Solutions The homogeneous mixture of a solute dissolved
- Slides: 49
Solutions
The homogeneous mixture of a solute dissolved in a solvent is called a “solution”.
The “solute” is the substance being dissolved. ex. Na. Cl in Na. Cl(aq)
The solute is often a solid, but it doesn’t have to be. Solutes can be gases or even liquids. ex. NH 3 in NH 3(aq)
The “solvent” is the liquid that is dissolving the solute. ex. water in Na. Cl(aq)
“Concentration” expresses how “strong” or “weak” a solution is.
If a “small” amount of solute is dissolved in a “large” amount of solvent, the solution is considered weak or “dilute”.
If a “large” amount of solute is dissolved in a “small” amount of solvent, the solution is considered strong or “concentrated”.
A “saturated solution” contains the maximum amount of solute that can dissolve in the solvent.
Another way of saying this is a solution is saturated when the maximum concentration is reached.
If more of a substance is added to a saturated solution, it can NOT dissolve.
“Precipitate” is the solid substance that settles to the bottom of a saturated solution and does NOT dissolve.
There are 3 factors that determine how well a solute will dissolve in a solvent.
Factor #1 What is the solute and how much of it are you trying to dissolve?
Factor #2 What is the solvent and how much of it are you dissolving the solute in?
Factor #3 What is the temperature of the solute?
In general, solid solutes dissolve better when the temperature of the liquid solvent is higher.
In general, gaseous solutes dissolve better when the temperature of the liquid solvent is lower.
When answering questions about solubility and temperature, always refer to Table G!
Another important factor affecting solubility is the polarity of the solute and the polarity of the solvent.
In general, ionic substances dissolve better in polar liquids like water because of the molecule-ion attractions that occur.
In general, polar molecules dissolve better in polar liquids such as water.
In general, non-polar molecules dissolve better in non-polar liquids such as oil.
“Likes Dissolve Likes!”
Predict the solubility in water or oil: NH 3 I 2 gasoline KMn. O 4 CH 4 HCl KBr sugar CO 2
In most double replacement reactions in solution, one of the products formed will be a precipitate.
Remember to use Table F to determine if a precipitate will form!
In general: Solids dissolve better at a higher temperature. Gases dissolve better at a lower temperature.
Pressure only has a significant effect on the solubility of gases. Solids and liquids are Not affected by pressure changes.
Gases dissolve better at high pressure. Gases don’t dissolve as well at low pressure.
Properties of Solutions
Chemists often use “Molarity” to express the concentration of a solution “quantitatively” (with numbers).
Molarity (M) = moles of solute liters of solution (Molarity is measured in moles/liter and can be found on Table T) Also helpful Moles = grams GFM (g/mole)
‘ppm’ (parts per million) is a term that is also used to express a concentration
The equation: ppm= grams of solute grams of solution This can also be found on Table T
% mass of a compound in solution is sometimes referred to as pph - parts per hundred
Any dissolved substance will lower the freezing point and raise the boiling point of a solvent.
The greater the concentration of dissolved particles is, the greater the effect will be.
freezing point boiling point O o. C more dissolved particles 100 o. C pure water more dissolved particles
Each mole of dissolved particles in 1000 g of water will lower the o freezing point by 1. 86 C.
Each mole of dissolved particles in 1000 g of water will raise the boiling point by 0. 52 o. C.
“Electrolytes” are substances that ionize (form charged particles) and conduct electricity when they are dissolved in water.
In general, ionic solutes (electrolytes) effect freezing and boiling points greater than covalent solutes (nonelectrolytes) do. Why?
Nonelectrolytes NH 3(aq) (1 mole produces 1 mole) C 6 H 12 O 6(aq) (1 mole produces 1 mole)
Electrolytes Na. Cl Na+(aq) + Cl-(aq) (1 mole produces 2 moles!) Ca. Cl 2 Ca+2(aq) + 2 Cl-(aq) (1 mole produces 3 moles!)
Vapor pressure - pressure exerted by molecules of a liquid as it evaporates
Boiling occurs when: vapor pressure = atmospheric (air) pressure
Always refer to Table H when answering questions about vapor pressure and boiling point!
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