Lithium phosphate , solubility

We calculate the solubility of lithium phosphate, s, as a molarity. We then use the solubility equation to (1) relate the concentrations of the ions and (2) write the Ksp expression. 

Sodium phosphate solution partial precipitation of lithium phosphate, Li3P04, in neutral solutions the precipitate is more readily obtained from dilute solutions on boiling. Precipitation is almost complete in the presence of sodium hydroxide solution. The precipitate is more soluble in ammonium chloride solution than in water (distinction from magnesium). 

Lithium phosphate is a white -r,vntullilu powder which in sololdc in acids lint difficultly soluble in water. 

Phosphorus species. Soluble phosphates precipitate lithium phosphate, more soluble in NH4CI than in H2O alone (distinction from Mg ). In dilute solutions the phosphate is not precipitated until the solution is boiled. The sensitivity of the test is increased by adding NaOH, forming a double phosphate of Na and Li. The phosphate dissolved in HCl is not at once reprecipitated on neutrahzation with NH3 (distinction from at least Ca " through Ra ty. Ethanol promotes precipitation. 

PRACTICE EXAMPLE B A handbook lists the aqueous solubility of lithium phosphate at 18°C as 0.034g Li3P04/100 mL soln. What is the fC p of Li3P04 at 18 °C ... 

The elements have remarkably low specific gravity, and a high atomic volume (q.v.). The oxides and hydroxides are markedly basic they do not exhibit acidic qualities. The physical properties of the salts—solubility in water, molecular volume, optical properties, and the variation in the form of the crystals show the same order of variation as the atomic weights of the elements. Lithium differs in mafiy respects from the other members of the family. The salts of the alkali metals —nitrates, chlorides, sulphides, sulphates, phosphates, carbonates, etc.—are nearly all soluble in water, although lithium, carbonate, phosphate, and fluoride are very... 

H. Stamm also measured the solubilities of the salts of the alkalies in liquid ammonia —potassium hydroxide, nitrate, sulphate, chromate, oxalate, perchlorate, persulphate, chloride, bromide, iodide, carbonate, and chlorate rubidium chloride, bromide, and sulphate esesium chloride, iodide, carbonate, and sulphate lithium chloride and sulphate sodium phosphate, phosphite, hypophosphite, fluoride, chloride, iodide, bromate, perchlorate, periodate, hyponitrire, nitrite, nitrate, azide, dithionate, chromate, carbonate, oxalate, benzoate, phtnalate, isophthalate ammonium, chloride, chlorate, bromide, iodide, perchlorate, sulphate, sulphite, chromate, molybdate, nitrate, dithionate, thiosulphate, persulphate, thiocyanate, phosphate, phosphite, hypophosphite, arsenate, arsenite, amidosulphonate, ferrocyanide, carbonate, benzoate, methionate, phenylacetate, picrate, salicylate, phenylpropionate, benzoldisulphonate, benzolsulphonate, phthalate, trimesmate, mellitate, aliphatic dicarboxylates, tartrate, fumarate, and maleinate and phenol. 

Solubility The phosphates of the alkali metals, with the exception of lithium, and of ammonium are soluble in water the primary phosphates of the alkaline earth metals are also soluble. All the phosphates of the other metals, and also the secondary and tertiary phosphates of the alkaline earth metals are sparingly soluble or insoluble in water. 

OH, S", C03", and P04 ", or with anions of medium strength, such as the halogens, are characterized by their ready solubility, with the exception of the carbonate and phosphate of lithium (pp. 74 and 76). The corresponding salts of the metals of the copper group are insoluble, with the exception of the cupric and auric halides (pp. 273 and 342). 

The flame coloration and the spectrum (p. 54) afford delicate tests for the presence of lithium. From solutions which are not too dilute it can be precipitated as phosphate, fluoride, or carbonate. Like sodium, it yields an antimonate of slight solubility, but in contradistinction to potassium its platino-chloride and hydrogen tartrate are soluble. 

Deoxygenation of phenols may be achieved by reduction of aryl diethyl phosphates with lithium or sodium in liquid ammonia." A recent application of the methodology is outlined in Scheme 43." The reaction works well with a variety of substituted phenols, but not with dihydric phenols or naphthols. The alternative reduction of aryl sulfonates has also been examined, but the limited solubility of these derivatives can present difficulties. 

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