Sodium chloride silver nitrate reaction with

The following sections are concerned with the use of standard solutions of reagents such as silver nitrate, sodium chloride, potassium (or ammonium) thiocyanate, and potassium cyanide. Some of the determinations which will be considered strictly involve complex formation rather than precipitation reactions, but it is convenient to group them here as reactions involving the use of standard silver nitrate solutions. Before commencing the experimental work, the theoretical Sections 10.74 and 10.75 should be studied. 

The monofluorophosphates can be prepared by neutralization of monofluorophosphoric acid (1). Sodium monofluorophosphate [7631 -97-2] is prepared commercially (57) by fusion of sodium fluoride and sodium metaphosphate, and the potassium monofluorophosphate [14104-28-0] can be prepared similarly. Insoluble monofluorophosphates can be readily prepared from reaction of nitrate or chloride solutions with sodium monofluorophosphate. Some salts are prepared by metathetical reactions between silver monofluorophosphate [66904-72-1] and metal chlorides. 

In Experiment 8 you determined the number of moles of silver chloride formed in the reaction of some sodium chloride with a known amount of silver nitrate. How many moles of sodium chloride reacted with the silver nitrate Compare this with the number of moles of sodium chloride you added. 

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. 

Explosive reaction with chlorosulfuric acid, hydroiodic acid, magnesium perchlorate, chromyl chloride. Forms sensitive explosive mixtures with metal halogenates (e.g., chlorates, bromates, or iodates of barium, calcium, magnesium, potassium, sodium, zinc), ammonium nitrate, mercury(1) nitrate, silver nitrate, sodium nitrate, potassium permanganate. Violent reaction or ignition with alkalies + heat, fluorine, chlorine, liquid bromine, antimony pentachloride. Reacts with hot alkalies or hydroiodic acid to form... 

The foregoing acids are crystalline solids, and in some cases may be crystallised from water. 5-Amino-2 4-dihydroxy-, 3 5-diamino-2-hydroxy-, and 4 5-diamino - 2 - hydroxyphenylarsinic acids reduce ammoniacal silver nitrate solution, the reaction being instantaneous with the latter two acids. 4-Acetylamino-8-hydroxy-2-nitrophenylarsinic acid, boiled with 2N sulphuric acid, yields 2 6-nitroaininophenol, but with potassium hydroxide the acetyl group is merely hydrolysed reduction of the acid with ferrous chloride produces the corresponding diamine. 3-Amino-4-hydroxyphenylarsinic acid tends to oxidise when recrystaUised from water, and when a cooled solution of the acid in 5 per cent, sodium hydroxide solution is treated with carbonyl chloride, it gives 1 2-dihydrobenzoxazolone-4-arsinic acid. 8-Amino-4-hydroxy-phenylarsinic acid also yields a number of N-acyl derivatives (see details on p. 296), the most important of which is the 8-acetylamino-compound,... 

MERCURIC BICHLORIDE (7487-94-7) HgClj Contact with acids or acid fumes evolves chloride and mercury vapors. Possible violent reaction with chlorine nitrate, sodium acetylide. Incompatible with albumin, alkalis, alkaloid salts, anhydrous ammonia, antimony, arsenic, borax, bromides, carbonates, chloric acid, copper, formates, gelatin, hydrozoic acid, infusions of cinchona, iron, lead and silver salts, lime water, light metals, methyl isocyanoacetate, oak bark or senna, phosphates, potassium, reduced iron, sodiiun, sodium peroxyborate, sulfides, sulfites, tannic acids, trinitrobenzoic acid, urea nitrate, vegetable astringents. Decomposed by sunlight. On small fires, use water spray, fog, foam, dry chemical powder, or CO2 extinguishers. 

Potassium nitrite solution on warming this reagent with a solution of the chlorate, the latter is reduced to a chloride, which may be identified by adding silver nitrate solution after acidification with dilute nitric acid. The nitrite must, of course, be free from chloride. A solution of sulphurous acid or of formaldehyde (10%) acts similarly. Excellent results are obtained with zinc, aluminium or Devarda s alloy and sodium hydroxide solution (see under nitrates. Section 4.18, reaction 4) the solution is acidified with dilute nitric acid after several minutes boiling and silver nitrate solution added. 

Since it is useful to know what state each reagent is in, we often designate the state in the equation. The modern practice is to add to the formula the designation in parentheses (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solution. Thus, a reaction of silver nitrate with sodium chloride in aqueous solution, yielding solid silver chloride and aqueous sodium nitrate, may be written as... 

In Nebraska, state regulations require that the chemical makeup of animal feed sold in the state be accurately reflected on the labels found on the feed bags. The Nebraska State Agriculture Laboratory is charged with the task of performing the analytical laboratory work required. An example is salt (sodium chloride) content. The method used to analyze the feed for sodium chloride involves a potentio-metric titration. A chloride ion-selective electrode in combination with a saturated calomel reference electrode is used. After dissolving the feed sample, the chloride is titrated with a silver nitrate standard solution. The reaction involves the formation of the insoluble precipitate silver chloride. The electrode monitors the decrease in the chloride concentration as the titration proceeds, ultimately detecting the end point (when the chloride ion concentration is zero). 

Effect of Light on the Decomposition of Silver Chloride. Introduce 2 ml of a 0.1 W silver nitrate solution into a test tube and add dropwise such an amount of a saturated sodium chloride solution that will be sufficient for the complete precipitation of the silver as -a chloride. Rapidly filter out the precipitate, rinse it with water and put it on two watch glasses. Place one glass with the precipitate in a dark cupboard, and leave the other at a window in daylight. In an hour, compare the colour of the precipitates and explain the phenom->ena you observe. How does light affect the reaction After the experiment, put the precipitates containing a silver compound into he jars set aside for them. 

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