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in a 0.5 g ore sample that contains 1.5 parts per thousand silver? Allow for a 50% excess
of the chloride solution?
Prepare 2 liters of a 4 molal solution of MgSO4 in water. The MgSO4 is the solute and water is the solvent. Use rounded numerical atomic weights instead of exact ones with decimal values.
a) how much MgSO4 should be weighed out?
b) how many molecules of MgSO4 should be weighed out?
c)How many individual atoms of solute are present?
d) how much water should be added?
The E can be electrolyzed after melting to yield 4.0 grams of F and 1.6 grams of G, neither of which can be further decomposed by ordinary chemical means. E combines with water to give 1.3 grams of J per gram of E and gas L. The gas L has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen.
The gas L has exactly the same properties as the product obtained when carbon is burned in an excess of oxygen
Write a balance molecular equation for the reaction between KMnO4 and KI in Basic Solution. The skeleton ionic reaction is MnO-4(aq)-> MnO2/4 (aq)+ IO-3 (aq). Show your solution.
Draw the procedure.
1.Tear off the outer cardboard covering and remove the metal plate at the top of the dry cell. Carefully draw out the carbon rod with its attached brass cap using a pair of pliers. Remove the pitch at the top. Scrape the mixture of manganese dioxide and ammonium chloride into the beaker. Clean the zinc casing by washing with hot water. Dry and cut it into small pieces. Keep the pieces of zinc in a stoppered and labeled bottle for future use. Save the carbon rods.
