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Chapter 4: Problem 60

A sample may contain any or all of the following ions: \(\mathrm{Hg}_{2}^{2+}\) \(\mathrm{Ba}^{2+}\) and \(\mathrm{Mn}^{2+}\) a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution. b. No precipitate formed when an aqueous solution of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ was added to the sample solution. c. A precipitate formed when the sample solution was made basic with NaOH. Which ion or ions are present in the sample solution?

Short Answer

Expert verified
Based on the reactions with NaCl, Na2SO4, and NaOH, the only ion present in the sample solution is \(Mn^{2+}\).

Step by step solution

01

Analyzing reaction with NaCl

When NaCl is added to the sample, it dissociates into Na+ and Cl- ions. If any of the cations (Hg2^2+, Ba^2+, or Mn^2+) form an insoluble chloride salt with Cl-, a precipitate should form. In this case, no precipitate is formed, which means that Hg2^2+ can't be present in the sample as Hg2Cl2 is insoluble in water.
02

Analyzing reaction with Na2SO4

When Na2SO4 is added to the sample, it dissociates into 2 Na+ and SO4^2- ions. If any of the remaining cations (Ba^2+ or Mn^2+) form an insoluble sulfate salt with SO4^2-, a precipitate should form. Since no precipitate is formed, this means that Ba^2+ can't be in the sample, as BaSO4 is insoluble in water.
03

Analyzing reaction with NaOH

When NaOH is added to the sample, it dissociates into Na+ and OH- ions. If any of the remaining cations (Mn^2+) form an insoluble hydroxide salt with OH-, a precipitate should form. A precipitate is formed in this case, which means that Mn^2+ must be present in the sample as Mn(OH)2 is insoluble in water.
04

Conclusion

Based on the reactions with NaCl, Na2SO4, and NaOH, the only ion present in the sample solution is Mn^2+.

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Most popular questions from this chapter

Using the general solubility rules given in Table 4.1, name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions. a. chloride ion \(\quad\) d. sulfate ion b. calcium ion \(\quad\) e. mercury \((1)\) ion, \(\mathrm{Hg}_{2}^{2+}\) c. iron(M) ion \(\quad\) f. silver ion

What mass of solid AgBr is produced when 100.0 \(\mathrm{mL}\) of 0.150 \(\mathrm{MAgNO}_{3}\) is added to 20.0 \(\mathrm{mL}\) of 1.00 $\mathrm{M} \mathrm{NaBr} ?$

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) A 0.205-g sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The BaSO\(_{4}\) that is formed is filtered, dried, and weighed. Its mass is 0.298 g. What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

Balance the following oxidation–reduction reactions that occur in basic solution. a. $\mathrm{Cr}(s)+\mathrm{CrO}_{4}^{2-}(a q) \rightarrow \mathrm{Cr}(\mathrm{OH})_{3}(s)$ b. $\mathrm{MnO}_{4}^{-}(a q)+\mathrm{S}^{2-}(a q) \rightarrow \mathrm{MnS}(s)+\mathrm{S}(s)$ c. $\mathrm{CN}^{-}(a q)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{CNO}^{-}(a q)+\mathrm{MnO}_{2}(s)$

One of the classic methods for determining the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing the periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.
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