|||O SIMPLE REACTIONSPredicting precipitationComplete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empiricalformula in the last column.solution Asodium sulfidepotassium hydroxidesodium acetateExplanationChecksolution Bzinc sulfateiron(II) nitratebarium bromideDoes aprecipitate formwhen A and Bare mixed?ⒸyesⒸyesyesnononoempiricalformula ofprecipitate0090₁Ś2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessiDELL

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||| = O SIMPLE REACTIONS Predicting precipitation Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A sodium sulfide potassium hydroxide sodium acetate solution B zinc sulfate iron(II) nitrate barium bromide Does a precipitate form when A and B are mixed? O yes no O yes no O yes no empirical formula of precipitate 0 0 X 2/5 Do

||| = O SIMPLE REACTIONS Predicting precipitation Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A sodium sulfide potassium hydroxide sodium acetate solution B zinc sulfate iron(II) nitrate barium bromide Does a precipitate form when A and B are mixed? O yes no O yes no O yes no empirical formula of precipitate 0 0 X 2/5 Do

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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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?
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Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A solution B Does a precipitate form when A and B are mixed? empirical formula of precipitate sodium chloride ammonium bromide yes no sodium iodide lead(II) nitrate yes no potassium sulfide iron(II) bromide yes no
Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. icrosoft O W W Microsoft Microsoft 6.52.210... esc solution A magnesium sulfate manganese(II) chloride potassium chloride Explanation ! < 8 2 solution B sodium hydroxide cadmium sulfate 9,214 barium bromide Check 280 3 Q Does a precipitate form when A and B are mixed? 103 O yes O yes NOV 1 yes 4 no no no % 5 empirical formula of precipitate ● 0 0 0 atv Google 6 3 09 & 7 X 2 00 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 9 Ś * 8 7 A nt ( 9 ) W 0 30 -DOCX + 11 - olo Ar 18 2 h E
Predicting precipitation Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A sodium hydroxide manganese(II) chloride potassium sulfide solution B zinc nitrate cadmium nitrate copper(II) sulfate Does a precipitate form when A and B are mixed? yes yes yes no no no empirical formula of precipitate П 0 X Ś
The solubility rules listed in table below. General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C. 1. Most nitrate (NO3¯) salts are soluble. 2. Most salts of Na+, K+, and NH4+ are soluble. 3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂. 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4. 5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH and KOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble. 6. Most sulfide (S²-), carbonate (CO3²), and phosphate (PO4³-) salts are only slightly soluble.* *The terms insoluble and slightly soluble really mean the same thing: such a tiny amount dissolves that it is not possible to detect it with the naked eye. a on the basis of the general solubility rules, which choice explains why sodium sulfide would be expected to be appreciably soluble in water. Most sulfide (S²-) salts are only slightly soluble. 2- Most salts of Na+ are…
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