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### Methods to Dilute a Solution of Sodium Chloride ([tex]\( \text{NaCl} \)[/tex])
- Add more [tex]\( \text{NaCl} \)[/tex] to the solution.
- This method is incorrect. Adding more [tex]\( \text{NaCl} \)[/tex] will increase the concentration of the solution, thus making it more concentrated, not diluted.
- Add more water to the solution.
- This method is correct. Adding more water to the solution will decrease the concentration of sodium chloride, thus diluting the solution.
- Remove a small amount of the solution and mix it with water.
- This method is correct. Removing a small portion of the original solution and mixing it with water will reduce the overall concentration of [tex]\( \text{NaCl} \)[/tex], thereby diluting it.
- Heat the solution to evaporate some of the water.
- This method is incorrect. Heating the solution to evaporate some of the water will increase the concentration of [tex]\( \text{NaCl} \)[/tex], thus making it more concentrated, not diluted.
Thus, the correct methods to dilute a solution of sodium chloride are:
- Add more water to the solution.
- Remove a small amount of the solution and mix it with water.
### Labeling Solutions as Concentrated (C) or Dilute (D)
Based on the provided molarity data, we will classify each solution as either concentrated (C) or dilute (D) using a threshold value of [tex]\( 1.0 \)[/tex] M.
Threshold: Molarity > 1.0 M is considered Concentrated (C), otherwise it is Dilute (D).
Given molarity values are:
- A = 12 M (concentrated)
- B = 0.5 M (dilute)
- C = 0.01 M (dilute)
- D = 6.0 M (concentrated)
- E = 0.05 M (dilute)
- F = 10 M (concentrated)
Following this classification:
[tex]\[ \begin{array}{|l|ll|} \hline \begin{array}{l} \text{acid } I \\ \text{base} \end{array} & \text{molarity} & \text{concentrated or dilute} \\ \hline \multirow{2}{*}{$\text{HCl}$} & 12 \, \text{M} & \text{C (concentrated) (A)} \\ \cline { 2 - 3 } & 0.5 \, \text{M} & \text{D (dilute) (B)} \\ \hline \multirow{2}{*}{$\text{NaOH}$} & 0.01 \, \text{M} & \text{D (dilute) (C)} \\ \cline { 2 - 3 } & 6.0 \, \text{M} & \text{C (concentrated) (D)} \\ \hline \multirow{2}{*}{$\text{H}_2\text{SO}_4$} & 0.05 \, \text{M} & \text{D (dilute) (E)} \\ \cline { 2 - 3 } & 10 \, \text{M} & \text{C (concentrated) (F)} \\ \hline \end{array} \][/tex]
Final Table with Labels:
[tex]\[ \begin{array}{|l|ll|} \hline \begin{array}{l} \text{acid } I \\ \text{base} \end{array} & \text{molarity} & \text{concentrated or dilute} \\ \hline \multirow{2}{*}{$\text{HCl}$} & 12 \, \text{M} & \text{C (concentrated)} \\ \cline { 2 - 3 } & 0.5 \, \text{M} & \text{D (dilute)} \\ \hline \multirow{2}{*}{$\text{NaOH}$} & 0.01 \, \text{M} & \text{D (dilute)} \\ \cline { 2 - 3 } & 6.0 \, \text{M} & \text{C (concentrated)} \\ \hline \multirow{2}{*}{$\text{H}_2\text{SO}_4$} & 0.05 \, \text{M} & \text{D (dilute)} \\ \cline { 2 - 3 } & 10 \, \text{M} & \text{C (concentrated)} \\ \hline \end{array} \][/tex]
### Summary:
1. The methods to dilute a solution of sodium chloride are adding more water [tex]\( \checkmark \)[/tex] and removing a small amount of the solution and mixing it with water [tex]\( \checkmark \)[/tex].
2. The classifications based on molarity are:
- [tex]\( A \)[/tex]: 12 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
- [tex]\( B \)[/tex]: 0.5 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( C \)[/tex]: 0.01 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( D \)[/tex]: 6.0 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
- [tex]\( E \)[/tex]: 0.05 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( F \)[/tex]: 10 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
- Add more [tex]\( \text{NaCl} \)[/tex] to the solution.
- This method is incorrect. Adding more [tex]\( \text{NaCl} \)[/tex] will increase the concentration of the solution, thus making it more concentrated, not diluted.
- Add more water to the solution.
- This method is correct. Adding more water to the solution will decrease the concentration of sodium chloride, thus diluting the solution.
- Remove a small amount of the solution and mix it with water.
- This method is correct. Removing a small portion of the original solution and mixing it with water will reduce the overall concentration of [tex]\( \text{NaCl} \)[/tex], thereby diluting it.
- Heat the solution to evaporate some of the water.
- This method is incorrect. Heating the solution to evaporate some of the water will increase the concentration of [tex]\( \text{NaCl} \)[/tex], thus making it more concentrated, not diluted.
Thus, the correct methods to dilute a solution of sodium chloride are:
- Add more water to the solution.
- Remove a small amount of the solution and mix it with water.
### Labeling Solutions as Concentrated (C) or Dilute (D)
Based on the provided molarity data, we will classify each solution as either concentrated (C) or dilute (D) using a threshold value of [tex]\( 1.0 \)[/tex] M.
Threshold: Molarity > 1.0 M is considered Concentrated (C), otherwise it is Dilute (D).
Given molarity values are:
- A = 12 M (concentrated)
- B = 0.5 M (dilute)
- C = 0.01 M (dilute)
- D = 6.0 M (concentrated)
- E = 0.05 M (dilute)
- F = 10 M (concentrated)
Following this classification:
[tex]\[ \begin{array}{|l|ll|} \hline \begin{array}{l} \text{acid } I \\ \text{base} \end{array} & \text{molarity} & \text{concentrated or dilute} \\ \hline \multirow{2}{*}{$\text{HCl}$} & 12 \, \text{M} & \text{C (concentrated) (A)} \\ \cline { 2 - 3 } & 0.5 \, \text{M} & \text{D (dilute) (B)} \\ \hline \multirow{2}{*}{$\text{NaOH}$} & 0.01 \, \text{M} & \text{D (dilute) (C)} \\ \cline { 2 - 3 } & 6.0 \, \text{M} & \text{C (concentrated) (D)} \\ \hline \multirow{2}{*}{$\text{H}_2\text{SO}_4$} & 0.05 \, \text{M} & \text{D (dilute) (E)} \\ \cline { 2 - 3 } & 10 \, \text{M} & \text{C (concentrated) (F)} \\ \hline \end{array} \][/tex]
Final Table with Labels:
[tex]\[ \begin{array}{|l|ll|} \hline \begin{array}{l} \text{acid } I \\ \text{base} \end{array} & \text{molarity} & \text{concentrated or dilute} \\ \hline \multirow{2}{*}{$\text{HCl}$} & 12 \, \text{M} & \text{C (concentrated)} \\ \cline { 2 - 3 } & 0.5 \, \text{M} & \text{D (dilute)} \\ \hline \multirow{2}{*}{$\text{NaOH}$} & 0.01 \, \text{M} & \text{D (dilute)} \\ \cline { 2 - 3 } & 6.0 \, \text{M} & \text{C (concentrated)} \\ \hline \multirow{2}{*}{$\text{H}_2\text{SO}_4$} & 0.05 \, \text{M} & \text{D (dilute)} \\ \cline { 2 - 3 } & 10 \, \text{M} & \text{C (concentrated)} \\ \hline \end{array} \][/tex]
### Summary:
1. The methods to dilute a solution of sodium chloride are adding more water [tex]\( \checkmark \)[/tex] and removing a small amount of the solution and mixing it with water [tex]\( \checkmark \)[/tex].
2. The classifications based on molarity are:
- [tex]\( A \)[/tex]: 12 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
- [tex]\( B \)[/tex]: 0.5 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( C \)[/tex]: 0.01 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( D \)[/tex]: 6.0 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
- [tex]\( E \)[/tex]: 0.05 M [tex]\(\rightarrow\)[/tex] Dilute (D)
- [tex]\( F \)[/tex]: 10 M [tex]\(\rightarrow\)[/tex] Concentrated (C)
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