Supersaturation in crystallization
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This document discusses supersaturation and solubility. It defines key terms like solubility, saturated solutions, and supersaturated solutions. Supersaturation occurs when the concentration of a solute is higher than the solubility limit. This drives crystallization. The document presents different ways to express the level of supersaturation, like concentration driving force and relative supersaturation. It provides an example calculation for sucrose in water. Finally, it notes that concentration units like g/kg solution can impact supersaturation values.
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The document discusses solutions and their properties. It begins by defining key terms like solute, solvent, and solution. It then describes different types of solutions such as true solutions, colloidal solutions, and suspensions based on particle size. Other classifications covered include aqueous vs non-aqueous solutions and saturated, unsaturated, and supersaturated solutions based on amount of solute. Factors that affect solubility like temperature, nature of solute and solvent, and pressure are also summarized. Examples are provided throughout to illustrate different solution types and concepts.
Solutions Powerpoint
This document defines key terms related to solutions and summarizes factors that affect solubility. It defines a solution as a homogeneous mixture where a solute is dissolved in a solvent. Temperature, pressure, and the nature of the solute and solvent affect solubility. There are various units to express concentration, including molarity, molality, and percent composition. Colligative properties like boiling point elevation and freezing point depression depend on the number of solute particles rather than their identity.
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This document provides an overview of colligative properties and solutions. It begins with definitions of colligative properties, noting that they depend on the number of solute particles rather than their identity. Examples of colligative properties are given as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The document then discusses each of these properties in more detail. Specific topics covered include how colligative properties are calculated using molality or molarity, data like freezing point depression constants for various solvents, and sample problems calculating values like boiling/freezing points of solutions. The last few pages shift to discussing colloids, providing definitions and examples of different types of colloids.
Properties of pure substances
Pure substances can exist in different phases including solid, liquid, and gas. They have a fixed chemical composition throughout. Phase changes between these states are associated with the absorption or release of latent heat. The properties of a pure substance, such as pressure, temperature, specific volume, and enthalpy are interrelated. Graphs of these properties, such as pressure-volume and temperature-entropy diagrams, can be used to determine the phase and properties of a pure substance at given conditions. Common phase change processes include vaporization, condensation, melting, and sublimation.
Evaporation
The document discusses evaporation in the sugar industry. It explains that evaporation is used to concentrate sugarcane juice by boiling off water in a series of connected evaporator vessels under decreasing pressure. This produces a thick juice containing around 60% sugar that is then crystallized to produce sugar. The process of evaporation increases the boiling point of the sugarcane solution compared to water alone. Various factors that affect evaporation like concentration, foaming, temperature sensitivity, and scale formation are also discussed.
MUCLecture_2023_1123221.pptx
This document discusses various concepts related to crystallization including:
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Mass transfer equipment
Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
Section: Distillation
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project.
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project.
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project.
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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This document discusses convective mass transfer and mass transfer coefficients. It defines convective mass transfer as the rapid transfer of mass that occurs when there is motion in the transfer medium compared to the slower process of molecular diffusion. Mass transfer coefficients are introduced to simplify calculations of mass transfer rates. Different types of mass transfer coefficients are presented based on whether they are used for gases or liquids, and whether they are expressed in terms of concentrations, mole fractions, or partial pressures. Approximations for typical values of mass transfer coefficients in gas and liquid phases are provided.
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This document discusses various types of equipment used for mass transfer operations in industry. It describes plate columns and packed columns as the two most widely used for distillation, gas absorption, and stripping. Plate columns are also known as tray columns, where the column is divided into stages by trays. The main types of trays are sieve, bubble-cap, and valve trays. Packed columns can use random, structured, or grid packings. Other equipment discussed include bubble columns, spray columns, and agitated vessels. Selection of mass transfer equipment depends on the process conditions and economics.
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Molecular diffusion
Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Overview of mass transfer mechanisms
Slides for the eLearning course Separation and purification processes in biorefineries (https://open-learn.xamk.fi) in IMPRESS project (https://www.spire2030.eu/impress).
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Supersaturation in crystallization
- 1. This project has received funding from the European Union’s Horizon 2020 research and innovation programme under grant agreement No 869993. Supersaturation
- 2. Solubility curves • Solubility defines the concentration of a solution in which it is saturated. • Saturated solution is at equilibrium. • Solubility usually varies with the temperature. Most substances are more soluble at higher temperatures, but there are some exceptions, for example HCl and NH3. • Solubilities can be expressed in solubility curves. • The temperature is on the x-axis and y-axis indicates the amount of the solute dissolved in 100 grams of solvent. Solubility curves for several compounds. (CK-12 Foundation,Christopher Auyeung)
- 3. Solubility of sugars and sugar alcohols in water
- 4. Levels of supersaturation • When the solution contains more than the maximum amount of the solute, it is called a supersaturated solution. • Supersaturated solution is not at equilibrium. • When the level of supersaturation is lightly increased, the solution gets metastable. • If the cooling is proceeded, the solution achieves the supersaturation limit and becomes unstable.
- 5. Driving force • Supersaturation is a driving force for crystallization. • Spontaneous nucleation may only occur above the supersaturation limit. • In industrial crystallization, nucleation is usually initiated by crystal seeds at the metastable zone. That is where the crystal growth also appears. • Crystallization may continue to the saturation curve at the most.
- 6. Expressions of supersaturation • There are several ways to express the level of supersaturation. The most commonly used are: Concentration driving force ∆𝑐 = 𝑐 − 𝑐∗ Supersaturation ratio S = 𝑐 𝑐∗ Relative supersaturation 𝜎 = ∆𝑐 𝑐∗ = 𝑆 − 1 It is essential to mention the temperature, because solubility is temperature dependent. c = solution concentration c* = concentration of the saturated solution at the given temperature
- 7. Example: Level of supersaturation • Solubility of sucrose in water is 2040 g/kg of water at 20 °C. Let c = 2450 g/kg. Concentration driving force ∆𝑐 = 𝑐 − 𝑐∗ = 2450 g kg − 2040 g kg = 410 g kg Supersaturation ratio S = 𝑐 𝑐∗ = 2450 g/kg 2040 g/kg ≈ 1.20 Relative supersaturation 𝜎 = ∆𝑐 𝑐∗ = 410 g/kg 2040 g/kg ≈ 0.20 Alternative calculation 𝜎 = 𝑆 − 1 = 1.20 − 1 = 0.20
- 8. Different units of concentration • It is essential to take into consideration the units of concentration used. They affect the obtained values as shown in the table below. • Let’s use the same values asc in the previous example (sucrose in water at 20 °C, c* = 2040 g/kg and c = 2450 g/kg). Molar mass of sucrose M ≈ 342 g/mol. Solution densities ρc* = 1330 kg/m3 and ρc = 1360 kg/m3. Solution composition c c* Δc S σ g/kg water 2450 2040 410 1.20 0.20 g/kg solution 710 671 39 1.06 0.06 g/l solution 966 893 73 1.08 0.08 mol/l solution 2.82 2.61 0.21 1.08 0.08 mole fraction 0.114 0.097 0.017 1.18 0.18
- 9. This project has received funding from the European Union’s Horizon 2020 research and innovation programme under grant agreement No 869993. References Mullin, J. W. 2001. Crystallization. Oxford: Elsevier Science & Technology. pp. 123-130. Myerson, A. S. (ed.) 2002. Handbook of Industrial Crystallization. Elsevier Inc. pp. 14-18. Videos: • Solubility vs concentration: https://youtu.be/cHBlDVg9nR8 • Saturated, unsaturated, supersaturated: https://youtu.be/s6KcCgnMnhA • Solubility curves: https://youtu.be/VKmyj1z8T8U