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Chapter 17: Problem 58

Give two examples of metal ions in each group (1 through 5) in the qualitative analysis scheme.

Short Answer

Expert verified
Group 1: Ag+, Hg2 2+, Group 2: Pb2+, Cd2+, Group 3: Fe3+, Al3+, Group 4: Ca2+, Ba2+, Group 5: K+, Na+

Step by step solution

01

Group 1: Cations Forming Chlorides

In Group 1, typical examples are Ag+ and Hg2 2+. This group includes metal ions that form insoluble chlorides. When a diluted hydrochloric acid (HCl) is added to a solution containing these ions, a white precipitate forms, indicating the presence of these ions as they react with chlorine to become AgCl and Hg2Cl2 respectively.
02

Group 2: Cations Forming Sulfides

For Group 2, the ions Pb2+, Cd2+ can be chosen. They are metal ions that form insoluble sulfides but soluble chlorides, reacting with hydrogen sulfide under acidic conditions to form precipitate like PbS or CdS.
03

Group 3: Cations Forming Hydroxides

In Group 3, metal ions that form hydroxides but not sulfides fall into this category. Representative ions include Fe3+ and Al3+. In the presence of a base like NaOH, these ions react to form Fe(OH)3 or Al(OH)3.
04

Group 4: Cations Forming Carbonates

In Group 4, the representative ions are Ca2+ and Ba2+, they form insoluble carbonates but soluble sulfides and hydroxides. When subjected to a carbonate solution, these ions participate in the reaction and form CaCO3 or BaCO3 as precipitate.
05

Group 5: Mostly Alkali Metal Ions

And finally, for Group 5, the ions K+ and Na+ are representative examples. These ions don't form precipitates and are typically found as alkali metal ions. They can be usually identified with flame tests. Sodium gives a distinctive yellow flame, while potassium gives a lilac flame.

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Most popular questions from this chapter

The molar mass of a certain metal carbonate, \(\mathrm{MCO}_{3}\), can be determined by adding an excess of \(\mathrm{HCl}\) acid to react with the carbonate and then "back-titrating" the remaining acid with \(\mathrm{NaOH}\). (a) Write an equation for these reactions. (b) In a certain experiment, \(20.00 \mathrm{~mL}\) of \(0.0800 \mathrm{M} \mathrm{HCl}\) were added to a \(0.1022-\mathrm{g}\) sample of \(\mathrm{MCO}_{3}\). The excess HCl required \(5.64 \mathrm{~mL}\) of \(0.1000 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the molar mass of the carbonate and identify \(\mathrm{M}\).

Describe a simple test that would enable you to distinguish between \(\mathrm{AgNO}_{3}(s)\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(s)\).

Both \(\mathrm{KCl}\) and \(\mathrm{NH}_{4} \mathrm{Cl}\) are white solids. Suggest one reagent that would enable you to distinguish between these two compounds.

How many milliliters of \(1.0 \mathrm{M} \mathrm{NaOH}\) must be added to \(200 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{NaH}_{2} \mathrm{PO}_{4}\) to make a buffer solution with a pH of \(7.50 ?\)

A sample of \(0.1276 \mathrm{~g}\) of an unknown monoprotic acid was dissolved in \(25.0 \mathrm{~mL}\) of water and titrated with \(0.0633 \mathrm{M} \mathrm{NaOH}\) solution. The volume of base required to reach the equivalence point was \(18.4 \mathrm{~mL}\). (a) Calculate the molar mass of the acid. (b) After \(10.0 \mathrm{~mL}\) of base had been added to the titration, the \(\mathrm{pH}\) was determined to be 5.87 . What is the \(K_{\mathrm{a}}\) of the unknown acid?
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