Salt (NaC1) is a compound. Is this true?
210369
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.
545422
I'm assuming you're talking about ionic compounds like CaCl2 or KNO3....In order to name things from their formulas, you MUST know the common ions.  I'm sure you have a list of a table of ions you are expected to know.  Once you know all of those ions and their names, you can go from a formula to a name or the other direction quite easily.  But you've got to learn those ions first. \n\nIn naming from a formula, you name the cation (usually a metal) first, and then name the anion.  So, Na2SO4 is sodium sulfate.\n\nCa3(PO4)2 would be calcium phosphate.\n\nYou need to learn the parts before you can name the compounds.\n\nGood luck at this point...
381343
There are a few methods, most of them require memorization, or a good chart.  For example, ionic compounds get named by adding the names of their ions, but molecular compounds get named by each individual element and a prefix of how many there are.  Then you have acids...  \n\nhere are some examples:\n\nNaCl - Sodium Chloride\nNa2CO3 - Soduum Carbonate\nNa3PO4 - Sodium Phosphate\n\nNotice that sodium is always sodium, not mono, di or tri.\n\nMolecular compounds are different, here are some examples:\n\nNF3- nitrogen trifluoride   \nNO - nitrogen monoxide OR nitric oxide (Ionic)\nNO2 - nitrogen dioxide  \nN2O - dinitrogen monoxide (laughing gas)\n\nI wont even go into acids, or Hydrocarbons\n\nI hope that gets you started anyway
383878
It's a salt - ammonium acetate. Ammonium is an acid, but the acetate ion is actually alkaline.
351316
It is neutral too.  In the NaClO case the oxidation number of Cl is different from the oxidation number of Cl in NaCl\n\nNaClO\nNa is +1, O is -2, so Cl must be +1\n\nNaCl\nNa is +1 so Cl must be -1.\n\nGo, for example, to the following sites for some good rules to find out the oxidation numbers:\n\nhttp://chemistry.boisestate.edu/rbanks/inorganic/oxidation-reduction/redox4.htm
395738
Starting material:\nCH3CH2CHBrCH2Br ?\n\nProduct wanted:\nCH3CH2CH2CH=CHCH3 ?  Cis or Trans?\n\nIf the starting material is 1,2 Dibromobutane, then treating it with base (eg. NaNH2) will give:\n\n CH3CH2CHBr–CH2Br   +   base   ——>  CH3CH2CH=CHBr   +   base   ——>  CH3CH2C≡CH\n\nIf this is done with excess NaNH2 in liquid ammonia or dry diethyl ether, then the sodium salt will be produced:\n\n(CH3CH2C≡C)- Na+\n\n(CH3CH2C≡C)- Na+ + BrCH2CH3  ——>  CH3CH2C≡CCH2CH3 \n\nCH3CH2C≡CCH2CH3 when heated gives the more stable compound CH3CH2CH2C≡CCH3  (this is 2-hexyne).  The path will be different from here depending on if you want a cis or trans product.  A controlled catalytic addition (Lindlar catalyst) of H2 will give the Cis form.  Na in liquid ammonia will give the Trans.\n\nThere might be an easier way, but this path is a classic.
293219
What you have as your reactant is really just expressing a complicated equilibrium for the sodium salt of a carboxylic acid.  You have calcium ion in your products, but not your reactants, which is a no-no.  Having said that, it looks like you're replacing the sodium ion with calcium ion as the cation associated with carboxylate anion.  Separating all of the reactants from one another won't be easy, but you could try adding calcium hydroxide.  That should precipitate sodium and calcium carbonate.
550947
b,\n\nall the others are ionic compounds.
622656
Na2CO3 + 2HCl-> NaCl + H2O + CO2
350912
A) Sodium and Chlorine yields Sodium Chloride.\n\nB and C) --> http://en.wikipedia.org/wiki/Conservation_of_mass
282419
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 !
317296
I really advise that you dont try it.\n\nToo much table salt will create a sodium imbalance in your body. \nSodium ions in your body are responsible for transferring chemical signals between nerve cells, so as you can imagine it's kind of important.
594302
1-. NaCl + H2O Sodium Chloride ( table salt )\n2-. NaSO3 +2 H2O Sodium Sulfate ( or sulfite I always forget which is the 3 and which is the 4 )\n3-. NaC2H3O2 + H2O ( I'm guessing.  You will want to check your periodic table for the charges on this one )\n4-.NH4Cl + H2O.  Ammonium Chloride\n5-.NSO2 + 3H2O\n6-. not sure\n\nI presume you are working salt solutions.  Ammonia was never my strong suit. I'm positive about the first two.
435436
I presume that both the chemicals are in solid state and remain as a mixture. Perhaps you can try to sieve the mixture and separate the two items since sodium hydroxide is a flaky material whereas, if I remember right, barium chloride is either amorphous or granular.
202856
The compound themselves are neutral but when each compound is dissolve in a solvent (like water), Calcium has a +2 charge, carbonate has a -2 charge, Acetic acid would become acetate (-1 charge) and hydrogen ion (+1 charge).  Hope that helps.
98294
Tommy was right as far as Mg & Ca are concerned.  Na is a Group 1 metal and is more reactive than either because it's 3s1 structure is an incomplete atomic orbital, whereas Mg (3s2) and Ca (4s2) have a certain stability from being a complete electron pair.
465060
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.