This is termed the hydrotropic effect. Examples of hydrotropic salts include ETH maleate‚ succinate‚ and oxalate2. The hydrotropic effect is achieved by adding an organic salt which will increase the saturation solubility of a drug in an aqueous solution by increasing hydrogen bonding. The mechanism of hydrotropism involves weak interactions between the hydrotropic agent and the insoluble drug. This method closely resembles complexation. Commonly used hydrotropic substances include caffeine‚ sorbitol
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Product Constant Q: Write the equilibrium equation for a saturated solution of the following salts and the corresponding solubility product expressions. a) BaSO4 (s) b) MgF2 (s) c) Ag2S (s) d) Cu(IO3)2 (s) [ ][ [ [ A: [ ( Q: ) ] ][ ][ ] ] What is the equilibrium concentration of Cd2+ ions in a saturated solution made by shaking CdS(s) with water? Ksp = 6.0x10-27 for CdS. [ A: [ Q: ][ ] ][ ] ; ][ ] √ √ A solution in equilibrium with a precipitate of AgCl was found to contain 3.4x10-6M
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test APPARATUS AND MATERIALS: 4% stock solution of glucose‚ water‚ 6 test tubes‚ ruler‚ water bath‚ solution of unknown concentration (Sample A)‚ Benedict’s reagent METHOD: 1. Solutions of different concentration were made from the stock solution and placed in test tubes. 2. All test tubes were labeled appropriately‚ according to table below‚ and Benedict’s test was carried out on the various dilutions for 5 minutes. 3. The colours of the solution were observed and heights of precipitate
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will decrease as the salt in the solution increases. This is because the solution around the potato will draw the water from the potato‚ causing it to decrease in size. Method: To begin this experiment‚ 1½ teaspoons of salt was added to a beaker containing 100 mL of distilled water. This was the 7% solution. 50 mL of this solution was poured into a second beaker and 50 mL of distilled water was added. This produced the 3.5% solution. 50 mL of this solution was added to a third beaker‚ then
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* In a solution‚ the positive hydrogen side of water is attracted to the negative parts if the compound it is dissolving while the negative oxygen is attracted to the positive parts * “Like dissolves like” – describes whether one substance will dissolve in another. Water for example can’t dissolve nonpolar substances Concentrations on Solutions * Solvent: The liquid in which a solute is dissolved to form a solution. * Solute: The minor component in a solution‚ dissolved
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concentrations and a blank solution are prepared and their absorbances are measured with a UV-Vis spectrophotometer (Table 1). The absorbances of three unknown samples with same concentration and a blank are measured (Table 2). The blank solutions are used as a reference solution to calibrate the colorimeter. The volumes of Fe solution for the delivery volume errors in the 10 ml graduated pipet are corrected (Table 3). The molarity (μg/mL) of Fe (o-phenanthroline)32+ in each standard solution is calculated by
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in solution move from areas of higher concentration to areas of lower concentration in the attempt to reach homeostasis in different circumstances. Introduction: The main purpose of this lab was to observe diffusion and osmosis. This is demonstrated using dialysis tubing and a combination of monosaccharaides‚ disaccharides‚ water (H20)‚ and sodium chlorine
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conducted to see if the potato cylinders would gain weight or lose weight because of osmosis. The second part was conducted to see if a dialysis bag‚ filled with sodium sulfate and starch solution and placed in an albumin/glucose solution‚ would contain albumin/glucose from the outside or the albumin/glucose solution would contain any sodium sulfate/starch from the inside. The first part of this experiment there is a relationship between the amount of sucrose concentration and final mass. As the sucrose
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settled on its own. We poured out the solution into a paper cup‚ leaving the sand in the beaker. We attempted to heat the sand slowly to dry it out‚ but there was one big splatter that occurred and we lost a tiny bit of sand‚ but we then scrapped the sand out of the beaker and onto the scale to weigh it as best we could. Then adding the paper cup solution to a cup of ice water we watched as the benzoic acid crystalized and floated to the top. We then poured that solution through a filter and funnel into
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To determine the effect osmotic pressure might have on cellular membranes‚ specifically when beet slices are placed in NaCl solutions of varying concentrations. 2. Hypothesis: The osmolarity will directly increase with increasing NaCl concentrations. 3. Control = Distilled Water – this was present in all solutions 4. The independent variable – salinity of the 6 solutions; while predetermined‚ the NaCl concentrations varied from 0% to 15%. The dependent variable – beet osmolarity; this lab’s focus
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