chemical react with each other. The first experiment will be a demonstration the professor will give to the class. the first experiment you will be performing will include a test tube you will add a couple drops of dilute hydrochloric. you will add this to five little pieces of zinc metal. In next experiment you will performed you will put 2 ml of 3% hydrogen peroxide solution in a test tube .you will also use a spatula and add a very small amount of manganese dioxide into the tube .to make sure the
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that is going to be measured. The independent variable is the titrant; zinc sulphate (ZnSO4) solution which will be prepared by dissolving ZnSO4 in distilled water. The materials that will be used in the following experiment include: • Sixteen volumetric flasks • Zinc sulphate (ZnSO4) solution • Axe deodorant solution • Nivea deodorant solution • Citymen deodorant solution • Ethylenediaminetetraacetic acid (EDTA)
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Evelyn Ramos CHEM LAB 201-003 Professor Ruddock Experiment #4 - Chemical Reactions Performed: 3/6/13 DUE: 3/13/13 Pre Lab Questions: 1. Before you can write a chemical equation‚ what must you know? You have to know what the products and reactants are. 2. What observations might you make that suggest that a chemical reaction has occurred? If a gas is produced or precipitates are formed that indicates chemical reaction. Also‚ if color changes occur or
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EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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15. Write the balanced chemical equation of the following and identify the type of reaction in each case: i. Potassium bromide(aq) = barium iodide(aq) -> potassium iodide(aq) = bariumbromide(s) ii. Zinc carbonate(s) -> zinc oxide(s) = carbon dioxide(g) iii. Magnesium(s) = hydrochloric acid(aq) -> magnesium chloride(aq) = hydrogen(g) Q. 16. Wrte an activity to shw the change in the state of matter and change in temperature during a chemical reaction (change). Q. 17. Write an activity
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I. Grade Level/Unit Number: 9-12 Unit 7 II: Unit Title: Mole Concept III. Unit Length: 7 days (on a 90 min. per day block schedule) IV. Major Learning Outcomes: Students should be able to: Mole Concept • Calculate formula mass. • Convert representative particles to moles and moles to representative particles. (Representative particles are atoms‚ molecules‚ formula units‚ and ions.) • Convert mass of atoms‚ molecules‚ and compounds to moles and moles of atoms
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°C [± 0.1] | | | | |Substance I |Substance II | | | | |1. |Sodium Hydroxide [l] + Dilute hydrochloric|10.0 cm³ |10.0 cm³ |27.9 |29.3 |Exothermic | | |acid [aq] | | | |
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should include three features of the flowers. [6] © UCLES 2009 0653/06/M/J/09 [Turn over 4 2 The teacher gives a student a piece of zinc and some dilute hydrochloric acid. The student uses the apparatus in Fig. 2.1 to investigate the speed of reaction of the zinc and hydrochloric acid. hydrogen measuring cylinder For Examiner’s Use zinc dilute hydrochloric acid 100 Fig. 2.1 • • • The student places 4 cm3 of the acid in a test-tube. He starts his clock. Every minute‚ he records in Fig. 2.2
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This happened because of the carbon dioxide | Weight before 120.3 g | Part C | Zinc with Hydrochloric acidIt bubbled up like it was boiling and produced hydrogen gas. | Zinc weight- 1.5 | Part D | It took a little while of just clear then turned into a Carolina blue precipitate | | Part E | Zinc turned fire red (The copper was already red)Liquid turned a tar heel blueWarm on the bottom | | Part F | H2O2 Hydrogen proxide KI |
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What precipitation reaction could be used to separate and remove silver ions from a mixture containing iron (III) and zinc ions? A precipitation reaction that could be used is hydrochloric acid Ag+(aq) + HCl(aq) AgCl(s) +H+(aq) – white. 2. What precipitation reaction could be used to separate and remove iron (III) ions from the remaining mixture containing iron (III) and zinc ions? Fe3+(aq) + 3NaOH(aq) Fe(OH)3(s) + 3Na+(aq) 3. How can the presence of silver ions be positively identified?
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