Silver nitrate reaction with copper

Write the net ionic equation for (a) the reaction of copper solid with silver nitrate to form copper(II) nitrate and silver solid, and (b) the reaction of copper solid with potassium nitrate that would form copper(II) nitrate and potassium solid. 

The presence of chloro-derivatives is detectable by the reaction with copper oxide (see p. 305) or by boiling a little of the solvent with alcoholic potash potassium chloride, readily detected with silver nitrate, is thus formed. 

When silver nitrate (AgNOg) or copper (1) chloride (CU2CI2) in HH3 solution is added to R — C C — H, copper acetylide or silver acetylide salts are formed. These are insoluble in water, and when dried and heated, explode. This reaction is useful to differentiate terminal allies from non-terminal ones. Terminal alkynes are the ones with the triple bond at the end of the chain. 

ACETYLENOGEN (75-20-7) Contact with water, moist air, steam, alcohols forms explosive acetylene gas, corrosive calcium hydroxide, and heat. Violent reaction with acid, acid fumes, copper salts, strong oxidizers (bromine, chlorine, iodine, etc.), iron trichloride, tin dichloride, silver nitrate. Incompatible with oxidizers, hydrogen chloride, methanol, copper salt solutions, lead fluoride, magnesium, selenium, sodium peroxide, stannous chloride, sulfur. 

Figure 8.17 The reaction between copper and a solution of silver nitrate, (a) A copper strip is placed in a clear, colorless solution of silver nitrate, (b) After about an hour at room temperature, the products of the reaction become visible. The copper strip is covered with solid silver metal. The solution becomes blue because of the presence of hydrated copper(II) ions. 

These reactions can be viewed as a competition between two kinds of atoms (or molecules) for electrons. Equilibrium is attained when this competition reaches a balance between opposing reactions. In the case of reaction (3), copper metal reacting with silver nitrate solution, the Cu(s) releases electrons and Ag+ accepts them so readily that equilibrium greatly favors the products, Cu+2 and Ag(s). Since randomness tends to favor neither reactants nor products, the equilibrium must favor products because the energy is lowered as the electrons are transferred. If we regard reaction (5) as a competition between silver and copper for electrons, stability favors silver over copper. 

Penta-1,3-diyne (Methyldiacetylene). CH3.CiC.CiCH mw 65.10 OB to C02 —294.93% liq mp —4.5 to -38.5° bp 76-77° (explds at atm press), 45° at 140mm d 0.7909 g/cc at 20/4° RI 1.4762 (Ref 3) and 1.4817 (Ref 1). Sol in ethanol and petr with a bp > 180°. Prepn is by reacting monosodium-acetylenide with dichloromethane in liq ammonia at 20 to 40°, followed by treatment with ammonium chloride. The product is stable in the dark at -35° but polymerizes readily at above —20° in the light. Penta-1,3-diyne forms two expl salts Copper penta-1,3-diyne, CuCsH3, dark yel ndls/by reaction with CuCl, explds on shock or by rubbing and Silver penta-1,3-diyne, yel-brn ndls, by reaction with aq silver nitrate in ammonium hydroxide, a v expl compd Refs 1) Beil 1, [247], 1057 <1117)... 

Other electrolytes, such as sodium sulfate or potassium nitrate, could be chosen for the salt bridge. Neither of these electrolytes interferes in the cell reaction. Silver nitrate, AgN03(aq), would be a poor choice for the salt bridge, however. Positive silver ions would migrate into the half-cell that contains the cathode. Zinc displaces both copper and silver from solution, so both copper(n) ions and silver ions would be reduced at the cathode. The copper produced would be contaminated with silver. 

The action of an active intermediate oxidation product would explain another feature of the reaction. The reduction of silver ions by hydrazine is extremely sensitive to the presence of small amounts of copper. For example, a solution containing a mixture of silver nitrate, sodium sulfite and hydrazine which normally showed no sign of reduced silver for several minutes underwent almost immediate reaction when merely stirred with a clean copper rod. In the presence of gum arabic as stabilizer, streamers of colloidal silver passed out from the copper surface. Similarly, the addition of small amounts of cupric sulfate to a hydrazine solution eliminated the induction period of the reaction with silver chloride. 

Diammino-silver nitrate forms glistening rhombic or prismatic crystals which blacken on exposure to light. It is fairly stable, and may be heated to 100° C. without loss of ammonia. Further heating causes it to decompose, and finally to melt with evolution of nitrogen and ammonia, leaving a residue of metallic silver and ammonium nitrate. It is soluble in water, but partial dissociation takes place so that the solution is alkaline in reaction, and it therefore yields a precipitate of silver chloride and soluble chlorides. Certain of the metals—for example, zinc, cadmium, and copper—quickly reduce the ammine in solution to metallic silver. 

Remove the bath with water, remove the rubber tube with a bent glass tip from the end of the apparatus, and pass the carbon(II) oxide through ammonia solutions of silver nitrate and copper(I) chloride poured into test tubes. What happens Does the carbon(II) oxide exhibit the same properties in these reactions How can one prove that carbon(II) oxide will evolve when the formed complex compound of copper(I) is heated ... 

Cupferron (29), as the name suggests, has been applied to the analytical determination of copper and iron. In neutral solution, a white 1 1 complex with Ag1 has been obtained which reacted with Mel to give the methyl ether.292 Reaction of the related ligand (30) with silver nitrate in aqueous methanol gave a red predpitate which on further reaction with Mel gave the methyl ether in a reaction analogous to that for cupferron.293... 

Hyposulfurous acid is a powerful reducing agent, e.g., with copper sulfate forms cuprous hydride Cu H , brown precipitate, which evolves hydrogen gas and leaves copper on warning, with silver nitrate yields finely divided silver, with permanganate yields manganous compounds. Hyposulfurous acid is formed by reaction of sodium hyposuliile and an acid. 

Heavy-metal salts, particularly those of silver, mercury, and copper, catalyze SX1 reactions of alkyl halides in much the same way that acids catalyze the SN reactions of alcohols. A heavy-metal ion functions by com-plexing with the unshared electrons of the halide, thereby making the leaving group a metal halide rather than a halide ion. This acceleration of the rates of halide reactions is the basis for a qualitative test for alkyl halides with silver nitrate in ethanol solution ... 

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