1. You are mixing an aqueous solution of NiCl2 (aq) with an aqueous solution of (NH4)2CO3(aq). (a) Use the double replacement method to identify the products of this reaction. NiCl2 (aq) + (NH4)2CO3(aq) (b) Rewrite the chemical equation in part a) in the space below and balance it accordingly. X (c) Use the Solubility Guidelines table (Chapter 4 lecture slide #28) to identify whether a precipitate (a compound that is not water soluble) will be formed during this reaction. Write the formula of the precipitate (the solid) in this box (d) Write the complete ionic equation for this precipitation reaction. Include physical status (aq, s)
1. You are mixing an aqueous solution of NiCl2 (aq) with an aqueous solution of (NH4)2CO3(aq). (a) Use the double replacement method to identify the products of this reaction. NiCl2 (aq) + (NH4)2CO3(aq) (b) Rewrite the chemical equation in part a) in the space below and balance it accordingly. X (c) Use the Solubility Guidelines table (Chapter 4 lecture slide #28) to identify whether a precipitate (a compound that is not water soluble) will be formed during this reaction. Write the formula of the precipitate (the solid) in this box (d) Write the complete ionic equation for this precipitation reaction. Include physical status (aq, s)
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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Transcribed Image Text:1. You are mixing an aqueous solution of NiCl2 (aq) with an aqueous solution of (NH4)2CO3(aq).
(a) Use the double replacement method to identify the products of this reaction.
NiCl2 (aq) + (NH4)2CO3 (aq)
-
(b) Rewrite the chemical equation in part a) in the space below and balance it accordingly.
I
(c) Use the Solubility Guidelines table (Chapter 4 lecture slide #28) to identify whether a precipitate (a
compound that is not water soluble) will be formed during this reaction.
Write the formula of the precipitate (the solid) in this box
(d) Write the complete ionic equation for this precipitation reaction. Include physical status (aq, s)
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