For the reaction that occurs when aqueous solutions of NazSO4 and Sr(NO3)2 are mixed; which of the following is corect?I Sr*2 is a spectator ionII. SrSO4 precipitatesIII. NANO3 precipitatesIV. NO3 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 (C1), Bromides (Br) and Iodides (I) are soluble in water; except those of silver (Ag), mercury(1) (Hg"), and lead(II) (Pb²").• All Nitrates (NO;) Chlorates (CIO3"), Perchlorates (CIO4) and Acetates (C2H302") are soluble in water.• All Sulfates (SO42-) are soluble in water;, except those of mercury(1) (Hg"), lead(II) (Pb2+) strontium (Sr2+) and barium (Ba?+).• All Oxides (02), Carbonates (CO;2-), Phosphates (PO43-) and Oxalates (C2042) are insoluble in water; except those of Group I and NH4* aresoluble.All Hydroxides (OH) and Sulfides (S2-) are insoluble; except those of Group I and NH, are soluble, calcium (Ca2+) & strontium (Sr2+) areslightly soluble.II and IVO A.I and IIOB.O. Only IVIII and IVOD.I and IIIOE.

Here , SrSO4 precipitates. Because it is given that all sulphates soluble in water except those of…

I. Sr*2 is a spectator ion II. SrSO4 precipitates III. NANO3 precipitates IV. NO3 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 (C1"), Bromides (Br) and Iodides (Ir) are soluble in water; except those of silver (Ag), mercury(I) (Hg), and lead(II) (Pb-). • All Nitrates (NO3), Chlorates (C1O3"), Perchlorates (C104") and Acetates (C2H302) are soluble in water. • All Sulfates (SO42) are soluble in water; except those of mercury(I) (Hg"), lead(II) (Pb2*) strontium (Sr2*) and barium (Ba2"). • All Oxides (02), Carbonates (CO32-), Phosphates (PO43-) and Oxalates (C2042-) are insoluble in water; except those of Group I and NH4* are soluble. • All Hydroxides (OH") and Sulfides (s2-) are insoluble; except those of Group I and NH,* are soluble, calcium (Ca2") & strontium (Sr2+) are slightly soluble. II and IV A. I and II B. Only IV C. III and IV D. I and III OE.

I. Sr2 is a spectator ion II. SrSO4 precipitates III. NANO3 precipitates IV. NO3 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 (C1"), Bromides (Br) and Iodides (Ir) are soluble in water; except those of silver (Ag), mercury(I) (Hg), and lead(II) (Pb-). • All Nitrates (NO3), Chlorates (C1O3"), Perchlorates (C104") and Acetates (C2H302) are soluble in water. • All Sulfates (SO42) are soluble in water; except those of mercury(I) (Hg"), lead(II) (Pb2) strontium (Sr2) and barium (Ba2"). • All Oxides (02), Carbonates (CO32-), Phosphates (PO43-) and Oxalates (C2042-) are insoluble in water; except those of Group I and NH4 are soluble. • All Hydroxides (OH") and Sulfides (s2-) are insoluble; except those of Group I and NH,* are soluble, calcium (Ca2") & strontium (Sr2+) are slightly soluble. II and IV A. I and II B. Only IV C. III and IV D. 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

Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
On the basis of the general solubility rules given in Table 6-1, predict which of the following substances are likely to be soluble in water. a. aluminum nitrate b. magnesium chloride c. rubidium sulfate d. nickel(II) hydroxide e. lead(II) sulfide f. magnesium hydroxide g. iron(III) phosphate
It is stated in Section 6.3 of the text that to balance equations by inspection you start “with the most complicated molecule.” What does this mean? Why is it best to do this?
Potatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?
3.106 Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.
Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. copper(II)sulfate(aq)+iron(s)copper(s)+iron(II)sulfate(aq)copper(II)sulfate(aq)+iron(s)copper(s)+iron(III)sulfate(aq) You place 87.7 mL of a 0.500-M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.
A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?
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.)
Determine the volume of sulfuric acid solution needed to prepare 37.4 g of aluminum sulfate, Al2(SO4)3, by the reaction 2Al(s)+3H2SO4(aq)Al2(SO4)3(aq)+3H2(g) The sulfuric acid solution, whose density is 1.104 g/mL, contains 15.0% H2SO4 by mass.
onsider separate aqueous solutions of HCI and H2S04 with the same concentrations in terms of molarity. You wish to neutralize au aqueous solution of’ NaOH. For which acid solution would you need to add more volume (in mL) to neutralize the base? The HCI solution. The H2SO4 solution. You need to know the acid concentrations to answer this question. You need to know the volume and concentration of’ the NaOH solution to answer this question. c and d plain your answer.