Notes, summaries, assignments, exams, and problems for Chemistry

Demineralization of Brackish Water by Electrodialysis

This detailed explanation covers the process of demineralization of brackish water using Electrodialysis (ED), based on standard water chemistry concepts.

Brackish Water Characteristics

Brackish water contains dissolved salts, with salinity levels higher than freshwater but lower than seawater. It tastes salty and is generally unsuitable for drinking or industrial use. To make it potable, salts must be removed (desalination).

Electrodialysis Principle

Electrodialysis is an electrochemical desalination process. When an electric field is applied, ions (salts) in the water migrate through specialized ion-selective membranes:

• Cation-exchange membranes: Allow only cations (e.g., Na⁺, Ca²⁺, Mg²⁺)

Essential Chemistry Definitions

Fundamental Concepts

• Physical Property: Characteristics observed without changing the substance (color, melting point, density, boiling point).
• Chemical Property: Characteristics observed when a substance changes into another (reactivity with air, acid, base, water, other chemicals).
• Law of Conservation of Matter: Matter is neither created nor destroyed.
• Atomic Theory: Theory of the nature of atoms.
• Isotope: Atoms of the same element with different numbers of neutrons.
• Ion: Atom or molecule with a net electric charge.
• Cation: Positively charged ion.
• Anion: Negatively charged ion.
• Atomic Mass Unit (amu): Unit of mass for expressing atomic & molecular weights.
• Mole: Unit for amount of substance (6.022 x 10^23 particles)

Material Structure and Properties

Inter-Atomic Bonding

Different materials are made up of different types of bonds. The following are examples and characteristics of the chemical bonds that make up materials.

• Ionic Bonding
  

  Ionic bonding in NaCl. Callister, W. D., & Rethwisch, D. G. (2018). Materials Science and Engineering: An Introduction.

  • Description: Found in compounds composed of metallic and nonmetallic elements; involves atoms at the extremes of the periodic table.
  • Process: Metallic atoms give up their valence electrons to nonmetallic atoms; atoms achieve stable inert gas configurations (filled orbital shells) and acquire electrical charges (become ions).
  • Example: Sodium chloride (NaCl) is a classic ionic material; a sodium atom transfers

1. Phases of Pure Substances

• Solid: Molecules are closely packed and vibrate in place due to strong intermolecular forces.
• Liquid: Molecules are closer together but remain free to move with weaker intermolecular forces.
• Vapor: Molecules are far apart and possess very high kinetic energy.

2. Phase Change Processes

• Compressed Liquid: A liquid that is not about to vaporize (e.g., water at 20°C and 1 atm).
• Saturated Liquid: A liquid that is about to vaporize (e.g., water at 100°C and 1 atm).
• Saturated Vapor: Vapor that is about to condense (e.g., steam at 100°C and 1 atm).
• Superheated Vapor: Vapor that is far from condensing (e.g., steam at 150°C and 1 atm).

3. Latent Heat

• Latent Heat of Fusion: The energy required to change 1 kg of solid into liquid.

The Law of Conservation of Mass

Matter cannot be created or destroyed. The number of atoms in the reactants must be the same as the products. Atoms don't appear or disappear, they just rearrange. (Hence why you have to balance out chemical equations)

Balancing Equations

• The subscripts in the chemical formula cannot be changed (The little number beside a formula that is part of it).
• Use coefficients to balance.
• Coefficients multiply the entire compound by that number (4PO = 4P 4O).

Example: N₂+O₂>N₂O = 2N₂+O₂>2N₂O

Balancing Word Equations

• Determine what the reactants and the products are, convert names to chemical formulas. (Individual elements that are diatomic (molecular) will be, S₈, P₄, I₂, Br₂, Cl₂, F₂, O₂, N₂, H₂) If it's not diatomic just

Classifying Matter

• Pure Substance: Element or compound.
• Mixture: Homogeneous (uniform) or heterogeneous (non-uniform).
• Element: One type of atom.
• Compound: Two or more atoms chemically bonded.

Properties of Matter

• Physical: Observable without changing the substance (e.g., color, density).
• Chemical: Describes the potential for a substance to change (e.g., reactivity).
• Physical Change: No new substance is formed (e.g., melting).
• Chemical Change: A new substance is formed (e.g., burning).

Atomic Structure

Protons, Neutrons, Electrons (PEN)

• Protons: Positive charge (+1), located in the nucleus.
• Neutrons: No charge (0), located in the nucleus.
• Electrons: Negative charge (-1), located in shells around the nucleus.
• PEN Relationships:
  • Protons = Atomic number.
  • Neutrons

Spaghetti Carbonara

Utensils and Ingredients

Utensils

• Large pot
• Large skillet
• Colander
• Large bowl
• Whisk or fork
• Tongs or a pasta fork
• Spoon or ladle

Ingredients:

• 400g spaghetti
• 200g pancetta or bacon, diced
• 4 large eggs
• 1 cup grated Parmesan cheese
• 4 cloves garlic, minced
• Salt and black pepper to taste
• 2 tablespoons olive oil
• Chopped parsley for garnish (optional)

Instructions

1.

Boil the Spaghetti

Start by boiling a large pot of salted water. While waiting, dice the pancetta, mince the garlic, and grate the Parmesan cheese.

2.

Cook the Spaghetti

Once the water boils, add the spaghetti and cook until al dente. Once cooked, reserve about a cup of pasta water before draining.

3.

Sauté the Pancetta and Garlic

In a large skillet, heat the olive oil over medium heat. Add... Continue reading "Classic Spaghetti Carbonara Recipe" »

Le Chatelier's Principle and Equilibrium

The forward reaction is exothermic, while the reverse reaction is endothermic (depending on the specific system). According to Le Chatelier's Principle, increasing the temperature favors the endothermic reaction. In this scenario, the forward reaction is favored, and the equilibrium moves from left to right, producing more CO. Therefore, high temperature is more favorable for the production of CO.

Regarding pressure, increasing pressure favors the side with fewer moles, while decreasing pressure favors the side with more moles.

Factors Influencing Reaction Rates

A chemical reaction will speed up if the frequency of the reacting particles increases and the proportion of the particles with energy greater than... Continue reading "Chemical Equilibrium and Reaction Rate Factors" »

Principle of Chromatography - Chromatography is a separation method where the analyte is combined within a liquid or gaseous mobile phase, which is pumped through a stationary phase. Usually, one phase is hydrophilic and one is lipophilic. The components of the analyte interact differently with these two phases. Depending on their polarity, they spend more or less time interacting with the stationary phase. This leads to the separation of different components present in the sample. Each sample component elutes from the stationary phase at a specific time called retention time.

Types of Chromatography

1. Liquid Chromatography - This type of chromatography is used to separate and analyze non-volatile compounds. In this technique, the sample is dissolved

Lowry Protein Estimation Protocol

Aim

To estimate the protein using Lowry’s method.

Principle

The –CO-NH– bond (peptide bond) in the polypeptide chain reacts with copper sulphate in an alkaline medium to produce a blue-colored complex. Additionally, tyrosine and tryptophan residues of the protein reduce the phosphomolybdate and phosphotungstate components of the Folin-Ciocalteau reagent, yielding bluish products that enhance the sensitivity of this method.

Reagents Required

• Reagent A: 2% sodium carbonate in 0.1 N sodium hydroxide.
• Reagent B: 0.5% copper sulphate (CuSO₄·5H₂O) in 1% potassium sodium tartarate. Prepare fresh by mixing stock solutions.
• Alkaline Copper Solution (Reagent C): Mix 50 mL of Reagent A and 1 mL of Reagent B prior to use.