Determining the State of the Solution

Oct 13, 2025 by recoveryshake.com 75 views

Introduction

In chemistry, the state of a solution is a crucial concept that helps us understand the behavior of substances dissolved in a solvent. A solution can be classified as saturated, supersaturated, dilute, or unsaturated based on the concentration of the solute and the solvent. In this article, we will explore the characteristics of each state and determine which one applies to a solution containing 60 grams of $$NaNO_3$$ completely dissolved in 50 grams of water at $$50^{\circ}C$$.

What is a Saturated Solution?

A saturated solution is a solution that contains the maximum amount of solute that can dissolve in a given amount of solvent at a particular temperature. In other words, the solution is fully saturated with the solute, and no more solute can be added without causing the solution to become supersaturated. A saturated solution is in equilibrium with its solid phase, meaning that the concentration of the solute in the solution is equal to the concentration of the solute in the solid phase.

What is a Supersaturated Solution?

A supersaturated solution is a solution that contains more solute than it can normally hold at a particular temperature. This means that the solution is not in equilibrium with its solid phase, and the concentration of the solute in the solution is greater than the concentration of the solute in the solid phase. Supersaturated solutions are unstable and can become saturated or even precipitate out of solution if a small disturbance occurs.

What is a Dilute Solution?

A dilute solution is a solution that contains a small amount of solute in a large amount of solvent. Dilute solutions are typically characterized by a low concentration of the solute, usually less than 1 mole per liter. Dilute solutions are often used in laboratory experiments and are typically stable and easy to handle.

What is an Unsaturated Solution?

An unsaturated solution is a solution that contains less solute than it can normally hold at a particular temperature. This means that the solution is not in equilibrium with its solid phase, and the concentration of the solute in the solution is less than the concentration of the solute in the solid phase. Unsaturated solutions are stable and can be used to dissolve more solute without causing the solution to become supersaturated.

Determining the State of the Solution

Now that we have a good understanding of the different states of a solution, let's apply this knowledge to the given problem. We are given a solution containing 60 grams of $$NaNO_3$$ completely dissolved in 50 grams of water at $$50^{\circ}C$$. To determine the state of the solution, we need to consider the concentration of the solute and the solvent.

Calculating the Concentration of the Solute

To calculate the concentration of the solute, we need to know the molar mass of $$NaNO_3$$. The molar mass of $$NaNO_3$$ is 84.99 g/mol. We can calculate the number of moles of $$NaNO_3$$ in the solution as follows:

n = \frac{m}{M}

where $$n$$ is the number of moles, $$m$$ is the mass of the solute, and $$M$$ is the molar mass of the solute.

n = \frac{60 \text{ g}}{84.99 \text{ g/mol}} = 0.707 \text{ mol}

Calculating the Concentration of the Solvent

To calculate the concentration of the solvent, we need to know the mass of the solvent. We are given that the mass of the solvent is 50 grams. We can calculate the molarity of the solution as follows:

M = \frac{n}{V}

where $$M$$ is the molarity, $$n$$ is the number of moles, and $$V$$ is the volume of the solution in liters.

Since we are given the mass of the solvent, we can calculate the volume of the solution as follows:

V = \frac{m}{\rho}

where $$V$$ is the volume, $$m$$ is the mass of the solvent, and $$\rho$$ is the density of the solvent.

The density of water at $$50^{\circ}C$$ is approximately 0.973 g/mL. We can calculate the volume of the solution as follows:

V = \frac{50 \text{ g}}{0.973 \text{ g/mL}} = 51.4 \text{ mL}

We can now calculate the molarity of the solution as follows:

M = \frac{0.707 \text{ mol}}{0.0514 \text{ L}} = 13.8 \text{ M}

Determining the State of the Solution

Now that we have calculated the concentration of the solute and the solvent, we can determine the state of the solution. We are given that the solution is at $$50^{\circ}C$$, which is above the solubility temperature of $$NaNO_3$$. This means that the solution is likely to be supersaturated.

However, we need to consider the concentration of the solute and the solvent. We have calculated the molarity of the solution to be 13.8 M, which is relatively high. This suggests that the solution is likely to be saturated.

Conclusion

In conclusion, the solution containing 60 grams of $$NaNO_3$$ completely dissolved in 50 grams of water at $$50^{\circ}C$$ is likely to be saturated. The high concentration of the solute and the solvent suggests that the solution is in equilibrium with its solid phase, and no more solute can be added without causing the solution to become supersaturated.

References

CRC Handbook of Chemistry and Physics, 97th ed.
International Critical Tables of Numerical Data, Physics, Chemistry and Technology, 3rd ed.
Physical Chemistry: A Molecular Approach, 2nd ed.

Glossary

Saturated solution: A solution that contains the maximum amount of solute that can dissolve in a given amount of solvent at a particular temperature.
Supersaturated solution: A solution that contains more solute than it can normally hold at a particular temperature.
Dilute solution: A solution that contains a small amount of solute in a large amount of solvent.
Unsaturated solution: A solution that contains less solute than it can normally hold at a particular temperature.
Molarity: A measure of the concentration of a solution, expressed in moles per liter.
Molar mass: The mass of one mole of a substance, expressed in grams per mole.
Density: The mass of a substance per unit volume, expressed in grams per milliliter.

Introduction

In our previous article, we explored the concept of the state of a solution, including saturated, supersaturated, dilute, and unsaturated solutions. We also applied this knowledge to a specific problem involving a solution containing 60 grams of $$NaNO_3$$ completely dissolved in 50 grams of water at $$50^{\circ}C$$. In this article, we will answer some frequently asked questions related to the state of a solution.

Q: What is the difference between a saturated and a supersaturated solution?

A: A saturated solution is a solution that contains the maximum amount of solute that can dissolve in a given amount of solvent at a particular temperature. A supersaturated solution, on the other hand, is a solution that contains more solute than it can normally hold at a particular temperature.

Q: How can I determine if a solution is saturated or supersaturated?

A: To determine if a solution is saturated or supersaturated, you need to consider the concentration of the solute and the solvent. If the solution is in equilibrium with its solid phase, it is likely to be saturated. If the solution contains more solute than it can normally hold at a particular temperature, it is likely to be supersaturated.

Q: What is the significance of the solubility temperature of a substance?

A: The solubility temperature of a substance is the temperature at which the substance dissolves in a solvent. If the solution is above the solubility temperature, it is likely to be supersaturated.

Q: Can a solution be both saturated and supersaturated at the same time?

A: No, a solution cannot be both saturated and supersaturated at the same time. A solution is either saturated or supersaturated, but not both.

Q: How can I prevent a solution from becoming supersaturated?

A: To prevent a solution from becoming supersaturated, you need to ensure that the solution is not heated above the solubility temperature of the substance. You also need to avoid adding too much solute to the solution, as this can cause the solution to become supersaturated.

Q: What is the difference between a dilute and an unsaturated solution?

A: A dilute solution is a solution that contains a small amount of solute in a large amount of solvent. An unsaturated solution, on the other hand, is a solution that contains less solute than it can normally hold at a particular temperature.

Q: Can a solution be both dilute and unsaturated at the same time?

A: Yes, a solution can be both dilute and unsaturated at the same time. For example, a solution that contains a small amount of solute in a large amount of solvent may also contain less solute than it can normally hold at a particular temperature.

Q: How can I determine the concentration of a solution?

A: To determine the concentration of a solution, you need to know the molarity of the solution. You can calculate the molarity of the solution by dividing the number of moles of the solute by the volume of the solution in liters.

Q: What is the significance of the molarity of a solution?

A: The molarity of a solution is a measure of the concentration of the solution, expressed in moles per liter. It is an important parameter in chemistry, as it helps to determine the behavior of the solution.

Q: Can a solution have a molarity of zero?

A: No, a solution cannot have a molarity of zero. A solution with a molarity of zero would mean that there is no solute present in the solution, which is not possible.

Q: How can I calculate the molarity of a solution?

A: To calculate the molarity of a solution, you need to know the number of moles of the solute and the volume of the solution in liters. You can calculate the molarity of the solution by dividing the number of moles of the solute by the volume of the solution in liters.

Q: What is the difference between a solution and a mixture?

A: A solution is a homogeneous mixture of two or more substances, where the solute is dissolved in the solvent. A mixture, on the other hand, is a heterogeneous mixture of two or more substances, where the components are not dissolved in each other.

Q: Can a solution be a mixture?

A: Yes, a solution can be a mixture. For example, a solution of sugar and water is a homogeneous mixture of two substances, but it is also a solution because the sugar is dissolved in the water.

Q: Can a mixture be a solution?

A: No, a mixture cannot be a solution. A mixture is a heterogeneous mixture of two or more substances, where the components are not dissolved in each other.

Conclusion

In conclusion, the state of a solution is an important concept in chemistry that helps us understand the behavior of substances dissolved in a solvent. By understanding the differences between saturated, supersaturated, dilute, and unsaturated solutions, we can determine the concentration of a solution and predict its behavior. We hope that this article has helped to answer some of the frequently asked questions related to the state of a solution.