Edited Invalid date
14.7 Colligative Properties of Strong Electrolyte -- Part 1
The osmotic pressures must be equal to those of body fluids.
When a patient is given an IV in a hospital, the majority of the fluid is usually an isosmotic saline solution.
In medicine and other health-related fields, solution concentrations are reported in units that show the mass of the solute per volume of solution.
The mass of the solute in grams is divided by the volume of the solution.
The concentration of an isotonic saline solution is 0.9% in these units.
The fluids used for transfusion must have the same osmotic pressure as body fluids.
The mixture of water and soap has a distinctive haze.
Some examples of colloids include fog, smoke, whipped cream, and milk.
The size of the particles in the mixture determines whether or not it is a colloid.
The mixture is a solution if the particles are small.
The mixture is a heterogeneous mixture if the particles have a diameter greater than 1mm.
Sand slowly leaves the water.
The small particles stay dispersed throughout the medium because of their small size.
The Soapy water is an example of a Brownian motion, which is caused by the collision of molecules in the liquid.
The haze is due to the beginning of the twentieth century, Brownian motion was a decisive factor in confirm scattering of light.
One end of the molecule interacts with water through ion-dipole interactions.
The soap molecule has a long tail.
The nonpolar hydrocarbon tails crowd into the center of the sphere to maximize their interactions with one another.
The haze seen in soapy water is caused by the micelle structures, which are too small to be seen by the naked eye, but still scatter light.
A soap and the ionic heads can interact with the hydrocarbon tail.
The colloid particles scatter the light when it passes through a suspension.
The beam wouldn't be visible in pure water or a noncolloidal solution.
The Tyndall effect can be observed in fog or dusty air.
The Tyndall effect can be used to determine whether a mixture is a solution or a colloid, since solutions are too small to scatter light.
Stable micelles are kept by the repulsions that occur at their surfaces.
The soap molecule's ionic heads form the surface of the spherical particle.
The ionic heads repel colloid particles but interact with water.
Light beams are invisible when posed of micelles because they are not scattered by particles such as dust and allow the molecule within the micelles to mist in.
Adding an electrolyte to a suspension of micelles can cause the repulsion of particles to destroy the colloid.
The reason soap doesn't work in a saltwater solution is because of this.
There are particles in a colloid.
Many colloids contain dispersed macromolecules.
A solution containing hemoglobin is a colloid.
The large molecule of hemoglobin scatters light.
The charged surface of one micelle repels the charged surface of another.
At room temperature, the solution is saturated in both carbon dioxide gas and potassium chlorate.
A sample of pure water is allowed to come to an unknown molecule in 50.0 liters of solution.
Determine the mass of the molecule.
The solution for NaOH has an enthalpy of -44.46 kJ/mol.
Nothing can be concluded about the 6H12O6 dissolved in 0.500 L of water.
Pure A has a Vapor Pressure of 1.44 M b, and pure B has a Vapor Pressure of 100 torr.
The pressure of the mixture is 85 torr.
Determine the vapor pressure between particles of A and B, relative to the solution of C2H6O2 that is 14.8 % C2H6O2 by mass.
The intermolecular forces between particles A and B are volatile.
The vapor pressure of pure A is 87mmHg, and between particles of B.
An equal number of moles of oxygen, nitrogen, and helium are present in the solution at 25 degC.
Determine the relative concentrations of each gas in the solution.
A solution is a mixture of two or more substances.
The tendency toward greater energy dispersal is the driving force for solution formation.
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