Salt (NaC1) is a compound. Is this true?
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If you mean NaCl (letter L at the end instead of number one), then, yes, sodium chloride is an ionic compound. In solid form it is NaCl(s), commonly known as table salt.\n\nIn case you're wondering, the formula NaCl is actually considered a "formula unit" rather than a "molecule." In solid form, ionic compounds are 3-D matrices of ions. But when dissolved or solvated in water, the ions become free floating Na+ and Cl- ions rather than individual NaCl units. A formula unit simply shows the lowest whole-number ratio of cations (positively charged ions) to anions (negatively charged ions) given by the formula. Sodium chloride's cation to anion ratio is one sodium cation Na+ per chloride anion Cl-, or 1 to 1.\n\nBy way of contrast, the formula H2O (for water) represents a molecule, because each molecule of water is a distinct unit.
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Ionic compounds (like NaCl) for lattice structures.  These lattice structures make up the crystaline arrangement of the compound.\n\nThe lattice of NaCl looks like a cube,\nhttp://zimmer.csufresno.edu/~davidz/Chem3AF97/ChB/IonicBond.html\nhttp://departments.kings.edu/chemlab/chemlab_v2/nacl.html
484197
Salt - sodium chloride.\n\nIf you need something a bit more unusual, I believe there is imitation salt which is potassium chloride.
617322
Althouigh I am sure you mean Sodium Chloride when you say "Salt", just to be perfectly clear....there are multiple types of "salt".\nA salt is an ionic compound made up of a matal cation and a non-metal anion. Sodium Chloride ("table salt") is an example of a salt, so is Potassium Chloride and Ammonium Nitrate.\n\nWhen you dissolve a salt in water, the freezing point of the solution is lowered.  Likewise, when dissolving a salt, the boiling point of the solution is raised.\n\nBut you asked about a temperature change.\nWhen dissolving some salts, the dissolving process is endothermic...meaning that it requires enegry input to proceed.  When a endothermic process occurs, the temperature of the surroundings (this case, the water) drops.\nThere are also salts which give off energy when they are dissolved in water.  Processes which give off excess energy are called exothermic and can raise the temperature of the surroundings.\nThere are also a few (not too many) "ideal" salts which neither take in or give off energy when they dissolve.\n\nWhen the salt dissolves, if the "product" (the aqueous salt) has a lower enthalpy than the undissolved salt, the solution is said to be exothermic.  If the enthalpy increases, the solution is said to be endothermic.\n\nSalts like Potassium Chloride, Ammonium Nitrate, and several others (probably NaCl too, which you refered to) are endothermic when dissolved in water, and thus, when dissolved cause the temperature of the solution to decrease slighty.\n\nSalts like Sodium or Potassium Hydroxide are great examples of salts which are exothermic (give off energy) when they are dissolved in water.  When dissolving these salts in water, a notible increase in temperature can be observed.
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The following links have a lot of information on it and then you can find some of the Sodium CMC online in different spots as shown in the same links!\n\nhttp://aic.stanford.edu/sg/bpg/annual/v01/bp01-04.html\nhttp://www.tradekey.com/ks-Sodium-Carboxymethylcellulose-CMC/\nhttp://www.par-chem.com/Product.aspx?ProductId=1882&Name=Sodium%20Carboxymethylcellulose,%20FCC\nhttp://www.kicgroup.com/cart/customer/search.php?substring=Sodium+CMC
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.001565mol / .075L = .021M NaCl
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Sodium chloride is table salt.  It readily dissolves in water.\n\nIron (II) Carbonate, on the other-hand is not very soluble and will precipitate from the solution.\n\nSodium is an alkali metal (in the first column of the Periodic chart).  Most simple alkali metal salts are soluble.\n\nCheck the site below for solubility rules of compounds.  If you do not memorize this, at least print out a copy and keep it in your text or notebook.
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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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A salt is the the end products of a reaction, "SALT" can be any various combinations of elements. Which one are you looking for?
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Table salt is sodium chloride, NaCl.  If it's "iodized," it will contain sodium or potassium iodide (NaI/KI).  It also contains (usually) an anti-caking agent, like sodium silico-aluminate, NaAlSi3O8.  Salt substitute is potassium chloride, KCl.  It also contains some other chemicals, which seem to vary by brand.
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There are all sorts of salts:\nacid + base = salt + water\nHCl + NaOH = NaCl + H2O\n\nNaCl is sodium chloride. This is the same stuff we use at the table. If you have a look at the packet it came in you will probably find there are a few other things in the 'table salt' too - perhaps some iodides and an anti-caking agent to keep it running freely.\n\nMore info. on 'table salts':
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NaCN-Sodium Cyanide-alkaline\nNH4NO3-Ammonium nitrate-acidic\nNH4Cl-Ammonium chloride-basic
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_NaOH(aq) + _Fe(ClO4)3(aq) => _Fe(OH)3(s) + _NaClO4(aq)\n\n3  NaOH(aq) + 1  Fe(ClO4)3(aq) => 1  Fe(OH)3(s) + 3  NaClO4(aq)\nThe coefficients of one could be excluded but I put one which is also equivalent.\n\n_((NH4)2)SO4(aq) + _Pb(NO3)2(aq) => _PbSO4(s) + _NH4NO3(aq)\n\n1  ((NH4)2)SO4(aq) + 1  Pb(NO3)2(aq) => 1  PbSO4(s) + 2  NH4NO3(aq)\n\nThese are only the balanced equations.\n\nThe following is the ionic equations:\n(Na)+ (aq) + (OH)- (aq) + (Fe)3+ (aq) + (ClO4)- (aq) => Fe(OH)3(s) + (Na)+ (aq) + (ClO4)- (aq)\nand\n(NH4)+ (aq) + (SO4)2- (aq) + (Pb)2+ (aq) + (NO3)- (aq) => PbSO4(s) + (NH4)+ (aq) + (NO3)- (aq)\n\nThe ionic equations are already balanced.  It is simply the breaking down of the equations into ions.  The solid remains intact while the compounds in aqueous solution become ions.\n\nThe + and - signs are the charge of the ions.  I can't find any other way to write them so I separated the compound with parentheses.  Sorry if it's confusing.\n\nThe net ionic equations are "simplified" ionic equations.  Basically, the things that are repeated on both sides get crossed off.  What is remaining is simply the net ionic equation.\n\n(OH)- (aq) + (Fe)3+ (aq) => Fe(OH)3(s)\nand\n(SO4)2- (aq) + (Pb)2+ (aq) => PbSO4(s)
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salt.\n\n(Sodium Chloride)
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No.  Any salt has a pH of 7.  Any acid has a pH of less than seven.  They're contradictory.  If you mixed some acid and some salt, I wouldn't call it salt any more.  I'd call it acid.
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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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Always remember that salts are formed by ions:\n\nCommon salt-forming cations include:\n\nammonium NH4+ \ncalcium Ca2+ \niron Fe2+ and Fe 3+ \nmagnesium Mg2+ \npotassium K+ \npyridinium C5H5NH+ \nquaternary ammonium NR4+ \nsodium Na+\n\nCommon salt-forming anions (and the name of the parent acids in parentheses) include:\n\nacetate CH3COO− (acetic acid) \ncarbonate CO32− (carbonic acid) \nchloride Cl− (hydrochloric acid) \ncitrate HOC(COO−)(CH2COO−)2 (citric acid) \ncyanide C≡N− (hydrogen cyanide) \nhydroxide OH− (water) \nnitrate NO3− (nitric acid) \nnitrite NO2− (nitrous acid) \noxide O2− (water) \nphosphate PO43− (phosphoric acid) \nsulfate SO42− (sulfuric acid)