---
title: "Saturated Solution | General Chemistry II"
description: "A saturated solution holds the maximum dissolved solute at a given temperature and pressure, creating equilibrium you use in Ksp and molar solubility problems."
canonical: "https://fiveable.me/general-chemistry-ii/key-terms/saturated-solution"
type: "key-term"
subject: "General Chemistry II"
unit: "Unit 5"
---

# Saturated Solution | General Chemistry II

## Definition

A saturated solution is a General Chemistry II solution that has dissolved as much solute as it can at a given temperature and pressure. Extra solute stays undissolved because the system has reached equilibrium.

## What It Is

A saturated solution is the point where a solute and its ions or molecules are in balance with the undissolved solid in General Chemistry II. At that point, the solution has dissolved the maximum amount it can hold under the current conditions, so any extra solute you add will not keep disappearing into the liquid.

The tricky part is that “maximum amount” does not mean the solution has stopped changing. In a saturated system, particles are still dissolving and also coming back out of solution at the same time. Those two rates are equal, so the concentration stays constant even though the process is active. That is why saturation is a dynamic equilibrium, not a motionless state.

For ionic solids, this idea connects directly to solubility and the solubility product constant, Ksp. Once a sparingly soluble salt reaches saturation, the dissolved ions in water are described by an equilibrium expression. A salt like silver chloride is a classic example, because only a tiny amount dissolves before the equilibrium is established and the rest remains as solid.

Temperature matters too. For many solid solutes, raising the temperature increases solubility, so a solution that was saturated at room temperature may become unsaturated if you heat it. The reverse can happen when you cool it, which is why crystals can form as a hot solution loses its ability to keep the same amount dissolved.

Do not confuse saturation with a cloudy or concentrated-looking mixture. A saturated solution can look perfectly clear if all of the dissolved solute is below the visible limit and no excess solid is being stirred up. The real test is whether more solute can dissolve under the same conditions, not whether the solution “looks full.”

## Why It Matters

Saturated solution is the starting point for a lot of the equilibrium chemistry in General Chemistry II. If you do not know when a solution is saturated, it is hard to set up Ksp problems, compare molar solubility values, or predict whether a precipitate should form.

This term also shows you how chemistry changes when conditions change. If you add more solute, heat the solution, or change the pH, the saturation point can shift. That is the same equilibrium thinking you use later for solubility in acidic solutions and complex ion behavior.

In lab, saturation shows up in real observations: leftover solid in a beaker, crystals forming after cooling, or a clear solution that suddenly turns cloudy when the ion product exceeds the solubility limit. Those are the moments when the abstract equilibrium language turns into something you can actually see and measure.

## Connections

### solubility product constant (Ksp)

Ksp is the equilibrium constant that describes a saturated solution of a sparingly soluble ionic compound. Once the solution is saturated, the dissolved ions settle into a fixed ratio, and Ksp lets you calculate or compare that equilibrium. If you know the Ksp, you can often work backward to the molar solubility.

### molar solubility

Molar solubility is the number of moles of a solute that dissolve per liter of solution at saturation. A saturated solution is the condition, and molar solubility is the measurable amount that results. In problem sets, you often use one to find the other by connecting the dissolution reaction to Ksp.

### [unsaturated solution](/general-chemistry-ii/key-terms/unsaturated-solution)

An unsaturated solution has not reached the maximum solute concentration yet, so more solute can still dissolve. That is the state before saturation, not after it. If you add a little more solute to an unsaturated solution, the amount disappears into the solvent instead of sitting at the bottom.

### [supersaturated solution](/general-chemistry-ii/key-terms/supersaturated-solution)

A supersaturated solution contains more dissolved solute than a normal saturated solution at that temperature, which makes it unstable. It can form by dissolving solute at a higher temperature and then cooling carefully. One crystal or disturbance can trigger rapid crystallization because the solution wants to drop back to saturation.

## On the AP Exam

A quiz or problem set question usually asks you to decide whether a solution is saturated, unsaturated, or supersaturated, then use that idea to predict what happens when more solute is added. You may also be asked to calculate molar solubility from a Ksp value or use the ion concentrations to see whether a precipitate forms. In a lab, the clue might be leftover solid, crystal formation after cooling, or a change in clarity when the equilibrium shifts. The main move is to connect the visible setup to the equilibrium condition underneath it.

## saturated solution vs supersaturated solution

A saturated solution is at equilibrium with the maximum amount of dissolved solute under the given conditions. A supersaturated solution has more solute dissolved than that equilibrium normally allows, so it is unstable and can crystallize suddenly. If a problem mentions leftover solid sitting at the bottom, that points to saturation, not supersaturation.

## Key Takeaways

- A saturated solution has dissolved as much solute as it can at a given temperature and pressure.
- Saturation is a dynamic equilibrium, so dissolving and precipitation are still happening at the same time.
- Extra solute added to a saturated solution will not dissolve unless the conditions change.
- Saturated solutions are the setup behind Ksp and many molar solubility calculations in General Chemistry II.
- Temperature can shift saturation, especially for solids, so heating or cooling can change how much stays dissolved.

## FAQs

### What is saturated solution in General Chemistry II?

A saturated solution is a solution that contains the maximum amount of solute that can dissolve at a specific temperature and pressure. At that point, the dissolved solute is in equilibrium with the undissolved solid. If you add more solute, it stays as solid instead of dissolving.

### How do you know if a solution is saturated?

If extra solute remains at the bottom after stirring, the solution is saturated at that temperature. In equilibrium language, the solution cannot dissolve any more solute without a change in conditions. A clear appearance does not prove saturation by itself, so the amount dissolving matters more than the look.

### Is a saturated solution the same as a concentrated solution?

No. A concentrated solution has a lot of solute, but it may still be unsaturated if more can dissolve. A saturated solution has reached the limit at that temperature, even if the actual concentration is lower than another concentrated solution made with a different solute.

### How does saturation connect to Ksp?

Ksp describes the equilibrium that exists in a saturated solution of a sparingly soluble salt. Once the solution is saturated, the dissolved ion concentrations are fixed by that equilibrium expression. That is why Ksp calculations often start with the idea of a saturated solution.

## Related Study Guides

- [5.1 Solubility product constant (Ksp) and molar solubility](/general-chemistry-ii/unit-5/solubility-product-constant-ksp-molar-solubility/study-guide/73dkXCWLy5QxcAB8)

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