Saturated and Supersaturated Solutions
Saturated and supersaturated solutions represent crucial concepts in the field of chemistry, particularly in understanding solubility and phase transitions. In a saturated solution, the solvent holds the maximum amount of solute at a given temperature, leading to equilibrium between dissolved and undissolved particles. On the other hand, supersaturated solutions contain more dissolved solute than theoretically possible under normal conditions, achieved through carefully controlled processes. These solutions are characterized by their instability and propensity to crystallize or precipitate out excess solute. Understanding the properties and behaviors of saturated and supersaturated solutions is fundamental to various industrial and scientific applications.
- How can you determine if the solutions made in a lab were saturated?
- How does pressure affect a saturated solution?
- How do you calculate the pH of a saturated solution?
- The solubility of #KNO_3# is 155 g per 100 g of water at 75° Cand 38.0 g at 25°C. What mass (in grams) of #KNO_3# will crystallize out of solution if exactly 100.0 g of its saturated solution at 75° C is cooled to 25°C?
- How to make a saturated solution of sodium chloride?
- What happens to a saturated solution of sugar in water when the temperature of the solution is suddenly lowered by 10°C?
- How can I calculate the molarity of a saturated solution?
- If #541*g# of calcium is reacted with water to give a #1*L# volume of solution, what is #[Ca^(2+)]#?
- A saturated solution of potassium chloride at #60# #""^@C#, is cooled to #20# #""^@C#. What happens, and how do we describe the solutions?
- Why is a saturated salt solution at equilibrium?
- Will a solution made by adding 9,0 g #NH_4Cl# to 20 g of #H_2O# be saturated or unsaturated at 50 degrees C?
- When does the air become saturated?
- A seed crystal was placed in a super-saturated solution. When crystals of solute formed, the resulting process was exothermic (felt warm). Why?
- How many total moles of #KNO_3# must be dissolved in water to make 1.5 liters of a 2.0 M solution?
- How does the amount of gas in a saturated solution change with pressure?
- What is an example of a saturation practice problem?
- How can you identify a saturated solution?
- Why are supersaturated solutions unstable?
- A mass of 80 g of #KNO_3# is dissolved in 100 g of water at 50°C. The solution is heated to 70°C. How many more grams of potassium nitrate must be added to make the solution saturated?
- How are supersaturated solutions prepared?