When aqueous solutions of AgNO3 and NaCl are mixed together, the precipitate that will form is Solubility of KCI at 20 oC is 34 g/100 g H20. A solution containing 20 g of KCI in 50 g of water at 20 oC is classified as NH3 will dissolve in water because NH3 is a solute. CCI4 is insoluble in water because water is a

When aqueous solutions of AgNO3 and NaCl are mixed together, the precipitate that will form is Solubility of KCI at 20 oC is 34 g/100 g H20. A solution containing 20 g of KCI in 50 g of water at 20 oC is classified as NH3 will dissolve in water because NH3 is a solute. CCI4 is insoluble in water because water is a

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Solid sodium hydroxide is slowly added to 175 mL of a 0.198 M magnesium bromide solution until the concentration of hydroxide ion is 0.0571 M. The percent of magnesium ion remaining in solution is| 1%. Solid ammonium carbonate is slowly added to 50.0 ml of a 0.118 M barium nitrate solution until the concentration of carbonate ion is 0.0440 M. The mass of barium ion remaining in solution is grams.
A sample contains MgCl2 (95.211 g/mol) and KCl (74.551 g/mol). A 6.6933-g sample was dissolved in enough H2O to make 250.0-mL solution. A 50.00-mL aliquot was treated with AgNO3 to precipitate the chlorides and after proper collection and drying gave a precipitate weighing 1.9620-g. Another 50.00-mL aliquot was tested for its Mg2+ content by precipitating it with NH4+ and PO43- giving an Mg2P2O7 (222.551 g/mol) precipitate weighing 0.5186 g with FW AgCl 143.32 g/mol. What is percent KCl in the sample?
Sample Mass of Original Mixture (g) Mass of Watch Glass (g) Mass of Filter Paper (g) Mass of Watch Glass, Filter Paper, and Precipitate (g) Avery 2.023 31.997 0.220 32.949 Zachariah 1.992 27.391 0.198 28.164 Sample Results from addition of ZnSO4 to supernatant (Beaker 1) Results from addition of Na3PO4 to supernatant (Beaker 2) Avery No change Precipitate forms Zachariah Precipitate forms No change 3 ZnSO4(aq) + 2 Na3PO4(aq) Zn3(PO4)2(s) + 3 Na2SO4 What was the mass, in grams, of the limiting reactant in the original mixture for Avery’s experiment?
30.0 mL of 0.322 M potassium iodide are combined with 20.0 mL of 0.530 M lead (II) nitrate. How many grams of lead (II) iodide will precipitate? Pbla 2KNO) + 2Ka Pb(NO,) O a 2.23 g 4.90 g 8.90 g 4.45 g
Suppose you are asked to determine the identity of a white solid. When you add water to the white solid, it dissolves and forms a clear solution. When you add a solution of Na, SO,, a white precipitate forms. Add Add H,O Na,SO, Determine the identity of the original solid. O PBCI, O MgCl, O ZNCI, O CaCl,
Give detailed Solution with explanation needed
4. Using the solublity chart we can see that compound is soluble KNO3 PBCI Ca(OH)2 Agl
! A solid mixture containing MgSO4 is dissolved in water and treated with an excess of Ba(NO3)2, resulting in the precipitation of 0.6 g of BaSO4.The molecular weight of BaSO4 is 233 g/mol. Number of moles of MgSO4 in the mixture is? 0.02570 mol 0.00257mol 0.05720 mol 0.52700 mol 0.25700 mol If the concentration of chloride ion is 1.5xE(-5) then the solubility product of AgCl is--- 2.00x10(-10) 1.69x10(-10) 1.96x10(-10) 0.69x10(-10) 19. x 610(-10)
Solid potassium sulfite is slowly added to 75.0 mL of a 0.0373 M barium nitrate solution. The concentration of sulfite ion required to just initiate precipitation is M.
Which of the following will occur when an aqueous solution of KBr is mixed with an aqueous solution of AGNO3? No precipitate will form. OA Aprecipitate of KNO3 will form. OB Oc A precipitate of AgBr will form. OD A precipitate of AgNo3 will form. DE Bright yellow precipitate will form.
Cis soluble in water and in nitric acid HNO3. It does not give a precipitate with Ba(NO3)2 solution but gives a precipitate with AgNO3 solution and the precipitate is not soluble in any strong acid. When solid C is heated, white smoke is observed. C SOLUBILITY RULES Solubilities of ionic substances in water: 1) All salts of Na*, K*, NH4+ are soluble in water. 2) All salts of NO;, CH;CO0- (C2H302) are soluble in water. 3) All salts of Clr, Br, I are soluble in water (except Agt, Pb2-, Hg,2+) 4) All salts of SO,2- are soluble in water ( except Ba2+, Pb2-, Sr2+) so,2- of Ca2+, Ag*, Hg22- are slightly soluble in water. 5) All salts of CO;2, PO- are insoluble in water (except Na*, K*, NH4*) 6) All salts of S2- are insoluble in water ( except Na*, K*, NH, Ba2+ Ca2+, Mg2+, Sr2-) 7) All salts of 02-, OH- are insoluble in water ( except Na", K*, NH4*, (Ba2-)) OH of Ca2+, Sr2-, (Ba2+) are slightly soluble in water OH of Mg?- is very very slightly soluble water STRONG ACIDS STRONG BASES HCI LIOH…
1. Reaction Add 1 drops of … Add 1 drops of… Did a precipitate form? 1 Fe(NO3)3 Na3PO4 2 AgNO3 3 Zn(NO3)2 4 Al(NO3)3 5 Pb(NO3)2