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    1. The traditional method of analysis for the amount of chloride ion present in a sample was to dissolve the sample in water and then slowly add a solution of silver nitrate, silver chloride is very insoluble in water, and by adding a slight excess of silver nitrate, it is possible effectively to remove all the chloride ion from the sample. First write a balanced net ionic equation for this reaction. Then, assume that a sample has a mass of 1.054 grams contains 10.3% chloride ion by mass. Then calculate the mass of silver nitrate that must be used to completly precipitate the chloride from the sample. How many silver chloride molecules will be formed?

    2. Many metals occur naturally as sulfide compounds, including CuS and CoS. Air pollution often accompanies the processing of these ores, because toxic sulfer dioxide is released as the ore is converted from the sulfide to the oxide by smelting. Condiser the reaction of zinc sulfide with oxygen to form zinc oxide and sulfer dioxide. First, write a balanced equation for this reaction. Then, how many kilograms of sulfer dioxide are produced when 100 kilograms of zinc sulfide is smelted in excess oxygen by this process? How many moles of zinc oxide are formed?

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    Solution Preview

    Please refer to the attached file. Cheers.

    1) The net ionic equation is:

    Ag+(aq) + Cl-(aq)  AgCl(s)

    mass of Cl in the sample = 1.054 g * 0.103
    = 0.108562 g

    moles of Cl- in the sample = mass / molar mass
    = 0.108562 g / 35.4527 g mol-1
    = 3.062  10-3 moles

    Because the chloride ...

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