mpound is dissolved in water, the olution is either an electrolyte or a yte. The solution of an electrolyte has o conduct an electric current. A strong dissociates or ionizes almost completely whereas weak electrolyte undergoes dionization or or dissociation. The solution vation ectrolyte does not conduct a current ew, if any, ions are present in the solution. ical conductivity of a solution can easily red with a meter a light bulb. The total ntration of any solution is determined by ype and the concentration of solute. The electrical conductivities of the following 0.100 M solutions were measured in an apparatus that contained a light bulb as the indicator of conductivity. Rank the solutions in order of decreasing intensity (brightest to dimmest) of the light bulb. Rank from brightest to dimmest bulb. To rank items as equivalent, overlap them. ►View Available Hint(s) Brightest Submit Al(NO3)3 | KI HF CH3OH Reset Help Dimmest
mpound is dissolved in water, the olution is either an electrolyte or a yte. The solution of an electrolyte has o conduct an electric current. A strong dissociates or ionizes almost completely whereas weak electrolyte undergoes dionization or or dissociation. The solution vation ectrolyte does not conduct a current ew, if any, ions are present in the solution. ical conductivity of a solution can easily red with a meter a light bulb. The total ntration of any solution is determined by ype and the concentration of solute. The electrical conductivities of the following 0.100 M solutions were measured in an apparatus that contained a light bulb as the indicator of conductivity. Rank the solutions in order of decreasing intensity (brightest to dimmest) of the light bulb. Rank from brightest to dimmest bulb. To rank items as equivalent, overlap them. ►View Available Hint(s) Brightest Submit Al(NO3)3 | KI HF CH3OH Reset Help Dimmest
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...
Related questions
Question
Answer part A,B , and C
![### Understanding Electrolytic Solutions
When a compound is dissolved in water, the resulting solution is either an electrolyte or a nonelectrolyte.
- **Electrolyte**: This type of solution can conduct an electric current. Strong electrolytes dissociate or ionize almost completely into ions, while weak electrolytes undergo only limited ionization or dissociation.
- **Nonelectrolyte**: This type of solution does not conduct a current due to the absence or minimal presence of ions.
The electrical conductivity of a solution is easily measured with a meter or a light bulb. The total ion concentration of any solution is determined by both the type and the concentration of solute.
### Ranking Conductivity of Solutions
**Part A:**
The electrical conductivities of the following 0.100 M solutions were measured using a light bulb as the conductivity indicator. Rank these solutions in order from the brightest (indicating highest conductivity) to the dimmest (indicating lowest conductivity) light bulb intensity:
- Al(NO₃)₃ (Aluminum nitrate)
- KI (Potassium iodide)
- HF (Hydrofluoric acid)
- CH₃OH (Methanol)
**Task:**
Rank from the brightest to the dimmest bulb by placing the chemical formulas in a box diagram labeled "Brightest" to "Dimmest." If solutions are equivalent in conductivity, overlap them.
- **Al(NO₃)₃**, **KI**, **HF**, **CH₃OH**
Example layout to complete:
| Brightest | | | Dimmest |
|-----------|------------------|----------------|---------|
| [ ] | | | [ ] |
### Instructions:
Drag each chemical formula to the appropriate spot on the diagram, considering their conductivity in water. Use "Help" or "Hint(s)" if necessary to make informed decisions.
Once your ranking is complete, select the "Submit" button.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2F9f5b5aa4-45cd-4dae-8bd2-cfe23b774d47%2F3oaiuu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding Electrolytic Solutions
When a compound is dissolved in water, the resulting solution is either an electrolyte or a nonelectrolyte.
- **Electrolyte**: This type of solution can conduct an electric current. Strong electrolytes dissociate or ionize almost completely into ions, while weak electrolytes undergo only limited ionization or dissociation.
- **Nonelectrolyte**: This type of solution does not conduct a current due to the absence or minimal presence of ions.
The electrical conductivity of a solution is easily measured with a meter or a light bulb. The total ion concentration of any solution is determined by both the type and the concentration of solute.
### Ranking Conductivity of Solutions
**Part A:**
The electrical conductivities of the following 0.100 M solutions were measured using a light bulb as the conductivity indicator. Rank these solutions in order from the brightest (indicating highest conductivity) to the dimmest (indicating lowest conductivity) light bulb intensity:
- Al(NO₃)₃ (Aluminum nitrate)
- KI (Potassium iodide)
- HF (Hydrofluoric acid)
- CH₃OH (Methanol)
**Task:**
Rank from the brightest to the dimmest bulb by placing the chemical formulas in a box diagram labeled "Brightest" to "Dimmest." If solutions are equivalent in conductivity, overlap them.
- **Al(NO₃)₃**, **KI**, **HF**, **CH₃OH**
Example layout to complete:
| Brightest | | | Dimmest |
|-----------|------------------|----------------|---------|
| [ ] | | | [ ] |
### Instructions:
Drag each chemical formula to the appropriate spot on the diagram, considering their conductivity in water. Use "Help" or "Hint(s)" if necessary to make informed decisions.
Once your ranking is complete, select the "Submit" button.
![**Transcription for Educational Website**
---
When you are given a concentration for a compound, such as \( 1 \, M \, \text{NaCl} \), it indicates the number of moles of formula units per liter (formula-unit concentration). By multiplying the formula-unit concentration by the number of ions per formula unit, you arrive at the ion concentration. For example, a \( 1 \, M \) solution of \(\text{NaCl}\) has a \( 2 \, M \) ion concentration (\( 1 \, M \) of \(\text{Na}^+\) ions and \( 1 \, M \) of \(\text{Cl}^-\) ions) because there are two ions per formula unit of \(\text{NaCl}\). A \( 1 \, M \) solution of \(\text{Na}_2\text{S}\) has a \( 3 \, M \) ion concentration (\( 2 \, M \) of \(\text{Na}^+\) ions and \( 1 \, M \) of \(\text{S}^{2-}\) ions) because there are three ions per formula unit of \(\text{Na}_2\text{S}\).
**Part B**
What is the concentration of \(\text{K}^+\) ions in a \( 0.045 \, M \, \text{K}_2\text{CO}_3 \) solution assuming complete dissociation?
**Express the concentration in molarity.**
\[ \text{concentration of } \text{K}^+ = \] \_\_\_\_\_ \( M \)
[Submit]
**Part C**
A \( 0.100 \, M \) solution of \(\text{K}_2\text{SO}_4\) would contain the same total ion concentration as which of the following solutions?
- \( 0.0800 \, M \, \text{Na}_2\text{CO}_3 \)
- \( 0.100 \, M \, \text{NaCl} \)
- \( 0.0750 \, M \, \text{Na}_3\text{PO}_4 \)
- \( 0.0500 \, M \, \text{NaOH} \)
[View Available Hint(s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2F9f5b5aa4-45cd-4dae-8bd2-cfe23b774d47%2Fq3j5h3u_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
---
When you are given a concentration for a compound, such as \( 1 \, M \, \text{NaCl} \), it indicates the number of moles of formula units per liter (formula-unit concentration). By multiplying the formula-unit concentration by the number of ions per formula unit, you arrive at the ion concentration. For example, a \( 1 \, M \) solution of \(\text{NaCl}\) has a \( 2 \, M \) ion concentration (\( 1 \, M \) of \(\text{Na}^+\) ions and \( 1 \, M \) of \(\text{Cl}^-\) ions) because there are two ions per formula unit of \(\text{NaCl}\). A \( 1 \, M \) solution of \(\text{Na}_2\text{S}\) has a \( 3 \, M \) ion concentration (\( 2 \, M \) of \(\text{Na}^+\) ions and \( 1 \, M \) of \(\text{S}^{2-}\) ions) because there are three ions per formula unit of \(\text{Na}_2\text{S}\).
**Part B**
What is the concentration of \(\text{K}^+\) ions in a \( 0.045 \, M \, \text{K}_2\text{CO}_3 \) solution assuming complete dissociation?
**Express the concentration in molarity.**
\[ \text{concentration of } \text{K}^+ = \] \_\_\_\_\_ \( M \)
[Submit]
**Part C**
A \( 0.100 \, M \) solution of \(\text{K}_2\text{SO}_4\) would contain the same total ion concentration as which of the following solutions?
- \( 0.0800 \, M \, \text{Na}_2\text{CO}_3 \)
- \( 0.100 \, M \, \text{NaCl} \)
- \( 0.0750 \, M \, \text{Na}_3\text{PO}_4 \)
- \( 0.0500 \, M \, \text{NaOH} \)
[View Available Hint(s
Expert Solution
Step 1: Concept
- Electrical conductivity of a solution is due to the motion of electron or ions present in it.
- Ionic substances dissolve in water and conduct electricity due to freedom of motion of ions.
- The electrical conductivity is directly related to the number of ions present in the solution and the rate of the ionization of compounds.
- The more the number of ions higher will be the conductivity.
- The higher the conductivity more brighter will be the bulb.
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