© Macmillan Learning Experiment 1: Suppose a student repeats the experiment, but adds 25 g of sodium bicarbonate to the 6 M HC instead of adding 1 M NaOH. What observations indicate that a reaction took place? Bubbles formed in the solution after the sodium bicarbonate was added to the HCl in the Erlenmeyer flas The solution changed color after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. A reaction did not happen when the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. The temperature decreased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. A precipitate (solid) formed after the sodium bicarbonate was added to the HCI in the Erlenmeyer flask. The temperature increased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.

© Macmillan Learning Experiment 1: Suppose a student repeats the experiment, but adds 25 g of sodium bicarbonate to the 6 M HC instead of adding 1 M NaOH. What observations indicate that a reaction took place? Bubbles formed in the solution after the sodium bicarbonate was added to the HCl in the Erlenmeyer flas The solution changed color after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. A reaction did not happen when the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. The temperature decreased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask. A precipitate (solid) formed after the sodium bicarbonate was added to the HCI in the Erlenmeyer flask. The temperature increased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.

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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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Macmillan Learning
Experiment 1: Suppose a student repeats the experiment, but adds 25 g of sodium bicarbonate to the 6 M HC
instead of adding 1 M NaOH. What observations indicate that a reaction took place?
Bubbles formed in the solution after the sodium bicarbonate was added to the HCl in the Erlenmeyer flas
The solution changed color after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
A reaction did not happen when the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
The temperature decreased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
A precipitate (solid) formed after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.
The temperature increased after the sodium bicarbonate was added to the HCl in the Erlenmeyer flask.

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