NOT FOR ELECTRONIC STUDENT ACCESS ONLY FOR CLASSROOM USE!! Unit 9: Stoichiometry Practice 1. Differentiate between the significance of the coefficients in a balanced chemical equation and the significance of the subscripts in a chemical formula. · Coefficients show the correct proportions of atoms and molecules in a chemical reaction. They are normal sized numbers placed at the beginning of the chemical formulas in a chemical reaction during the process of balancing. They tell how many of an entire
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cm3 of hydrochloric acid measured by glass pipette. Add 0.5 g of eggshell dust to each beaker‚ measured by balance. While the reaction of eggshell with acid occurs‚ prepare the buret and clamp for titration. Make sure they are clean. Pour NaOH solution into the buret to the ’0’ level. Make sure all of the eggshell reacted with the HCl. If not‚ you can help the reaction by using the baguette. Put two drops of phenolophateine into each beaker using the plastic pipette. Take the first
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Titration: Titrations are a quantitative chemical analysis technique. They are done to tell us how much acid is required to neutralise a certain quantity of alkali. A titration is a technique in which a solution of reactant (the titrant) is added to a solution of a second reactant (the analyte) until the end point is reached. The end point of the titration is the point at which the titrant has been added in the right quantity to neutralise the analyte. Usually you can see this by adding a reagent
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ids Acids‚ Bases‚ Buffers and Respiration Darlene E. McDonald WCCC Fall 2012 Ap Lab 071-07 Dr. Roxanne Levandosky August 31‚ 2012 I. INTRODUCTION: A.PURPOSE: a. To define and understand the key terms. ~acid ~buffer system ~base ~acidosis ~pH ~alkalosis ~pH scale ~hypoventilation ~pH indicators ~hyperventilation b. To determine the acidic or base nature and actual pH of various substances. c. To discuss the formation of the carbonic acid/bicarbonate ion
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bases). After ranking the pH of these solutions‚ you will then test your predictions in the laboratory. 1. Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO‚ HCl‚ HCN‚ NaOH‚ NH3‚ NaCN‚ KNO3‚ H2SO4‚ NH4Cl‚ H2SO3‚ NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: H2SO4: This is because the first hydrogen is strong and completely ionizes and the second is weak and ionizes very minutely
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0.0746 moles unreacted. The amount of NaOH moles needed to completely react with this excess HCl is .0746 moles of HCl and .0746 moles of NaOH. To titrate the excess HCl you would need a molarity of 2.984 NaOH. In the equation Zn(s) + 2HCl (aq) = H2 (g) + ZnCl2 (aq) ZnCl2 is soluble. When using NaOH the equation would be ZnCl2 + 2NaOH = Zn (OH)2 + ZnCl and Zn(OH)2 has a low solubility. Procedure: In this part of the lab we will be titrating ZnCl2 and NaOH with HCl to figure out how much zinc is
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lease favorable for bioavailability of iron) 5. Which substance would hinder the intestinal uptake of iron? Caffeine would hinder the intestinal uptake of iron. This is because it formed the largest precipitate when reacted with iron solution and NaOH. 6. Consider the substances you tested and the sources for these substances in the American diet. What recommendations can you make which would optimize iron absorption? According to Mayo clinic‚ experts advise that we should eat foods high in iron
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EXPERIMENT-1 CHEMICAL REACTIONS AIM: To perform and observe the following reactions and classify them into: (i) Combination reaction (action of water on quick lime) (ii) Decomposition reaction (action of heat on ferrous sulphate crystals) (iii) Displacement reaction (iron nails kept in copper sulphate solution) (vi)Double decomposition reaction (reaction between sodium sulphate and barium chloride) APPARATUS REQUIRED: 1. A rack of at least six clean test tubes and a boiling
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Ka Strong acid + strong base: equivalence pH 7 Strong acid + weak base: equivalence pH 3-6 Strong base + weak acid: equivalence pH 8-11 Weak base + weak acid: equivalence unknown (use back titration for analysis) i. A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 v. The titration curves will essentially be the same after passing the equivalence point vi. Methyl red would be a suitable indicator for both titrations 1.3 Back Titration
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different solutions to the test tubes (pepsin‚ distilled water‚ HCI‚ and NaOH) Controlled variable: *the same amount of solution poured into each test tube *ensuring that each test tube is clean Responding variable: *The pH levels and the size of the egg white Materials: Hydronium pH paper 6 large test tubes (22*175mm) 10 mL graduated cylinder 10% pepsin solution Knife Tweezers or forceps Wax pen 1.0 mol NaOH solution 1.0 mol HCI solution Hard-boiled egg Metric ruler Plastic gloves
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