Lab This procedure is one type of redox titration known as an iodometric analysis. In the first step, excess potassium iodide is added to a solution of bleach and is oxidized to iodine by the hypochlorite ion. Acetic acid is added to provide the hydrogen ion needed for the reaction. CIO +2H+ + 21- ----- 12 + CI- + H2O The amount of iodine formed by this reaction is found by titrating with sodium thiosulfate solution. 12 + 2S2032---- 21- + S4062- Step 1 Use 5ml pipet to measure out a sample of a laundry bleach and transfer to a 250ml volumetric flask. Using the density of bleach (1.11g/cm°) determine the mass of the 5ml sample. Step 2 Fill the buret with the sodium thiosulfate solution. The concentration of the sodium thiosulfate solution is 0.100M. Step 3 Place 50ml of bleach solution into a flask. Add a stir bar and stir the solution gently using the stir plate. Step 4 Add 2 gr of potassium iodide to the flask. The amount added does not have to be precise. Add 10ml of glacial acetic acid Step 5 Add about 2ml of the starch indicator Step 6 Titrate slowly until the blue color disappears. Document the value when the blue color disappears. Blue color disappears at 17.5ml Q 1. Calculate the moles of sodium thiosulfate used. 2. Calculate the moles of iodine formed. 3. Calculate the moles of NaCIO in the original sample. Oxidizing Power of Laundry Bleach

7. How many moles of ions are produced if 1 mole of LizSO4 is dissolved in water? C. 3 a. 1 b. 2 d. 4 e. 5

Write the balanced equation for the following situation. In addition, list the reaction type. You must tell the amount of every substance that remains in the container at the end of the reaction. Assume that all reactions go to completion. If only stoichiometry, tell how much excess reactant is used. Reaction Type:a. Combination Reactionb. Decomposition Reactionc. Single Displacement / THIS IS ONE TYPE OF Oxidation Reduction Reaction d. Precipitation Reactione. Gaseous Reactionf. Neutralization Reactiong. Combustion Reaction 61.802 cg of nitrogen gas is reacted with 61.802 cg of hydrogen gas to form ammonia

O science 24: Module 1 O bas ( 1 E Assignment Booklet 18 For questions 5 to 9, read each question carefully. Decide which of the choices BEST completes the statement or answers the question. Place your answer in the blank space given. 2 5. Iron oxide (FeO)) seperated into solid iron an example of a 1 (Fe (0)) A. simple composition reaction B. simple decomposition reaction C. combustion reaction D. neutralization reaction 6. In a simple composition reaction, A. one substance combines with another to form a salt and water B. two or more elements combine to form a compound C. a compound is broken down into two or more elements D. water is separated into hydroxgen gas and oxygen gas 7. fuel + oxygen → carbon dioxide + water vapour + energy This word equation is an example of a A. simple composition reaction B. simple decomposition reaction C. combustion reaction D. neutralization reaction A. simple composition reaction B. simple decomposition reaction C. combustion reaction D.…

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Please answer all parts of this question. 1. Magnesium oxide can be made by heating magnesium metal in the presence of oxygen gas. a. Write the balanced equation, including phase symbols. b. When 10.1 g of magnesium reacts with 10.5 g of oxygen gas, 11.9g of magnesium oxide is collected.       i. Determine the limiting reactant      ii. Determine the theoretical yield    iii. Determine the percent yield for the reaction

Answer questions 2 & 3