States of Matter Jun Ruan Solid Molecules are tighly packed and harder than liquids and gases. Examples: Ice‚ Coal‚ Salt Amorphous solid-a solid which has a disordered atomic structure. Examples: Glass‚ Rubber Liquids flowing freely but of constant volume. Examples: Water‚ Mercury‚ Alcohol Viscosity-a measure of its resistance to gradual deformation by shear stress or tensile stress. Surface tension-the force that acts on the surface of a liquid and tends to minimize the surface
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Preparation of Standard Solutions and Use of a Spectrophotometer to Measure the Concentration of an Unknown Solution Introduction Concentration is the ratio of the quantity of solute to the quantity of the solvent or the quantity of solution. By knowing this‚ CO(NO3)2 *6H2O Purpose What is the percent transmittance of six different solutions of cobalt (II) nitrate hexahydrate using a spectrophotometer? Materials * Graduated cylinder (10 mL) * Graduated cylinder (25 mL) * pipet
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transitions. By comparing the spectrum of an analyte with those of sample molecules‚ you can get an idea as to the identity of the absorbing groups. Solutions of transition metal ions can be colored (i.e.‚ absorb visible light) because d electrons within the metal atoms can be excited from one electronic state to another. The color of metal ion solutions is strongly affected by the presence of other species‚ such as certain anions or ligands‚ an example of this is the chromium (VI)‚ Cr (VI) specie.
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DETERMINATION OF THE WATER POTENTIAL OF POTATO TUBER CELLS. Method. Five sucrose solutions with varying molarity and one control containing distilled water were prepared and poured into test tubes. The potato discs were dried‚ weighed and added to the test tubes. The discs were then weighed again after a period of 24 hours. The percentage change in mass was then calculated. Apparatus.  Specimen tubes with stoppers x6  1cm3 diameter cork borer  razor
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Electrolyte and Nonelectrolytes Electrolytes •Separates in water forming a solution that conducts electric current •IONIC COMPOUNDS Non- electrolytes • does not allow the flow of an electric current • COVALENT COMPOUNDS Freezing Point Depressio n Freezing Point Depression Adding a solute to a solvent decreases freezing point of the solvent Amount of solute Freezing Point of solvent Tf° (pure solvent) > Tf (solution) Freezing point of pure solvent – 0o Tf = Tf° - Tf Freezing Point Depression
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Freeze! The Effect of Super Cooling Water on Nucleation in Aqueous Solutions Hunter B. Tuck Author Note Hunter B. Tuck‚ Southside Virginia Community College‚ Keysville‚ VA. Contact: huntertuck1212@gmail.com Abstract This particular study demonstrated the overall effects of super cooling different types of aqueous solutions. In similar studies conducted upon super cooling water‚ researchers have only used distilled water in their experiments. In this study‚ however‚ rain‚ tap‚ and purified bottled
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The solution my group used was NaCl‚ and we used varying concentrations to see if that would affect the osmolality of our potato cores. Our explanatory hypothesis was that concentrations of a solution and osmolality of potato cores would be unrelated. We predicted that even though there were varying concentrations of solute‚ potato osmolality would be
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Purpose : The experiment this week had two different purposes. The first is to teach us about freezing points. This lab was designed to show us the freezing point of a pure solvent‚ in comparison to a solvent in a solution with a non-volatile solute. The second goal of the experiment is to teach students about osmosis. In the experiment‚ we got to observe osmosis as well as understand dialysis. Procecure : Part 1. Colligative Properties 1. Create a water
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amount of the solutes‚ roughly one scoop from the scoopula‚ were placed into clean test tubes. 2-3 pipettes of the solvent were placed on to the solutes. They were placed onto a tray and were left to dissolve over time. Obsevations were taken of each solution mixture. The solvents
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water concentration of a solution outside the cell is lower than the concentration inside the cell‚ water will move from the inside to the outside of the cell due to osmosis. As we increase the concentration of the NaCl solutions we have used (0.1M to 0.6M)‚ more moles of NaCl are dissolved in the solution. Thus‚ the solutions increases in solute concentration but decreases in water concentration. We can therefore assume; the higher the concentration of the NaCl solution‚ the higher the number of
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