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Questions and Answers
What is the unit of molality?
What is the unit of molality?
Why is molality not temperature-dependent?
Why is molality not temperature-dependent?
What is the equivalent weight of H2SO4?
What is the equivalent weight of H2SO4?
What is the concentration of a solution that contains 20.0 grams of NaCl in 800.0 grams of solution?
What is the concentration of a solution that contains 20.0 grams of NaCl in 800.0 grams of solution?
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What is the normality of a 3 M H2SO4 solution?
What is the normality of a 3 M H2SO4 solution?
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What is the percentage of a solution that contains 1 ml of HCl in 100 ml of solution?
What is the percentage of a solution that contains 1 ml of HCl in 100 ml of solution?
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How many grams of NaCl are in 200.0 grams of solution that is 15.0% NaCl by mass?
How many grams of NaCl are in 200.0 grams of solution that is 15.0% NaCl by mass?
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What is the molarity of a solution that contains 4% NaOH by mass?
What is the molarity of a solution that contains 4% NaOH by mass?
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How many grams of NaOH would be required to react with 1.50 L of 3.75M sulfuric acid?
How many grams of NaOH would be required to react with 1.50 L of 3.75M sulfuric acid?
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What is the normality of a 9.8% H2SO4 solution?
What is the normality of a 9.8% H2SO4 solution?
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Study Notes
Mixtures
- A mixture is a combination of two or more substances that do not combine chemically, but remain the same individual substances and can be separated by physical means.
- There are two types of mixtures: heterogeneous and homogeneous.
Heterogeneous Mixture
- A heterogeneous mixture is a mixture in which the composition is not uniform throughout the mixture.
- It consists of visibly different substances or phases (solid, liquid, gas).
- Examples: sand in water, oil and water.
Homogeneous Mixture
- A homogeneous mixture is a mixture in which the composition is uniform throughout the mixture.
- It has a uniform appearance and maintains one phase (solid, liquid, gas).
- Examples: salt water, sugar syrup.
- All solutions are mixtures, but not all mixtures are solutions.
Solution
- A solution is a homogeneous mixture of two or more substances whose particle size ranges between 0.1nm to 1nm.
- Examples: soda water, sugar syrup, salt solution.
Components of Solution
- Solute: the substance which is being dissolved.
- Solvent: the component of a solution in which the solute is being dissolved.
- Solute is the minor component in a solution, dissolved in the solvent.
Types of Solutions
- Gaseous solutions: air = Oxygen + Nitrogen.
- Liquid solutions: drinks = mix + water.
- Solid solutions: alloys = steel, brass, etc.
Properties of Solution
- It is a homogeneous mixture.
- Its particles are too tiny and have a diameter of less than 1 nm.
- The particles are not visible to the naked eye.
- Particles don’t scatter a beam of light passing through it and hence the path of the light is not visible.
- Solutes are inseparable from the mixture and do not sediment.
- A solution is stable.
- The components of a mixture cannot be separated using filtration.
Concentration
- The amount of solute dissolved in a solvent at a given temperature.
- Dilute solution: has a low concentration of solute dissolved.
- Concentrated solution: has a high concentration of solute dissolved.
Saturation
- Unsaturated: has less than the maximum concentration of solute dissolved.
- Saturated: has the maximum concentration of solute dissolved (can see solid in the bottom of the solution).
- Supersaturated: contains more dissolved solute than normally possible (usually requires an increase in temperature followed by cooling).
Solubility
- The amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution.
Factors Affecting Solubility of Solids
- Temperature: increased temperature causes solids to dissolve faster.
- Particle Size: smaller particles dissolve faster because they have more surface area.
- Vibration (agitation): shaking or agitation causes solids to dissolve faster.
Solubility Curves
- Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
- A point on the line is a saturated solution.
- Above the line is supersaturated.
- Below the line is unsaturated.
Mole
- According to the International System of Units (SI), a mole is defined as exactly 6.02214076 × 10²³ particles, which may be atoms, molecules, ions, or electrons.
- Example: 1 mole H2O = 6.022 × 10²³ H2O (water) molecules.
Mass and Mole
- The mass of one mole of a substance is equal to that substance's molecular weight.
- Example: Mass of water: 18.01528 g/mol.
Molarity (m)
- The number of moles of solute per liter of solution.
- M = moles of solute / liters of solution.
Dilutions and Molarity
- Use the formula: Molarity1 x Volume1 = Molarity2 x Volume2.
- Example: How many liters of 2.5 M HCl are required to make 1.5 L of 1.0 M HCl?
Molality (M)
- The number of moles of solute per kilogram of solvent.
- M = moles of solute / kilograms of solvent.
Normality
- The number of mole equivalents per liter of solution.
- Normality = number of mole equivalents / 1 L of solution.
- Equivalent weight or Mole equivalent = Molar mass / Valence factor.
Percent Solution
- v/v (volume per volume): 100 ml, 99 ml water + 1 ml HCl = 1% HCl v/v.
- w/v (weight per volume): 100 ml water, 2 gm NaCl = 2 % NaCl w/v.
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Description
Learn about the different types of mixtures, including heterogeneous and homogeneous mixtures, and how they can be separated by physical means.
