September 1, 20XX
The colorful landscape and the Mushroom Castle in the background created an enchanting atmosphere. Princess Peach, with her gentle smile and grace, introduced me to the group of heroes who had gathered in the courtyard.
First, there was Little Mac, the boxing champion. He stood tall and proud, wearing his trademark green boxing gloves. He radiated confidence and determination.
Next was Captain N, who looked like he had stepped right out of a retro video game. With his iconic red jacket and Zapper in hand, he brought a nostalgic vibe to the gathering.
Ash and Pikachu, were an electrifying duo. Ash, a determined Pokémon Trainer, and Pikachu, his loyal partner, greeted me with a friendly wave and a cheerful statement, "Pika Pika!" It was surreal to hear this voice often.
Donkey Kong, the giant ape with a heart of gold, made a grand entrance. He thumped his chest and let out a boisterous roar, which was quickly followed by a warm and inviting smile. His playful nature and love for bananas were instantly endearing.
Link, the legendary Hero of Hyrule, was a sight to behold. Dressed in his green tunic and carrying the Master Sword, he exuded an aura of bravery and wisdom. I couldn't help but feel a sense of awe in his presence.
Ness, the psychic boy from Onett, was quiet and introspective. He greeted me with a nod and a faint smile, giving off an air of mystery. His psychic powers were no less intriguing in person.
Last but not least, there was Kirby, the adorable pink puffball. With his round, smiling face and ability to inhale just about anything, Kirby brought a sense of lightheartedness to the group. He even waved his stubby arms enthusiastically, trying to mimic the others.
Throughout the day, I had the opportunity to chat with each of these iconic heroes who fight against recent villains I often hear about, sharing stories and experiences from their respective journeys.
As the day came to a close, Princess Peach and Mario expressed their gratitude for my presence and hoped I had enjoyed my time with their extraordinary friends.
Chem Notes: (filled with academic musings)
Solubility Terminology
• When one substance (solute) dissolves in another (solvent), it is said to be soluble.
• Salt is soluble in water.
• When one substance does not dissolve in another, it is said to be insoluble.
• Oil is insoluble in water.
• The maximum amount of solute that can be dissolved in a given amount of solvent is called the solubility. (e.g. Salt solubility in water is 359 g/L)
• There usually is a limit to the solubility of one substance in another.
• Gases are always soluble in each other.
• Two liquids that are mutually soluble are said to be miscible.
• Alcohol and water are miscible.
• Oil and water are immiscible.
• The solubility of one substance in another varies with temperature and pressure.
Solubility Limit
• A solution that has the solute and solvent in dynamic equilibrium is said to be saturated.
• If you add more solute, it will not dissolve.
• The saturation concentration depends on the temperature and pressure of gases.
• A solution that has less solute than saturation is said to be unsaturated.
• More solute will dissolve at this temperature.
• A solution that has more solute than saturation is said to be supersaturated.
Temperature Dependence of Solubility of Solids in Water
• Solubility is generally given in grams of solute that will dissolve in 100 g of water.
• For most solids, the solubility of the solid increases as the temperature increases.
• When ΔHsolution is endothermic
Temperature Dependence of Solubility of Gases in Water
• Gases have lower solubility in water than ionic or polar covalent solids because most are nonpolar molecules or atoms (e.g. He)
• For all gases, the solubility of the gas decreases as the temperature increases.
• The ΔHsolution is exothermic because you do not need to overcome solute–solute attractions.
The solubility of one substance in another depends on the following
1. The types of intermolecular attractive forces
2. Nature's tendency toward mixing
The solubility of one substance in another depends on the following
Energy changes in the formation of most solutions involve differences in attractive forces between the particles.
Highly Important:
1. The types of intermolecular attractive forces
2. Nature's tendency toward mixing
The solubility of one substance in another depends on the following
• The gases mix because the energy of the system is lowered through the release of entropy.
• Entropy is the measure of energy dispersal throughout the system.
• Energy has a spontaneous drive to spread out over as large a volume as it is allowed.
• As each gas expands to fill the container, it spreads its energy out and increases its entropy.
Energy Changes and the Solution Process
There is an entropy change for the solution process
Spontaneous: −ΔG
Nonspontaneous: + ΔG
Endothermic: + ΔH
Exothermic: −ΔH
Solution Concentrations
• Solutions have changing composition. To describe a solution, you need to describe the components and their relative amounts.
Concentration = amount of solute in a given amount of solution.
• The terms dilute and concentrated can be used as qualitative descriptions of the amount of solute in solution.
*Dilute = small amount, concentrated = large amount
Molarity, M
• Molarity (M or mol/L) is defined as the moles of solute per 1 liter of solution.
• Molarity describes how many molecules or atoms of solute are in each liter of solution.
• If a sugar solution concentration is 2.0 M,
• then 1 L of solution contains 2.0 mol of sugar; or
• 2 L = 4.0 mol sugar; or
• 0.5 L = 1.0 mol sugar.
Molality, m
• Molality (m or mol/kg) is defined as the moles of solute per 1 kilogram of solvent.
• Molality (m) is defined in terms of amount of solvent, not solution.
• It does not vary with temperature because it is based on masses, not volumes.
Parts Solute in Parts Solution
Parts can be measured by mass or volume.
• Parts are generally measured in the same units.
• By mass in grams, kilograms, pounds (lb), etc.
• By volume in mL, L, gallons (gal), etc.
• Percentage = parts of solute in every 100 parts solution.
• If a solution is 0.9% by mass, then there are 0.9 g of solute in every 100 g of solution (or 0.9 kg solute in every 100 kg solution).
• Parts per million = parts of solute in every 1 million parts solution.
• If a solution is 36 ppm by volume, then there are 36 mL of solute in 1 million mL of solution.
Mole Fraction, χa
• A mole fraction is the fraction of the moles of one component in the total moles of all the components
of the solution.
• Total of all the mole fractions in a solution = 1.
χa = moles of substance a / moles of substance a + moles of substance b
• Mole fraction has no units.
• The mole percentage is the percentage of the moles of one component in the total moles of all the components of the solution.
mol % = mole fraction (χa) × 100%
Dynamic Equilibrium of Liquids
• In a closed container, once the rates of vaporization and condensation are equal, the total amount of vapor and liquid will not change.
The pressure exerted by the vapor when it is in dynamic equilibrium with its liquid is called the vapor pressure.
Vapor Pressure versus Temperature
• When the temperature of a liquid reaches a point where its vapor pressure is the same as the external pressure, vapor bubbles can form anywhere in the liquid, not just on the surface. (boiling point)
• Increasing the temperature increases the number of molecules able to escape the liquid.
• The net result is that as the temperature increases, the vapor pressure increases.