what are the various hydrated ionic conpounds?
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There are several.\n\nA few\n\n1) Copper sulphate penta hydrate (Cu SO4. 5 H2O)\n2) Ferrous sulphate hepta hydrate (Fe SO4. 7 H2O)\n3) Potash Alum (K2SO4. Al2 (SO4)3. 24 H2O)\n\nThe first two can exist in different states of hydration. The former as mono and tri hydrates also and the latter as mono, tetra and penta hydrates also.
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Ionic compound\n\n The crystal structure of NaCl, a typical ionic compoundIn chemistry, an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. The positively charged ion is usually a metal ion and the negatively charged ion is non-metallic element or molecule.\n\nIons can be single atoms, as in common table salt sodium chloride, or more complex groups such as calcium carbonate. But to be considered ions, they must carry a positive or negative charge.\n\nThus, in an ionic bond, one 'bonder' must have a positive charge and the other a negative one. By sticking to each other, they resolve, or partially resolve, their separate charge imbalances. Positive to positive and negative to negative ionic bonds do not occur. (For a real world analogy, experiment with a pair of bar magnets.)\n\nIonic compounds have strong bonds between particles and thus generally have high melting and boiling points. They have good electrical conductivity when molten or in aqueous solution. While ionic inorganic compounds are solids at room temperature and will usually form crystals, organic ionic liquids are increasingly of interest.\n\nIonic compounds also dissolve in polarised liquids, of which water is an example, while they do not dissolve in organic liquids, such as Petrol. This is the opposite of covalent compounds.\n\nWhen an ionic compound is named, the cation is named first and then the anion. When an elemental anion is named, the suffix, -ide, is added to the name of the element. There are two common types of cations: Type I and Type II. Type I cations have only one charge and their name is simply listed when the compound is named. Type II cations have more than one charge and when the ionic compound is named, a Roman numeral is used to denote the charge of the cation. In addition, there are common polyatomic anions which do not have suffixes in their name such as hypochlorite (ClO–).\n\nRetrieved from "http://en.wikipedia.org/wiki/Ionic_compound"
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1. Molarity = concentration and it expressed as mol per dm^3\n    Change the mass to mole and the 851 ml to dm^3. Then find   \n    the ratio of the number of moles to volume in dm^3\n\n2. Soluble ionic compounds breaks up the water molecules in H^+ ions and OH^- ions. Sodium carbonate give Na^+ ions and CO3^2- ions......Other ions that are present are HCO3^- ions called hydrogen carbonate ions. I have found that a solution of sodium carbonate is alkaline: implying that there are more OH^- ions to H^+ ions, due to the formation of HCO^- ions.\n3. OH^- (aq) + H^+(aq) ----> H2O (l)\n4. H^+ ions (ie. hydrogen ions), OH^- ions (ie. hydroxyl ions),\n   Ca^2+ calcium ions and Cl^- chloride ions\n5. Hydrogen ions, hydroxyl ions. ammonium ions and sulphate ions.\n6. Actually the calcium metal reacts with water to give hydrogen gas and calcium hydroxide. At the same time, calcium reacts with nitric acid to give calcium nitrate, water and brown nitrogen dioxide gas.\nHence there is no simple ionic equation for your question\nYou may want to consider this one:\nCa^0  +  2H^+   + 2OH^-  -----> H2(g)  + Ca^2+  + 2OH^-\n7. Hydrogen ions, hydroxyl ions, iron (III) ions Fe^3+  and sulphate ion SO4^2-
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H2SO4 + 2NaOH ----> 2H2O + Na2SO4\n\nYOU MUST SEPARATE AND CANCEL THE COMMON IONS (AQUEOUS ONES)
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The net ionic equation is :\n\nNH3(aq) + H2O(l)+ Cl2(g) ---> OCl-(aq) + Cl-(aq) + NH4+(aq)+ H2O(l)
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Salt, sodium chloride [NaCl]... all you need to know is on that page so I won't bother repeating it all here>>>\n\nhttp://en.wikipedia.org/wiki/Sodium_chloride
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http://www.chem1.com/CQ/ionbunk.html\n\nskim this article.
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Since the reaction is between two ionic compounds, it will be double replacement.  In that case, the positive ion of one compound switches places with the positive ion from the other.  The two products will then be sodium chloride (NaCl) and Calcium Carbonate (CaCO3).  Sodium Chloride is soluble, as are all ionic compounds with group 1 ions present, however, carbonate compounds are almost never soluble in water.  The only water-soluble carbonate compoounds that I can think of are ammonium carbonate and group 1 carbonate compounds.
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Mg2+ < Na+ < Br-\n\nIon size depends first on the main quantum number. Na and Mg both strip down to the Ne configuration, while Br takes up the Xe configuration, two main quantum numbers higher.\n\nMg2+ is smaller than Na1+ because the remaining electrons are subject to a stronger electrostatic field.\n\nThe above is true for ions in crystal lattices.\n\nNote that in watery solutions ion size has to be calculated differently when you take the hydrate shell into account. Na+ becomes Na(H2O)6(1+), and Mg2+ becomes Mg(H2O)6(2+). Bromide won't take up a regular hydrate shell.
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All ionic compounds dissociate into respective +ve and -ve ions in aquous solutions.\n\nYou possibly want to know such compounds which give both +ve and -ve ions with more than 1 charge.\n\nYes salts of all alkline earth metals (+ve2) with ions of more than one atoms (CO3,PO4 etc) having more than 1 -ve charge dissociate in the way you need to know.
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hi, \n\nordinary table salt is an example of an ionic solid.  it is composed of a regular lattice of alternating sodium (Na+) and chlorine (Cl-) ions.  when in the solid form they do not actually exchange electrons, so they are still ions in the solid form.\n\ncheers !
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an ion with both acidic and basic part
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Ba(OH)2, MgBr2, CH3COOH, NH4OH\n\nFirst two are strong electrolytes, second two are weak (do not completely dissociate).
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Salt - sodium chloride.\n\nIf you need something a bit more unusual, I believe there is imitation salt which is potassium chloride.
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Sodium Chloride is an obvious example, as is Potassium Flouride, Lithium Bromide, or any other combination os the alkali metals and halogens from the periodic table.\n\nThe alkali metals are on the far left column of the table, and halogens are on the column 2nd from the right (next to last).\n\nAll of these combinations are collectively refered to as "salts".\nA salt is an ionic compound which contains a metal cation (+) and a nom-metal anion (-).  It is not a requirement that it be a specific type of metal or a specific type of non-metal though, for example, Iron Oxide is also technically a "salt", but it is more commonly refered to as an "Oxide", a more specific type of salt.\n\nhttp://www.webelements.com/index.html
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Sugar water is NOT an electrolyte.\n\nElectrolytes break into ions when dissolved in water, allowing an electric current to pass through the solution.\n\nSoluble salts are good electrolytes since they will easily break into ions in solution.  A very common salt table salt (NaCl) breaks into Sodium +1 and Chloride -1 ions.\n\nOther household items that will break into ions in solution are:\n--Vinegar (a weak electrolyte, breaks into H+ and Acetate -1 ions)\n--Drain Cleaner (commonly NaOH, breaks into Na+1 and OH-1), actually, most household cleaners are made of things that break into ions, but it is not a good idea to just start mixing things unless you know what they are (many people die by doing this and unknowingly make deadly gas).\n\nHousehold bleach is made of a solution of Sodium Hypochlorite (NaOCl) in addition to NaCl and NaOH, so that has all kinds of ions in solution.\n\n\nIf you have ever listened to a Gatorade commercial, you'd know that they are big on putting a buch of electrolytes into their sports drink.
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1. Covalent Bonds\n2. Ionic Bonds\n3. Hydrogen Bonds