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Chapter 27: Q6P (page 767)

Why is it less desirable to wash AgCl precipitate with aqueous NaNO3 than with HNO3 solution?

Short Answer

Expert verified

The AgCI precipitateHNO3 would be more desirable than withNaNO3

Step by step solution

01

Definition

It is an analytical technique that uses a precipitation reaction to separate ions from a solution. The chemical that is added to cause the precipitation is called the precipitant or precipitating agent

02

Characteristics of HNO3 and NANO3

doesn鈥檛 evaporate during drying.

evaporates during drying.

03

Washing of AgCl precipitate solution.

If we washed with AgCI precipitate with HNO3,would evaporate during drying this would leave a clean AgCI precipitate.

If we washed with AgCI precipitate with NaNO3,NaNO3,is non volatile and wouldn鈥檛 evaporate during drying this would leave a dirty AgCI precipitate.

Therefore, precipitate withHNO3 would more desirable than that NaNO3.

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Most popular questions from this chapter

A solid mixture weighing 0.5485 gcontained only ferrous ammonium sulfate hexahydrate and ferrous chloride hexahydrate. The sample was dissolved in 1MH2SO4 , oxidized to Fe3+ with H2O2, and precipitated with cupferron. The ferric cupferron complex was ignited to produce 0.1678 gof ferric oxide, Fe2O3(FM 159.69). Calculate the weight percent of Clin the original sample.

Determination of sulfur by combustion analysis produces a mixture of SO2and SO3 that can be passed through H2O2to convert both into H2SO4, which is titrated with standard base. When 6.123m g of a substance were burned, the H2SO4 required 3.01mL of0.010576MNaOHfor titration. Find wt% sulfur in the sample.

To find the Ce4+ content of a solid, 4.37 g were dissolved and treated with excess iodate to precipitate Ce(IO3)4. The precipitate was collected, washed well, dried, and ignited to produce 0.104 g of CeO2 (FM 172.114). What was the weight percent of Ce in the original solid?

1.475-g sample containing NH4Cl(FM53.491),K2CO3(FM 138.21), and inert ingredients was dissolved to give 0.100 L of solution. A 25.0-mL aliquot was acidified and treated with excess sodium tetraphenylborate,Na+B(C6H5)4-, to precipitateK+and

NH4+ions completely:

(C6H5)4B-+K+鈫�(C6H5)4BK(s)FM358.33(C6H5)4B-+NH4+鈫�(C6H5)4BNH4(s)FM337.27

The resulting precipitate amounted to 0.617 g. A fresh 50.0-mL aliquot of the original solution was made alkaline and heated to drive off all theNH3.

NH4++OH-鈫�NH3(g)+H2O

It was then acidified and treated with sodium tetraphenylborate to give 0.554 g of precipitate. Find the weight percent ofNH4ClandK2CO3in the original solid.

Why is sample dropped into the preheated furnace before the oxygen concentration reaches its peak in Figure 27-9?

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