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Chapter 16: Q10P (page 391)

What is a Jones reductor and what is it used for?

Short Answer

Expert verified

Jones reductor is a reducing substance that can be used to lower the oxidation state of a metal ion in an aqueous solution

Step by step solution

01

Definition of Jones reductor.

A device that is used to chemically decrease liquids, such as ferric salt solutions, by pouring the solution into a vertical tube containing granular zinc.

02

Determine the Jones redactor and uses.

Jones reductor is a column that contains zinc coated with zinc amalgam (solution with mercury).
Analyte is pre-reduced by passing through the Jones reductor with sulfuric acid as a solvent Analytes that can be reduced with Jones reductor are ${Fe}^{3 +}, {Sn}^{4 ‐} and {MnO}_{4}^{‐}$ Uses:

A Jones reductor is a reducing substance that can be used to lower the oxidation state of a metal ion in aqueous solution.
A zinc amalgam is the active ingredient. It can be used to make solutions of ions that are promptly oxidised when exposed to air, such as Chromium(II), ${Cr}^{2 ι}$ , and uranium(III), $U^{3 +}$ .

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Most popular questions from this chapter

Write balanced reactions for the destruction of $S_{2} O_{8}^{2 ‐}, {Ag}^{3 +} and H_{2} O_{2}$ ,by boiling.

Why is iodine almost always used in a solution containing excess $l^{-}$ ?

Aqueous glycerol solution weighing 100.0m gwas treated with 50.0 mL of 0.083 7 M ${Ce}^{4 +}$ in 4 MHCI $O_{4}$ at $60 °$ for15minto oxidize glycerol to formic acid.

${CH}_{2} - CH - {CH}_{2} | | | OH OH OH$ ${HCO}_{2} H$

Glycerol Formic acid

FM92.095

The excess ${Ce}^{4 +}$ required 12.11mL of 0.044 8 MF $e^{2 +}$ to reach a ferroin end point. Find wt%glycerol in the unknown.

A 25.00mL volume of commercial hydrogen peroxide solution was diluted to 250.0mL in a volumetric flask. Then 250.0 of the diluted solution were mixed with 200mL of water and 20mLof $3 {MH}_{2} {SO}_{4}$ and titrated with $0.02123 {MKMnO}_{4}$ . The first pink color was observed with 27.66mL of titrant. A blank prepared from water in place of $H_{2} O_{2}$ required 0.04Ml to give visible pink color. Using the $H_{2} O_{2}$ reaction in Table16 - 3, find the molarity of the commercial $H_{2} O_{2}$ .

Winkler titration for dissolved $O_{2} .$ Dissolved $O_{2}$ is a prime indicator of the ability of a body of natural water to support aquatic life. If excessive nutrients run into a lake from fertilizer or sewage, algae and phytoplankton thrive. When algae die and sink to the bottom of the lake, their organic matter is decomposed by bacteria that consume $O_{2}$ from the water. Eventually, the water can be sufficiently depleted of $O_{2}$ so that fish cannot live. The process by which a body of water becomes enriched in nutrients, some forms of life thrive, and the water eventually becomes depleted of $O_{2}$ is called eutrophication. One way to measure dissolved $O_{2}$ is by the Winkler method that involves an iodometric titration: 35

Dissolved oxygen or biochemical oxygen demand

1. Collect water in a $~ 300 m L$ bottle with a tightly fitting, individually matched ground glass stopper. The manufacturer indicates the volume of the bottle $(\pm 0.1 mL)$ with the stopper inserted on the bottle. Submerge the stoppered bottle at the desired depth in the water to be sampled. Remove the stopper and fill the bottle with water. Dislodge any air bubbles before inserting the stopper while the bottle is still submerged.

2. Immediately pipet 2.0 mL of $2.15 M {MnSO}_{4}$ and 2.0 mL of alkali solution containing $500 g NaOH / L, 135 g NaL / L$ and $10 g N a N_{3} / L$ (sodium azide). The pipet should be below the liquid surface during addition to avoid introducing air bubbles. The dense solutions sink and displace close to 4.0 Ml of natural water from the bottle. 3. Stopper the bottle tightly, remove displaced liquid from the cup around the stopper, and mix by inversion. $O_{2}$ is consumed and $M n (O H)_{3}$ precipitates:

$4 M n^{2 +} + O_{2} + 8 O H^{-} + 2 H_{2} O \to 4 M n (O H)_{3} (s)$

Azide consumes any nitrite $(N O_{2}^{-})$ in the water so that nitrite cannot subsequently interfere in the iodometric titration:

$2 N O_{2}^{-} + 6 N_{3}^{-} + 4 H_{2} O \to 10 N_{2} + 8 O H^{-}$

4. Back at the lab, slowly add 2.0 mL of $18 M H_{2} S O_{4}$ below the liquid surface, stopper the bottle tightly, remove the displaced liquid from the cup, and mix by inversion. Acid dissolves which reacts quantitatively with

$2 Mn (OH)_{3} (s) + 3 H_{2} {SO}_{4} + 3 I^{-} \to 2 {Mn}^{2 +} + I_{3}^{-} + 3 {SO}_{4}^{2 -} + 6 H_{2} O$

5. Measure 200.0 mLof the liquid into an Erlenmeyer flask and titrate with standard thiosulfate. Add 3mL of starch solution just before the end point and complete the titration.

A bottle of 297.6 mLof water from a creek at $0 ° C$ in the winter was collected and required 14.05 mL 10.22 mM thiosulfate.

(a) What fraction of the 297.6 mL sample remains after treatment with and alkali solution?

(b) What fraction remains after treatment with $H_{2} S O_{4}$ ? Assume that $H_{2} S O_{4}$ sinks into the bottle and displaces 2.0 mL of solution prior to mixing.

(c) How many mL of the original sample are contained in the 200.0 mLthat are titrated?

(d) How many moles of $l_{3}^{-}$ are produced by each mole of $O_{2}$ in the water?

(e) Express the dissolved $O_{2}$ content in (f) Pure water that is saturated with $O_{2}$ contains $14.6 m g O_{2} / L a t 0 ° C .$ What is the fraction of saturation of the creek water with $O_{2}$ ?

(g) Write a reaction of $N O_{_{2}}^{-}$ with $l^{-}$ that would interfere with the titration if $N_{3}^{-}$ were not introduced. See Table 16-5.

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