What is Sodium Chloride (Liquid Form) used for?
824009
It sounds a lot like a nasal spray I used to use. It is simply salt water. Isotonic means that it is roughly the same salt concentration as the tissue that you spray it with, so that it doesn't make it drier. "For irrigation" means that it is for rinsing. Because it has no antimicrobials, it is not for contact lens or eye cleaning, so it could be for a nasal spray, for cleaning wounds, or perhaps something else.
727659
1.when sodium and chlorine combine they lose their harmful properties and become altogether new substance\n\n2.carbon di oxide\n\n3.bauxite(alumina)
513498
salt.\n\n(Sodium Chloride)
340627
The atomic bonds in sugar are very tight and do not allow for (measurable) ionization, which is what helps water conduct electricity.  Salt (NaCl) is a powerful ionization agent - the Cl atom "steals" Na's outer electron, forming a Na+ ion, which attracts new electrons introduced into the water.  We call that a conductor!
192043
It sort of depends on what you mean by contains water, sodium chloride in water is a solution containing water where water is the solvent.  Hydrochloric acid is another, (that is just HCl dissolved in water).  Hope this helps
213697
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':
327351
The previous answer is correct if an equal number of moles is dissolved.  If you were looking at a saturated solution, it would be LiCl, which can dissolve in greater quantities than any other salt, even greater than NaCl. (36 g of NaCL will dissolve in 100 ml water compared to 55 grams LiCl per 100 ml water). The Li+ ion is very very small-it's only larger than hydrogen and helium. For an equal weight of LiCl and Al(NO3)3 dissolved in water, LiCl would also have a greater effect, because of the greater number of ions per gram.  Thus, in either a saturated solution or a weight to volume solution, LiCl would produce the greater number of ions, whereas it would not in a equamolar solution.  LiCl is used a great deal in density experiments, because you can make a very dense aqueous solution of it, and in reducing freezing point, since you can get the maximum number of ions of any aqueous solution, so the questioner is probably looking for LiCl.
1072536
The liquid you want is a solution of boracic (or boric) acid.
253912
http://en.wikipedia.org/wiki/Liquid_soap
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.
809
Sodium chloride or common salt is the chemical compound NaCl, composed of the elements sodium and chloride. Answer 2 grams of salt/sodium = 2 grams!
676532
This is known as a colligative property of most solvents, namely freezing point depression and boiling point elevation.  For freezing water, the molecules need to align themselves in a very organized lattice.  When other substances (salt for example) are present, they interfere with the ability of water molecules to align themselves properly.  This is how salt is used to keep water from freezing in the winter.  It doesn't melt it, it lowers its freezing point.
710667
A) Sodium and Chlorine yields Sodium Chloride.\n\nB and C) --> http://en.wikipedia.org/wiki/Conservation_of_mass
958951
Sodium Chloride = Table Salt\nPotasium Chloride = buffering salt used by all animals and plants\nSodium hypochlorate = Bleach\nSodium BiCarbonate =  Baking soda\nSodium Hydroxide = lye   (strongly caustic .. basic solution used in manufacturing and synthesis of many compounds\non, and on, and on
588420
sodium chloride and water
731293
sodium & chlorine to make NaCl, table salt
603247
An electrolyte is a liquid substance which acts as a medium to conduct electricity. One speaks of an electrolyte in a number of different contexts, the most common including health and fitness, and various electronics and automotive disciplines. An electrolyte is full of ions, which are atoms that have some sort of net electric charge, either positive or negative. A dilute electrolyte has a relatively small amount of ions for its volume, while a concentrated electrolyte has a high amount of ions.\n\nIn basic fuel cells, such as those used in automotive technology, an electrolyte acts as the liquid that allows ions to travel between the cathode and anode to keep the power-generating process underway, while keeping the reactive oxygen and hydrogen apart. In the type of fuel cell known as a proton exchange membrane cell, the electrolyte specifically moves protons (positively-charged hydrogen ions) to the cathode from the anode where they are produced, with the end result being the production of water and electricity.\n\nBatteries also employ an electrolyte of some sort, both to conduct electricity between the battery plates, and to store energy on the plates themselves. The electrolyte used in a battery depends on the battery's type and purpose. Most car batteries, for example, use an electrolyte which contains sulfuric acid, which is why they require careful handling. Alkaline batteries use an alkaline solution for their electrolyte. Lithium batteries use a special organic electrolyte which freezes at much lower temperatures than more traditional water-based electrolytes.\n\nIn human health, electrolytes aid in a number of vital bodily processes. Many heart and nerve functions, muscle control and coordination, and the body's ability to absorb fluids all depend on a healthy balance of electrolytes. The most common electrolytes found in the human body are sodium, potassium, magnesium, chloride and calcium. Various hormones in the body help regulate intake of these electrolytes, and the kidneys filter electrolytes which reach excessive levels. Unhealthy levels of consumption of any or all of the body's necessary electrolytes can cause serious health issues. The most common imbalances are hyper- and hypo-natremia, or excessive and insufficient levels of sodium, and hyper- and hypo-kalemia, or excessive and insufficient levels of potassium.\n\nMany sports drinks contain added potassium and sodium to help restore the body's proper electrolyte balance after intense physical exertion. After exercising heavily, it can be dangerous to ingest large quantities of water, as it may dilute existing electrolyte levels and cause physical problems. Additionally, a number of electrolyte enhanced drinks exist specifically for children and may be helpful for regular use, particularly to restore electrolyte balance after sickness which has included vomiting or dihorrea