluble; except those of Group I and NH4* are soluble, calcium (Ca2+) & strontium (Sr2*) areslightly soluble.OA II and IVO B. Iand IIoc l and IVOD. Only IOE Tand III

When two or more than two Aqueous Substances are mixed together , if they form atleast one product…

For the reaction that occurs when aqueous solutions of Mg(C10:2 and K2S are mixed; which of the following is correct? 1. s is a spectator ion II. KCIO; precipitates III. MgS precipitates IV. CIO;" is a spectator ion (Solubility Rules are given as below) · All salts of ammonium (NH4) and Group I metals (Li, Na, K, Rb, Cs) are soluble in water. · All Chlorides (CI"), Bromides (Br) and lodides (1') are soluble in water, except those of silver (Ag), mercury) (Hg"), and lead(I) (Pb"). · All Nitrates (NO;"), Chlorates (CIO;"), Perchlorates (C104") and Acetates (CH302) are soluble in water. · All Sulfates (SO,2) are soluble in water, except those of mercury() (Hg), lead(I) (Po2¬) strontium (Sr2-) and barium (Ba). · All Oxides (02), Carbonates (CO32), Phosphates (PO43) and Oxalates (C20,2) are insoluble in water, except those of Group I and NH,“ are soluble. All Hydroxides (OH") and Sulfīdes (s2-) are insoluble; except those of Group I and NH, are soluble, calcium (Ca") & strontium (Sr²") are slightly soluble. III and IV OA I and II OB. Il and IV OD Only I I and III OE.

For the reaction that occurs when aqueous solutions of Mg(C10:2 and K2S are mixed; which of the following is correct? 1. s is a spectator ion II. KCIO; precipitates III. MgS precipitates IV. CIO;" is a spectator ion (Solubility Rules are given as below) · All salts of ammonium (NH4) and Group I metals (Li, Na, K, Rb, Cs) are soluble in water. · All Chlorides (CI"), Bromides (Br) and lodides (1') are soluble in water, except those of silver (Ag), mercury) (Hg"), and lead(I) (Pb"). · All Nitrates (NO;"), Chlorates (CIO;"), Perchlorates (C104") and Acetates (CH302) are soluble in water. · All Sulfates (SO,2) are soluble in water, except those of mercury() (Hg), lead(I) (Po2¬) strontium (Sr2-) and barium (Ba). · All Oxides (02), Carbonates (CO32), Phosphates (PO43) and Oxalates (C20,2) are insoluble in water, except those of Group I and NH,“ are soluble. All Hydroxides (OH") and Sulfīdes (s2-) are insoluble; except those of Group I and NH, are soluble, calcium (Ca") & strontium (Sr²") are slightly soluble. III and IV OA I and II OB. Il and IV OD Only I I and III OE.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

See similar textbooks

Similar questions

On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are likely to be appreciably soluble in water. Indicate which specific rule(s) led to your conclusion. :math>Ba(NO3)2e. KCl :math>K2SO4f. Hg2Cl2 :math>PbSO4g. (NH4)2CO3 :math>Cu(OH)2h. Cr2S3
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.
On the basis of the general solubility rules given in Table 7.1, predict the identity of the precipitate that forms when aqueous solutions of the following Substances are mixed. If no precipitate is likely, indicate which rules apply. mg src=Images/HTML_99425-7-16ALQ_image001.jpg alt="" align="top"/>
A 300.0-g sample of a solid is made up of a uniform mixture of NaNO3, MgCl2, and BaCl2. A 100.0-g sample of the mixture is dissolved in water and treated with an excess of KOH. The precipitate from the reaction has a mass of 13.47 g. The remaining 200.0-g sample is also dissolved in water and treated with an aqueous solution of AgNO3. The resulting precipitate has a mass of 195.8 g. What are the masses of NaNO3, MgCl2, and BaCl2 in the 300.0-g sample?
In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 123 for definitions.)
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?
On the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.
The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with MnO4 in acidic solution to form V(OH)4+ and manganese(II) ion. The unbalanced titration reaction is MnO4(aq)+VO2++(aq)+H2O(l)V(OH)4+(aq)+Mn2+(aq)+H+(aq) To titrate the solution, 26.45 mL of 0.02250 M MnO4 was required. If the mass percent of vanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.