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Chapter 4: Problem 27
Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.
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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 -mL sample of this solution was transferred to a 1000 -mL volumetric flask and diluted to the mark with water. Next, \(10.00 \mathrm{~mL}\) of the diluted solution were transferred to a 250 -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.
Someone gave you a colorless liquid. Describe three chemical tests you would perform on the liquid to show that it is water.
A \(35.2-\mathrm{mL}, 1.66 \mathrm{M} \mathrm{KMnO}_{4}\) solution is mixed with \(16.7 \mathrm{~mL}\) of \(0.892 \mathrm{M} \mathrm{KMnO}_{4}\) solution. Calculate the concentration of the final solution.
What are the characteristics of an acid-base neutralization reaction?
Calculate the mass of \(\mathrm{KI}\) in grams required to prepare \(5.00 \times 10^{2} \mathrm{~mL}\) of a \(2.80 \mathrm{M}\) solution.
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