Barium nitrate, Ba NO

Find the ionic strength of (i) 0.05 molal sodium sulfate (Na,SO ) solution, and (ii) 0.25 molal nitric acid (HNO,) and 0.4 molal barium nitrate (Ba(NO,) ) together ill one solution. 

When concentrated aqueous solutions of barium nitrate, Ba(NO )2, and ammonium iodate, NH4I03, are mixed, insoluble barium iodate, Ba(I03)2, forms. The chemical equation for the precipitation reaction is... 

Barium Nitrate—Ba(NO,), —260.8—is prepared by n utralizing HNO, with BaOO,. It forms octahedral crystals, soluble in H,0. 

Barium nitrate, Ba(N03)2, is a colorless, crystalline material with a melting point of 865 K. Ba( NO2) 2 and O2 are producedin the low-temperature region, and Ba(N02) 2 decomposes to produce BaO, N O, and NO. in the high-temperature region according to ... 

Potassium chloraie KClOj, icing sugar, barium nitrate Ba(NOi)>, strontium nitrate Sr(NO ) , concentrated sulfuric acid, sodium nlirate NaNO. ... 

Samples of dry solid potassium sulfate, K2SO4, and dry solid barium nitrate, Ba(N03)2, can be mixed with no appreciable reaction occurring for several years. But if aqueous solutions of the two are mixed, a reaction occurs rapidly, forming a white precipitate of barium sulfate. 

In fireworks, barium nitrate (Ba(N03)2) imparts the color green. Strontium chloride (SrCl2) imparts unique shades of red and purple for which there are no substitutes. Barium nitrate is also used in infrared flares, and various strontium and barium compounds are used in small-arms tracers. 

Because KCl is a strong electrolyte, it undergoes complete dissociation in solution. Thus, a 1 M KCl solution contains 1 mole of K ions and 1 mole of Cl ions, and no KCl units are present. The concentrations of the ions can be expressed as [K ] = 1 M and [CF] = 1 M, where the square brackets [ ] indicate that the concentration is expressed in molarity. Similarly, in a 1 Af barium nitrate [Ba(N03)2] solution... 

Calcium nitrate Ca(N03)2, magnesium nitrate Mg(N03)2, barium nitrate Ba(N03)2 and bismuth nitrate Bi(N03)2, whether dry or in solution, have no action on aluminium. In a solution of 600 g-l calcium nitrate Ca(N03)2, the decrease in thickness of 3003 is below 0.1 mm per year. 

Barium nitrite [13465-94-6] Ba(N02)2, crystallines from aqueous solution as barium nitrite monohydrate [7787-38-4], Ba(N02)2 H2O, which has yellowish hexagonal crystals, sp gr 3.173, solubihty 54.8 g Ba(NO2)2/100 g H2O at 0°C, 319 g at 100°C. The monohydrate loses its water of crystallization at 116°C. Anhydrous barium nitrite, sp gr 3.234, melts at 267°C and decomposes at 270 °C into BaO, NO, and N2. Barium nitrite may be prepared by crystallization from a solution of equivalent quantities of barium chloride and sodium nitrite, by thermal decomposition of barium nitrate in an atmosphere of NO, or by treating barium hydroxide or barium carbonate with the gaseous oxidiation products of ammonia. It has been used in diazotization reactions. 

Barium nitrate oxidizer, Ba(NO 3) 2 Potassium nitrate oxidizer, KNO3... 

V)Analysis of Mixtures Containing Lead Azide, Barium Nitrate, Basic Lead Styph-nate and Antimony Sulfide. As an example of such mixts may be cited the NOL No 130 Primer Mixture used in T—32E1 and M47 Detonators LA(dextrinated) 20.0, Ba(NOs)2 20.0, LSt (basic) 40.0, tetracene 5.0, St Sb,S, 15.0/5, Its max moisture content is 0.3%, The method of analysis of such mixts was developed at PicArsn by J.Campisi, ChemLabRept 52—HI—2114(1952) and was incorporated in the Purchase Descriptions PA—PD—202(Rev 1)(1952) and PA-PD-124 (1953)... 

Ionic compounds containing polyatomic ions (Section 2.8) are named in the same way as binary ionic compounds First the cation is identified and then the anion. For example, Ba(N03)2 is called barium nitrate because Ba2+ is the cation and the N03 polyatomic anion has the name nitrate. Unfortunately, there is no systematic way of naming the polyatomic ions themselves, so it s necessary to memorize the names, formulas, and charges of the most common ones listed in Table 2.3. The ammonium ion (NH4+) is the only cation on the list all the others are anions. 

A mixed convention will be employed in this chapter as an aid to indicate whether a given compound may be written in the ionized form. Thus, Ba (N03)2 should indicate to the student that barium nitrate has the overall composition of Ba(N03)2, that it is soluble and ionized, and that either the barium ion, Ba, or the nitrate ion, NO, may be written separately if desired. The absence of an ionic notation, as in AS2S5, means that only the neutral formula of the whole compound should be used. This mixed convention will not be uniformly used in subsequent chapters. Experienced chemists may write Ba(N03)2 in a reaction in aqueous solution, recognizing the ionic character of this salt even without an explicit ionic notation. 

The designation BeL(NO )2(aq) means that barium nitrate (a white soiid) has been dissolved in water. Note from its formula that barium nitrate contains the Ba " and N03 ions. In virtually every case when a solid containing ions dissolves in water, the ions separate and move around independently. We say that the ions of the solid dissociate when the solid dissolves in water. That is, Ba(N03)2(uij) does not contain Ba(N03)2 units. Rather, it contains separated Ba " " and N03 ions. In the solution there are two N03 ions for every Ba " " ion. Chemists know that separated ions are present in this solution because it is an excellent conductor of electricity (see Figure 8.2). Pure water does not conduct an electric current. Ions must be present in water for a current to flow. 

It should be observed that mixtures which evolve sulfur as diatomic gas often show large spritzels with the blue flame typical of burning sulfur. Conversely, mixtures which tend to evolve sulfur as monoatomic gas often show no visible flame, but SO2 can be detected a few inches from the burning material as monoatomic sulfur combines with atmospheric oxygen. Burning the comps which produce monoatomic sulfur in quartz tubes with inert atmosphere, the sulfur will be recovered as the element. The barium nitrate formulation produces only BaS and is energetic enough to produce monoatomic sulfur. 

Write the net ionic equation for the reaction of aqueous ammonium sulfate and aqueous harium nitrate to produce a precipitate of barium sulfate. The balanced formula equation is iNH )2SO iaq) + Ba NO iaq) — 2NH4N03( qf) + BaS04(s)... 

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