Mixtures, Solution Concentrations, Osmosis and Dialysis

Chapter 8

Homogenous Mixture

Evenly distributed throughout the mixture

• orange juice with no pulp

Heterogenous Mixture

Unevenly distributed throughout the mixture

• orange juice with pulp

Solution

A homogenous Mixture of two or more substances

• Tin in copper is a solution called bronze

• Alloys are solutions

Solvent

the element that dissolves the Solute

What are 3 examples that solutes can be

1. molecules uncharged (sugar in H2O)

2. Charged ions (salt in water). Ions in solutions often referred to as electrolytes

3. A gas (fizzy water or O2 and CO2 dissolved in out blood)

Solutes

The minor component in a solution that is applied to the solvent to dissolve

Isomerism Reactions

A chemical reaction that converts one geometric isomer into another isomer

Physical properties of Hydrocarbons

Non-polar, low boiling pts, (only dispersion forces), low density

Hydrophilic

Mix with, dissolve in, or wetted by water

Hydrophodic

repel water

Colloids

Homogenous solutions that contain large solutes that dissolve from 100-1000 nm. Often in the form of “aggregates”

• also called colloids Dispersion

• examples: mayo and protein

Suspension

heterogeneous mixtures containing large particles. - larger than 1000nm (71um)

• Ex; med, particulates in paint, blood cells and medicine

How do you find the concentration of a solution

Mass (solutes in mg)/volume (solvent in mL)

what does mass / volume mean?

amount of solute/amount of solvent

• Parts per million (ppm) = which is mg/L (100mg in 1L is 100ppm)

What are units of concentration

• % mass/ volume

• Mass(mg solute)/ Volume (solvent in mL)

• Equivalents/liter (eq/L)

• Molarity

% mass/ volume

in units of g/mL * 100. AN IV solution contains 100mg NaCl in 100mL

• ex:0.1g/10mL * 100 = 1.0% NaCl Solution

Equivalents / liter (eq/L)

Equivalents = moles of an ion * its charge

• Find the moles of an ion and multiply them by the charge

• Ex: 1 mol of MgCl2 is Mg+2 in a liter of H2O = 1 mole 2+ = 2 equivalents, for Cl-= 2 mols * 1-= 2eq

Molarity

Most commonly used to describe concentration

moles solute/ volume solvent

Membranes

Semi-permeable simple diffusion, Osmosis, and Dialysis and cell membrane

Semi-permeable membranes

a membrane that lasts somethings through, but not others. Most cell membranes

simple diffusion

The spontaneous movement of a molecule or ion from a region of high to low concentration

• eventually concentration reach an equilibrium

What does simple diffusion do?

this diffusion delivers nutrients and removes waste in/out of cells across semi-permeable membranes

Osmosis

If solvent flows through the membrane

• Governed by # of particles

Dialysis

Solutes moving crosses membranes and separates small particles from large ones (colloids/suspension)

Hypertonic

solutions with high soluble concentration

hypotonic

solutions with lower soluble concentration

Isotonic

the solutions and soluble the same

Reverse Osmosis

Drives solutes from low to high concentration

• hypotonic to hypertonic

Osmosis Pressure

putting pressure on the system to prevent inward flow

Hemolysis

Given a distilled “pure” water as a IV, a;; their cells would burst due to Osmosis of water into a cell

Crenation

Hypertonic IV solution

Why is dialysis useful

because small solutes can pass through membranes, but colloidal particles cannot

How does diaylsis work chemically

The Solute tries to equilibrate itself, so you put the Solute you want in the tube of the diaylsis solution