Why do you need to know the ion concentrations when precipitation occurs?
479476
You need to know concentrations to determine the amount of substance that precipitates out by using solubility products. In this case the precipitate will be CaSO4, so the solubility product will be given by:\n\nk=[Ca(+2)]*[SO4(-2)]\n\nWhere k is the equilibrium constant (probably a given), and [Ca(+2)] & [SO4(-2)] are the concentrations of Ca(+2) and SO4(-2) in the solution. Any amounts greater than the equilbrium concentration will precipitate out as a solid.
634552
an ion with both acidic and basic part
724819
To determine the concentration of a reagent.
91636
Based on one of my chem classes:\n\nA reaction goes to completion if:\n>there's a precipitate.\n>one of the product is a gas and the system isn't isolated.\n>conditions are kept constant.\n\nI think the 'precipitation' you are asking is a 'precipitation reaction'. This effect is useful in many industrial and scientific applications whereby a chemical reaction may produce a solid that can be collected from the solution by various methods (e.g. filtration, decanting, centrifuging). Precipitation from a solid solution is also a useful way to strengthen alloys.
975119
Okay now you're getting into physics or something here, so I have absolutely no idea!\n\nBut it might have something to do with.......oh yeah, ions, that's it! Ions......
864409
All four ions involved would diffuse and, at some point, the sulphate and barium ions would meet and produce an obvious white band. Since the ions would not move at the same speed the band would not e halfway between the points where the samples were added.
147985
it is when a material is caused to drop out of solution, think about a salt water solution and then you make the salt to come out of the solution. i could give you a chemial reaction equation for a different example, but just imagine that you dissolved salt into water (any solution) and then you wanted to make that salt come back out of the water again. you could add another chemical to make that happen, and when you did, the salt would drop out of the water along with whatever chemical you added to make the reaction occur.  hope that helps!
716763
depending on what kind of ions, you can use a spectrometer.\n\nOr a titration with a color change to see how much of a reactant it takes to consume all of the ions.
164971
BaCl2 + Na2SO4 --> BaSO4 + 2NaCl is the chemical reaction. \nNet ionic equation: Ba(2+) + SO4(2-) --> BaSO4 \nTotal ionic equation: Ba2+ 2Cl- + Na+ + 2SO4(2-) --> BaSO4(s) + 2Na+ + Cl-\nBarium sulfate is a classic precipitate.  \n\nAll of the masses of these compounds can be calculated by adding the individual ions' masses together, which is the same as atomic masses on a periodic table.   \nBarium chloride: 208.25 g/mol\nSodium sulfate: 142.04 g/mol (anhydrous)\nBarium sulfate: 233.43 g/mol \nSodium chloride: 58.4 g/mol
834819
Without knowing what reaction you're trying to get, or everything else present, thats a difficult question to answer.\n\nIn a sense. you're forming a silver nitrate solution, but you have to knw all the spectator ions to know what reaction will actually occur.  The silver cation in solution needs to have a anion associated with it.  \n\nThe purpose may also have something to do with the variable solubilities of the silver compound that may be formed.  \n\nAnother potential reaction involves the nitrate as an oxidizing agent.
1027970
Simply that during the induction period, the actual concentrations may not be 100% homogeneous and the rates will increase of decrease from theoretical.  This is much more important with macromolecules, but can be seen in other cases.  See\n\nwww.uem.mz/faculdade/ciencias/ ciencias_revista/textos/elalves.pdf\n\ndx.doi.org/10.1063/1.1954769\n\nwww.platinummetalsreview.com/ dynamic/article/view/50-2-54-63\n\nwww.citadel.edu/chemistry/scas2005.pdf
1110554
I believe you mean "titration".\n\nTitration is a way to measure the concentration of a dissolved substance by seeing exactly how much of a neutralizing substance you have to add to the mixture to bring it to a neutral concentration.  \n\nThis is usually done by adding drops of a neutralizing substance of known strength until the original solution becomes neutral.  By calculating exactly how much neutralizer was needed, you know the strength of the original mixture.
561756
Do you perhaps mean DETECTS precipitation??\n\nRADAR
139481
What I think you want is how do you split ionic compounds into ions.  Solutions!\n\nWhen you have an ionic compound, like salt (NaCl) you can split the compound into its ions by dissolving it in water.\n\n     (H2O)\nNaCl(s) ----->  Na+(aq) + Cl-(aq)\n\nThe (s) means solid, cause salt is a solid.  When you put it in water, it changes from (s) to (aq) which means aqueous.  Aqueos basically means that the substance is an ion in a water solution.\n\nHope this helps.
766145
It depends on how far away from the noble gases they are. Like anything in gourp IA would be 1+, IIA 2+ etc, then when theyre closer to the right then its like VIIA 1-, VIA 2-\n\nTransition metals are different because they form multiple ions. It would indicate what the charge is.
444914
Q which is the reaction quotient is the ratio of concenctration of reactants to concention of products each concentrations raised to their respective stiochiometry (the number infront of the products or reactants when u balance the equation) at any given time other than equilibrium. Unlike Ksp which is solubility product is the same except it's at equilibrium.\nHowever, Q can help to to find out whether or not there is a precipitate will be formed so if Qsp is < Ksp no precipitate but if Qsp > Ksp a precipitate is formed  and will continue until the concentration of ions remaining in solution satisfy Ksp\nif u don't understand maybe u can send a e-mail and i can explain what u don't understand
1092099
to determine whether an acid or a base is soluble in say the universal polar solvent water, u should be knowing whether the substance is strong or weak\nnow bases like NaOH, CsOH, RbOH, Mg(OH)2 are strong bases and in solution they give us the cations and anions(mostly the hydroxyl grp)\nbases like Be(OH)2, Fe(OH)2 or 3, Cu(OH)2 or any of their oxides are weak and hence in solution they do not undergo complete dissociation and most of these are insoluble\nso in case ur not in a lab, the only way is to identify their degree of weakness