I believe that would be Barium nitrate or Ba(NO3)2
It is Barium nitrate Ba(NO3)2
The formula for the nitrate ion is NO3 -1.
Fe2+ and NO3- ions will combine to form ferrous nitrate with the formula, Fe(NO3)2
Formula: Pb(NO3)4
The chemical formula of iron nitrate are Fe(NO3)2 and Fe(NO3)3.
The chemical formula of stannous nitrate is Sn(NO3)2.
Ba2(SO4)2
Ba2+
This is not an equation but the chemical symbol of the cation: Ba2+.
Formula: Ba2+
Ba2+
NH4+ and NO3- don't react, Only SO42- and Ba2+ do so by forming precipitate: SO42- + Ba2+ --> (BaSO4)s
Ba2+ and Cl-.
The formula for the nitrate ion is NO3 -1.
Solubility is normally measured as the amount of a substance that can dissolve in a solvent and is measured in units of (amount of substance)/(volume of solvent).Barium nitrate, for example, has a solubility of 0.105 moles/litre in water, or it can also be expressed as 27.3g/litre.The solubility product is an equilibrium constant for the process:salt (solid) cations (aq) + ions (aq)As the activity of the solid is taken to have a value of 1, the solubility product is the result of multiplying the concentrations of the dissolved ions at the solid's maximum solubility.The solubility product (Ksp) can be thought of as a more general expression of the solubility of a substance. To obtain the solubility product, we multiply the concentrations (mol/litre)* of ALL the ions that result from the substance dissolving when they are at their maximum concentration.In the case of barium nitrate, we have:Ba(NO3)2 ---> Ba2+ + NO3- + NO3-So the solubility product , Ksp = [Ba2+][NO3-][NO3-] = [Ba2+][NO3-]2The experimentally determined value of the solubility product for Barium Nitrate is 4.64×10-3.For barium nitrate dissolving in pure water, [NO3-]= 2[Ba2+], so we can writeKsp = [Ba2+][NO3-]2 = 4[Ba2+]3 = 4.64×10-3Solving this, [Ba2+] = 0.105 mol/litreAs [Ba2+] equals the concentration of barium nitrate that is dissolved, this is the solubility of barium nitrate in pure water.The usefulness of the solubility product is that we can use it to look at the effects of ions from other sources than the salt. For example, if we try to dissolve barium nitrate in 10 molar nitric acid, we use the same expression as before:Ksp = [Ba2+][NO3-]2 = 4.64×10-3But this time [NO3-] = 10 mol/litre (approx), as that is already in solution, so:100 [Ba2+] = 4.64×10-3[Ba2+] = 4.64×10-5The solubility of barium nitrate in 10M nitric acid is 4.64×10-5 Mol/litre, MUCH less than its solubility in pure water, and not something that you could determine from the solubility alone.*Strictly, we should use activity rather than concentration.
The molecular formula is Co(NO3)2Co(NO3)2
Zn(NO3)2 + 2Ag ---> Zn + 2AgNO3
Formula: NO3-