How do you get a qualitative idea of how certain solutes dissolve in certain solvents?
927953
Try to remember "like dissolves like".  Look at the compound that you're trying to dissolve and determine how polar it is or how "organic" it is.  Molecules with high polarity like salts or sugars will dissolve in polar solvents like water, alcohols, esters.  Molecules that are very non-polar will dissolve in non-polar solvents like benzene, hexane, petroleum ether and so on.  Solvents "in the middle" like acetone and longer-chain alcohols will dissolve the mid-range solutes but not the very polar or the very non-polar.\n\nHope this helps you.
965514
solution:\nA homogeneous, liquid mixture of two or more substances.\n\nsolvent: The dissolving agent of a solution. Water is the most versatile solvent known.\n\nsolute:\nA substance that is dissolved in a solution.
684681
C because the solution is SATURATED with solute, meaning no more solute can be dissolved by the solvent in the solution.
485893
Check on the internet for the ratios used by comercial factories, then prepare a solution from glycol and water in the given proportion. That's all!!!
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IF substance contains both hydrophobic and hydrophilic parts:\n  Make the part that is soluble in polar solvents i.e the part having polarity in water and rest in some nonpolar solvent.\n\nIFsubstance is purely ionic represent it as ions in water.
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This is a poorly worded question.  All chemicals have some solubility in water, however minute.\n\nOf these selections, I would go with A\n\nAdding a charge facilitates dissolution.\nMany covalent materials (oil) have low solubility \nMany large molecules are water soluble (Poly Ethylene Glycol)
900560
Most solutes (sugar in this case) have limited solubility (ability to dissolve) in most solvents (water in this case). This solubility varies with temperature - the hotter the solution, the higher the solubility. As mentioned in an earlier answer, this means more energy must be added to dissolve more solute. On the other hand, if energy is taken out of a solution, the solute will usually  come out of the solution, depending on the concentration.\n\nThis physical law that governs this is the 2nd law of thermodyamics.
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See comment above.\n\nYou do need to do several trials at various concentrations though. You can then determine it through a linear regression.\n\nI also suggest that you consult a book on Analytical chemistry, because Beer's law has limitations. For example, it loses linearity at higher concentrations.
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to determine whether an acid or a base is soluble in say the universal polar solvent water, u should be knowing whether the substance is strong or weak\nnow bases like NaOH, CsOH, RbOH, Mg(OH)2 are strong bases and in solution they give us the cations and anions(mostly the hydroxyl grp)\nbases like Be(OH)2, Fe(OH)2 or 3, Cu(OH)2 or any of their oxides are weak and hence in solution they do not undergo complete dissociation and most of these are insoluble\nso in case ur not in a lab, the only way is to identify their degree of weakness
889419
1) Decide what solvent you want to use: water or organic?\n2) Decide how much solution you want: 1L?\n3) Check the solubility of phenol in the solvent you choose. And calculate how much phenol you'll need by weight to make a saturated solution\n4) Find out the relationship between solubility and temperature.\n5) I assume you want to make a saturated phenol solution at room temperature. If the solubility increases as temperature goes higher, add a bit more phenol than needed (from the calculation above) to the solvent. \n6) Heat the flask or beaker that contains the solvent and phenol until all phenol dissolves.\n7) Let the container cool down to room temperature.\n8) If no phenol crystalizes the solution is over-saturated. You may rub the side of the flask or beaker to help phenol crystalize.\n9) You have your saturated phenol solution!!
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Molecular compounds do not dissolve in aqueous solution. Ionic compounds do. Sugar does not dissolve readily into water because it is an organic substance. Organic substances do not dissolve easily.
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In chemistry, concentration or Mass Percent is the measure of how much of a given substance there is mixed with another substance. This can apply to any sort of chemical mixture, but most frequently is used in relation to solutions, where it refers to the amount of solute dissolved in a solvent.\n\nTo concentrate a solution, one must add more solute, or reduce the amount of solvent (for instance, by selective evaporation). By contrast, to dilute a solution, one must add more solvent, or reduce the amount of solute.\n\nThere exists a concentration at which no further solute will dissolve in a solution. At this point, the solution is said to be saturated. If additional solute is added to a saturated solution, it will not dissolve. Instead, phase separation will occur, leading to either coexisting phases or a suspension. The point of saturation depends on many variables such as ambient temperature and the precise chemical nature of the solvent and solute.\n\nQualitative description\nOften in informal or non-technical language, concentration is descibed in a qualitative way, through the use of adjectives such as "dilute" or "weak" for solutions of relatively low concentration and of others like "concentrated" or "strong" for solutions of relatively high concentration. Those terms relate the amount of a substance in a mixture to the observable intensity of effects or properties caused by that substance. For example, a pratical rule is that that the more concentrated a chromatic solution is, the more intensely coloured it is.\n\nQuantitative notation\nFor scientifical or technical applications, a qualitative account of concentration is almost never sufficient, therefore Quantitative notations are needed to describe concentration. There are a number of different ways to quantitatively express concentration; the most common are listed below.\n\nNote: Many units of concentration require measurement of a substance's volume, which is variable depending on ambient temperature and pressure. Unless otherwise stated, all the following measurements are assumed to be at standard state temperature and pressure (that is, 25 degrees Celsius at 1 atmosphere or 101.325 kPa).\n\nMass percentage\nMass percentage denotes the mass of a substance in a mixture as a percentage of the mass of the entire mixture. For instance: if a bottle contains 40 grams of ethanol and 60 grams of water, then it contains 40% ethanol by mass. Commercial concentrated aqueous reagents such as acids and bases are often labeled in concentrations of weight percentage with the specific gravity also listed. In older texts and references this is sometimes referred to as weight-weight percentage (abbreviated as w/w).\n\nMass-volume percentage\nMass-volume percentage, (sometimes referred to as weight-volume percentage and often abbreviated as % m/v or % w/v) denotes the mass of a substance in a mixture as a percentage of the volume of the entire mixture. Mass-volume percentage is often used for solutions made from solid reagents. It is the mass of the solute in grams divided by the volume of solution in millilitres and multiplied by one hundred .\n\nVolume-volume percentage\nVolume-volume percentage or % (v/v) describes the volume of the solute in mL per 100 mL of the resulting solution. This is most useful when a liquid - liquid solution is being prepared. For example, beer is about 5% ethanol by volume. This means every 100 mL beer contains 5 mL ethanol (ethyl alcohol).\n\nMolarity\nMolarity (M) denotes the number of moles of a given substance per litre of solution. For instance: 4.0 litres of liquid, containing 2.0 moles of dissolved particles, constitutes a solution of 0.5 M. Such a solution may be described as "0.5 molar." (Working with moles can be highly advantageous, as they enable measurement of the absolute number of particles in a solution, irrespective of their weight and volume. This is often more useful when perform
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When choosing a recrystallizing solvent you want a liquid that:\n\n1. Does Not React with what your trying to recrystallize.\n\n2. A solvent that the compound is barely soluble in. \n\n3. A solvent that quickly evaporates.\n\n    After you determine your solvent you can dissolve your compound without changing it. You can add just enough solvent to dissolve the compoud. Wait for the solvent to evaporate causing the ppt of your purified compound.\n\nMark
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TSP is a solid.  You have to dissolve it to get a pH reading.   The pH will necessarily be dependent upon concentration and the pH of the solvent used.
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First, you dissolve your compound in the solvent in which is is most soluable (perhaps THF or methylene chloride).  Then you very carefully use a pipette to layer the solvent in which it is not soluable on top (perhaps diethyl ether or pentane).  You need to add the second solvent slowly and carefully.  Let the solvent run down the side of the container.  Obviously the top solvent needs to be less dense than the bottom one.  You then let the container sit undisturbed on the bench or in the freezer away from any vibrations until crystals form.  As the upper solvent diffuses into the lower solvent, you compound will become less soluable until it falls out.  The first solution should be as close to saturated as possible.
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Solution is the mixture of a solvent and a solute ,where the solute dissolves in the solvent.
512002
Yup, non-polar solvents.  If acetone, alkanes, or toluene don't work, then go with petroleum ether(hist. ligroin) that dissolves alot of things.