In another experiment, assuming that Na2CO3 were not in excess but rather was the limiting reactant. If tap water containing calcium ions is used instead of deionized water, to dissolve the reactants, how would the amount of precipitate change?
In another experiment, assuming that Na2CO3 were not in excess but rather was the limiting reactant. If tap water containing calcium ions is used instead of deionized water, to dissolve the reactants, how would the amount of precipitate change?
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
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
Transcribed Image Text:In another experiment, assuming that Na2CO3 were not in excess but rather was
the limiting reactant. If tap water containing calcium ions is used instead of
deionized water, to dissolve the reactants, how would the amount of precipitate
change?
Stay the same.
Increase
Cannot be determined.
Decrease
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