Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) a. Balanced formula equation: HNO3(aq) + Complete ionic equation: + Net ionic equation: + Mg(OH)₂ (s) +
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) a. Balanced formula equation: HNO3(aq) + Complete ionic equation: + Net ionic equation: + Mg(OH)₂ (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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![### Balanced Formula and Ionic Equations
**Balanced Formula Equation:**
\[ \text{HCNO(aq)} + \text{KOH(aq)} \rightarrow \]
**Complete Ionic Equation:**
\[ \text{HCNO(aq)} + \text{KOH(aq)} \rightarrow \]
**Net Ionic Equation:**
\[ + \rightarrow + \]
#### Description:
The image illustrates how to write balanced formula equations, complete ionic equations, and net ionic equations for a given reaction. Spaces are provided where the reactants and products should be placed.
**Balanced Formula Equation:**
The balanced formula equation involves writing down the reactants and products of the reaction in their correct molecular forms. In this case, the reactants are HCNO (aqueous) and KOH (aqueous).
**Complete Ionic Equation:**
The complete ionic equation splits the aqueous compounds into their respective ions. This representation shows all of the ions that participate in the reaction.
**Net Ionic Equation:**
The net ionic equation further simplifies the complete ionic equation by removing the spectator ions (ions that do not participate in the reaction). Only the ions that undergo a chemical change are included. This provides a clearer depiction of the actual chemical reaction taking place.
In each step, the reactants are written on the left side and the products on the right side, separated by an arrow indicating the direction of the reaction.
These steps are crucial in understanding chemical reactions, ensuring they are balanced in terms of mass and charge, and identifying the actual species involved in the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6866a817-1533-406a-ba8e-1b8632cbf7e9%2F539e66a5-c7f6-45a7-925b-54f06ca802a4%2Fdbtp9i_processed.png&w=3840&q=75)
Transcribed Image Text:### Balanced Formula and Ionic Equations
**Balanced Formula Equation:**
\[ \text{HCNO(aq)} + \text{KOH(aq)} \rightarrow \]
**Complete Ionic Equation:**
\[ \text{HCNO(aq)} + \text{KOH(aq)} \rightarrow \]
**Net Ionic Equation:**
\[ + \rightarrow + \]
#### Description:
The image illustrates how to write balanced formula equations, complete ionic equations, and net ionic equations for a given reaction. Spaces are provided where the reactants and products should be placed.
**Balanced Formula Equation:**
The balanced formula equation involves writing down the reactants and products of the reaction in their correct molecular forms. In this case, the reactants are HCNO (aqueous) and KOH (aqueous).
**Complete Ionic Equation:**
The complete ionic equation splits the aqueous compounds into their respective ions. This representation shows all of the ions that participate in the reaction.
**Net Ionic Equation:**
The net ionic equation further simplifies the complete ionic equation by removing the spectator ions (ions that do not participate in the reaction). Only the ions that undergo a chemical change are included. This provides a clearer depiction of the actual chemical reaction taking place.
In each step, the reactants are written on the left side and the products on the right side, separated by an arrow indicating the direction of the reaction.
These steps are crucial in understanding chemical reactions, ensuring they are balanced in terms of mass and charge, and identifying the actual species involved in the reaction.
![### Acid-Base Reaction Equations
This section covers the process of writing balanced formula, complete ionic, and net ionic equations for acid-base reactions. Please pay attention to the importance of specifying states such as (aq) for aqueous and (s) for solid. If a box is not needed, you may leave it blank. If no reaction occurs, leave all boxes blank and proceed by clicking 'Submit.'
#### Reaction Example:
#### Balanced Formula Equation:
\[ \text{HNO}_3 (aq) + \text{Mg(OH)}_2 (s) \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|
| | \[ + \] | |
#### Complete Ionic Equation:
\[ \text{\_\_\_\_\_\_\_\_\_\_} \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|:--:|:--:|
| \[ \rightarrow \] | | \[ + \] | | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
#### Net Ionic Equation:
\[ \text{\_\_\_\_\_\_\_\_\_\_} \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|
| \[ \rightarrow \] | |
#### Notes:
- **Balanced Formula Equation**: Consists of the complete compounds that participate in the reaction.
- **Complete Ionic Equation**: Shows all the ions separately as they exist in the aqueous solution. Solids and liquids are un-diassociated.
- **Net Ionic Equation**: Shows only the species that actually participate in the reaction, omitting the spectator ions.
By correctly identifying each step and using the appropriate states](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6866a817-1533-406a-ba8e-1b8632cbf7e9%2F539e66a5-c7f6-45a7-925b-54f06ca802a4%2Fhqi8zn1_processed.png&w=3840&q=75)
Transcribed Image Text:### Acid-Base Reaction Equations
This section covers the process of writing balanced formula, complete ionic, and net ionic equations for acid-base reactions. Please pay attention to the importance of specifying states such as (aq) for aqueous and (s) for solid. If a box is not needed, you may leave it blank. If no reaction occurs, leave all boxes blank and proceed by clicking 'Submit.'
#### Reaction Example:
#### Balanced Formula Equation:
\[ \text{HNO}_3 (aq) + \text{Mg(OH)}_2 (s) \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|
| | \[ + \] | |
#### Complete Ionic Equation:
\[ \text{\_\_\_\_\_\_\_\_\_\_} \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|:--:|:--:|
| \[ \rightarrow \] | | \[ + \] | | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
#### Net Ionic Equation:
\[ \text{\_\_\_\_\_\_\_\_\_\_} \rightarrow \]
| \( \text{\_\_\_\_\_\_\_\_\_\_} \) | \[ + \] | \( \text{\_\_\_\_\_\_\_\_\_\_} \) |
|:--:|:--:|:--:|
| \[ \rightarrow \] | |
#### Notes:
- **Balanced Formula Equation**: Consists of the complete compounds that participate in the reaction.
- **Complete Ionic Equation**: Shows all the ions separately as they exist in the aqueous solution. Solids and liquids are un-diassociated.
- **Net Ionic Equation**: Shows only the species that actually participate in the reaction, omitting the spectator ions.
By correctly identifying each step and using the appropriate states
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