Lab – Solubility Curve for Potassium Nitrate I. Purpose: To plot a solubility curve for potassium nitrate in aqueous solution. II. Safety: Wear eye protection throughout the experiment. Be cautious of hot water. Wash hands if you come into contact with potassium nitrate. III. Procedure: 1. Carefully weigh out your assigned mass of potassium nitrate on a piece of weigh paper. Carefully pour the sample into the large test tube. 2. Add 20. mL of distilled water to the tube.
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changes that indicate a chemical reaction such as a color change‚ the formation of a precipitate‚ or the evolution of a gas should be noted. Each mixture contained five drops of the nitrate solution being tested‚ mixed with five drops of the solutions containing sulfate‚ carbonate‚ oxalate‚ or iodate. After mixing‚ the observation of chemical change was
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Solubility as a Property of Matter A Lab of Chemicals‚ Chromatography‚ and Crime! Chemistry is a natural science that deals with the composition of matter and the changes it undergoes. At crime scenes‚ investigators often find unknown materials that need to be identified. If an unknown material is a mixture‚ an investigator may want to know one or two things about it: What are the ingredients of the mixture? Is the mixture found at the scene the same as a known mixture? A mixture is a collection
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Lost and Found in Translating Tourist Texts Domesticating‚ Foreignising or Neutralising Approach He Sanning‚ Nanjing University of Information Science and Technology ABSTRACT Domesticating and foreignising strategies are popular in translation studies and each of them has its own advantages and disadvantages in translating tourist texts. The advantages for domesticating include maintaining the terseness of the text‚ obtaining the reader‘s understanding of the translated text‚ and gaining
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parameters sush as pH‚ Temperature or dissolved Oxygen and compare findings. To produce anti-microbial activity from Staphylococcus warneri. II. INTRODUCTION: Staphylococcus warneri is a member of bacterial genus Staphylococcus‚ consisting of Gram-positive bacteria with spherical cells appearing in clusters. Colonies of S. warneri are usually tan‚ yellow and about 2-4mm in diameter after 48 hours incubation at 35°C. It is commonly found as part of the skin flora on humans and animals.
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In this experiment all of the precipitates result from the exchange of positive and negative ions between reacting solutions of two ionic compounds. Thus‚ in this example the precipitate must be either silver chloride‚ AgCl or sodium nitrate‚ NaNO3. Sodium nitrate dissolves readily in water and is therefore soluble. Thus we can conclude that silver chloride is the insoluble precipitate. We can represent the formation of this precipitate by a net ionic equation: Ag+ +NO3 ̄ +Na++Cl ̄→AgCl+NO3 ̄+Na+
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The primary focus of experiment 4 was to teach a student the basic solubility rules of salts in aqueous solutions. After developing and using a scheme for the qualitative analysis of three cations in an aqueous mixture‚ a student would use a centrifuge to identify‚ precipitate‚ and separate the three ions in the mixture. After becoming familiar with all three cations‚ the student would use the scheme again to identify at least two of the cations in an unknown solution. In order to begin the separation
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The Sequence of Chemical Reactions Drew Selfridge Dave Allen‚ Lab partner Instructor Yang February 11‚ 1997 INTRODUCTION This experiment was to recover the most amount of copper after it is subjected to a sequence of reactions. The copper is originally in solid form‚ but the reactions will turn it into free Cu+2 ions floating in solution. The ions will then be regrouped to form solid copper once again. During this process‚ however‚ some of the Cu+2 ions may be lost. The copper will subjected
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Figure 2. Absorption of isolated chloroplasts from spinach using multiple color filters References Dansereau‚ D. 2013.Molecular and Cellular Biology Lab Manual‚ Saint Mary’s University‚ Lab 7.
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Experimental Prep and Optimum wavelength Selection An ionic Iron solution with a known concentration of 4.047x10-3 M was obtained. A 250-mL sample of a 10-fold dilution of this ionic iron solution and 5 drops of concentrated HNO3 was made. This solution served as the source of ionic Iron for the remainder of the lab and was labeled “stock ionic Iron solution.” Next‚ a 50-mL aqueous ionic Iron and FerroZine® complex solution was prepared by adding 5.00mL stock ionic Iron‚ 3-mL of acetic acid buffer‚ 2-mL of 5%
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