Chapter 4: Problem 104
Oxygen \(\left(\mathrm{O}_{2}\right)\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.
Chapter 4: Problem 104
Oxygen \(\left(\mathrm{O}_{2}\right)\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.
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Get started for freeCalculate the concentration of the acid (or base) remaining in solution when \(10.7 \mathrm{~mL}\) of \(0.211 \mathrm{M}\) \(\mathrm{HNO}_{3}\) are added to \(16.3 \mathrm{~mL}\) of \(0.258 \mathrm{M} \mathrm{NaOH}\).
Carbon dioxide in air can be removed by an aqueous metal hydroxide solution such as \(\mathrm{LiOH}\) and \(\mathrm{Ba}(\mathrm{OH})_{2} .\) (a) Write equations for the reactions. (Carbon dioxide reacts with water to form carbonic acid.) (b) Calculate the mass of \(\mathrm{CO}_{2}\) that can be removed by \(5.00 \times 10^{2} \mathrm{~mL}\) of a \(0.800 \mathrm{M} \mathrm{LiOH}\) and a \(0.800 M \mathrm{Ba}(\mathrm{OH})_{2}\) solution. (c) Which solution would you choose for use in a space capsule and which for use in a submarine?
Write the equation that enables us to calculate the concentration of a diluted solution. Give units for all the terms.
Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?
The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measure a very small volume of a stock solution. Instead, it is done by a series of dilutions. A sample of \(0.8214 \mathrm{~g}\) of \(\mathrm{KMnO}_{4}\) was dissolved in water and made up to the volume in a 500-mL volumetric flask. A \(2.000-\mathrm{mL}\) sample of this solution was transferred to a \(1000-\mathrm{mL}\) volumetric flask and diluted to the mark with water. Next, \(10.00 \mathrm{~mL}\) of the diluted solution were transferred to a \(250-\mathrm{mL}\) flask and diluted to the mark with water. (a) Calculate the concentration (in molarity) of the final solution. (b) Calculate the mass of \(\mathrm{KMnO}_{4}\) needed to directly prepare the final solution.
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