the qualitative traits of chemicals and their corresponding chemical reactions with other chemicals were more evident and familiar. Five preliminary tests were used to infer possible ions: two for cations‚ namely‚ precipitation reactions with hydroxide (OH-) and ammonia (NH3) respectively; and two for anions‚ namely‚ precipitation reactions with barium nitrate (Ba(NO3)2)‚ and non-precipitation reactions involving ferric chloride (FeCl3) and potassium permanganate (KMnO4) respectively. Confirmatory tests
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Yuri Anthony D. Sucgang BMLS-IA Electrophoresis Machine Gel Electrophoresis Apparatus(Aragose Gel) Electrophoresis is the motion of dispersed particles relative to a fluid under the influence of a spatially uniform electric field. Gel electrophoresis is a laboratory procedure used to separate biological molecules with an electrical current. In this lesson‚ we’ll review how agarose gel electrophoresis works and introduce the equipment necessary to perform an electrophoresis experiment.
Free Chromatography Thin layer chromatography Hydrochloric acid
Chart Negative Ions (Anions) + Positive Ions (Cations) = Solubility of Compounds in water Example any anion + Alkali Ions (Li+‚ Na+‚ K+‚ Rb+‚ Cs+‚ Fr+) = soluble Sodium fluoride‚ NaF‚ is soluble any anion + hydrogen ion [H+ (aq)] = soluble hydrogen chloride‚ HCl‚ is soluble any anion + ammonium ion (NH4) = soluble ammonium chloride‚ NH4Cl‚ is soluble nitrate NO3- + any cation = soluble potassium nitrate‚ KNO3‚ is soluble acetate (CH3COO-) + any cation (except Ag) = soluble sodium
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Conclusion…………………………………………………………………………………………………………….11 Anion Percipitate Test #1 1. For the first percipiate test with my unknown H chemical‚ I mixed it with ‚ or Lead (III) nitrate. The purpose of this test was to determine whether my unknown formed a percipitate with Lead (III) nitrate‚ and to eliminate anions. 2. If the reaction with is soluble‚ it would allow me to narrow down my options to fewer suspected anions. Since only a few anions formed percipitates with Lead (III) nitrate according
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deliquescent and colorless. The student is asked to perform test and observation on the salt to determine the cation and anion present. HYPOTHESIS: Perhaps by using the flame test or reacting salt x with NaOH‚ or NH4OH the cation could be distinguished by observing the color changes or solubility while reacting salt x with H2SO4 or a mixture of copper turnings and concentrated sulphuric acid the anion of the salt could be found. AIM: To determine the constituents of salt x. APPARATUS/MATERIALL:
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The potassium atoms and the lead atoms can be classified as cations‚ since they are metals. The iodine atoms and the nitrate ion can be classified as anions since they are nonmetals. Upon mixing‚ the solution turned into a cloudy yellow color. Evidence that a chemical reaction occurred was that the two solutions created a new color because the two solutions were originally colorless. There was no gas formed. Part B: (Testing the Anions) Iodide reaction with hydrogen peroxide observations- The
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substances are split-up into two types of charged particles one of which is positively charged and the other is negatively charged. The charged particles are called ions or radicals. The positively charged ions are called cation or basic radical. The negatively charged ion is called anion or acid radical. In the qualitative analysis of an inorganic substance number of tests are carried out in order to discover the acidic and basic radical present in it. A test is an experiment along with an observation
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IONIC COMPOUNDS In chemistry‚ an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. Usually‚ the positively charged portion consists of metal cations and the negatively charged portion is an anion or polyatomic ion. Ions in ionic compounds are held together by the electrostatic forcesbetween oppositely charged bodies. Ionic compounds have high melting and boiling points‚ and they are hard and very brittle. Ions can be single atoms‚ as the sodium and chlorine in
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inorganic compounds begins with naming ions. Cations formed from metal atoms have the same name as the metal. See a chart of common cations If - and ONLY if - a metal can form different cations‚ the positive charge is indicated by a Roman numeral in parentheses following the name of the metal. Fe+2 iron (II) Fe+3 iron (III) The names of monatomic anions are formed by replacing the ending of the name of the element with -ide. See a chart of common anions. Cl− chloride ion Br− bromide ion
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SEVEN STEPS TO A NET IONIC EQUATION EXAMPLE: KCl(aq) + Pb(NO3)2(aq) ( 1. a. Take only one of the first cation(s) and match it with one of the second anion(s). (Write the cation first) b. Take only one of the second cation(s) and match it with one of the first anion(s). (Write the cation first) KCl(aq) + Pb(NO3)2(aq) ( KNO3 +PbCl 2. Correct the formulas of the products based on the charges of the ions. KCl(aq) + Pb(NO3)2(aq) ( KNO3 +PbCl2 ◄ 3. Balance the equation
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