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Chapter 4: 4.94P (page 182)
Predict the product(s) and write a balanced equation for each of the following redox reactions:
The product and the balanced equation of the given reactions are:
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Is the following a redox reaction? Explain
Which ions do not appear in a net ionic equation? Why?
Mixtures of CaCl2 and NaCl are used to melt ice on roads. A dissolved 1.9348-g sample of such a mixture was analyzed by using excess Na2C2O4 to precipitate the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid, and the resulting H2C2O4 was titrated with 37.68mL of 0.1019M KMnO4 solution.
(a) Write the balanced net ionic equation for the precipitation reaction.
(b) Write the balanced net ionic equation for the titration reaction. (See Sample Problem 4.11.)
(c) What is the oxidizing agent?
(d) What is the reducing agent?
(e) Calculate the mass percent of CaCl2 in the original sample.
A student forgets to weigh a mixture of sodium bromide dehydrate and magnesium bromide hexahydrate. Upon strong heating, the sample loses 252.1 mg of water. The mixture of anhydrous salts reacts with excess AgNO3 solution to form 6.00x10-3 mol of solid AgBr. Find the mass % of each compound in the original mixture.
How many total moles of ions are released when each of the following samples dissolves completely in water?
(a) 0.734 mol of
(b) 3.86 g of
(c) formula units of localid="1656604875395"What do you think about this solution?
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