Eroup I metals, ammonium, acetate, and nitrate always form water soluble salts Chlorides generally form water soluble salts with the exception of Ag", Pb* and Hg, Based on the solubility information, finish the following equations by predicting products. Including (s) for any insoluble salt formed and (aq) for water soluble salts. 1. NaCl(aq) + AgNO3(aq) → 2. CaCl2(aq) + NH,NO3(aq) →

Eroup I metals, ammonium, acetate, and nitrate always form water soluble salts Chlorides generally form water soluble salts with the exception of Ag", Pb* and Hg, Based on the solubility information, finish the following equations by predicting products. Including (s) for any insoluble salt formed and (aq) for water soluble salts. 1. NaCl(aq) + AgNO3(aq) → 2. CaCl2(aq) + NH,NO3(aq) →

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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For the reaction Ba(OH)2 (aq) + (NH4)½CO3 (aq)--> What one of the following species would appear in the molecular equation? (Don't worry about coefficients. Just write the molecular equation, and see which of these appears in it.) OH (s) Ba2 (aq) O NH,OH (s) BaCO3 (s) O NH2"(aq)
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A 38.5 mL sample of 0.875M AgNO3 solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and the percent yield.AgNO3 (aq) + NaCl (aq) ---> AgCl (s) + NaNO3 (aq)
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Complete and balance the given precipitation reactions, including the physical states of the products as predicted by the solubility rules. Ba(NO3)2 (aq) + CuSO4 (aq) ---> K3PO3(aq) + MgCl2 (aq) ---> Examine the precipitation reactions to determine whether each of the involved species is oxidized, reduced, or neither. Ba2+, SO42-, Cu2+, PO43-, Cl-, Mg2+, K+, NO3-