what is the difference between an electrolyte and a nonelectrolyte?
141938
Electrolytes- compounds which when dissolved in water produce solutions that conduct an electric current. \n\nNonelectrolytes- compounds which when dissolved in water produce solutions that do not conduct an electric current.
1169890
Pure water is a poor conductor but when you have water on a surface, you basically have an electrolyte solution that allows electricity to flow much easier.
1024740
The question makes no sense.  A single, isolated anion has no pH value.  pH refers to the H+ concentration in aqueous solutions.
525723
when an atom loses an electon from its outermost shell then it forms an electropositive ion while when an atom gains an electron it forms an electronegative elctron.\n\nfor e.g. during the formation of nacl na atom loses an elcron to the cl atom to form a +ve ionwhile the cl atom which gains that electon forms a -ve ion.
726534
When salt  ( NaCl ) dissolves in water, it becomes Na+ and Cl-, or, atoms called "ions".  It's these ions that carry the electrical charge.  The higher the concentration of these ions, the more conductive the solution will be.
386269
-molecular:it is a double replacement reaction.  i.e.:ab+cd=ad+bc.  \n-net ionic: you find the one that becomes the solid, and you remove all the other spectator ions.\n\nno way, i have to do the same exact thing for homework tonight.  writing net ionic, gross ionic, and molecular formulas. damn.  are you doing molarity too?  are you a sophomore?  damn science.  i hate science.
824595
You can't remove the sodium ions without replacing them with something else positively charged. You cannot have a solution with a net charge.\n\nIn the second case, replacing the sodium ions with protons would increase the conductivity of the solution a little bit because protons have a greater mobility than do sodium ions.
551430
You cannot have one without the other.  If there are cations present, there will be an equally charged pile of anions there with it.  The charge on any system is always neutral (or very close - it may have some electrical potential but relatively speaking, it's very low).
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
926599
There is a mnemonic to easily remember the basic tenet of solubility: "Like dissolves like.." Salt, NaCl, is an ionic compound. Water is a polar compound. That is why water dissolves salt, becuase they could both be considered polar, they have a positive and negative end. Butanol is non-polar. That is why it dissolves napthalene, which is also non-polar, better than water.
548540
Ionic bonds are comprised of a metal and a non-metal.\nCovalent bonds are comprised of two bonded non-metals.
519991
1, 1, 2, HNO3, 1, PbSO4.\n\nTechnically, the HNO3 is aqueous and stays in ion form, but it doesn't seem like you're looking for a net ionic.
929685
When you have weak electrolytes, (equillibria in general) you should make the following table.\n\n1. write the reaction\n\nHNO2 <=> H+ + NO2-\n\n2.Put the initial amounts (expressed as concentration) of each molecule. In this case we have only the concentration of HNO2, so\n\n.. .. .. .. .. .. HNO2 <=> H+ + NO2-\nInitial .. .. .. .. 0.5\n\n3.Assume that an unknown amount "x" of the reactants react.\nThen write also how much of each product you expect to be produced according to the stoichiometry. In this case 1 mole of HNO2 gives one mole of H+  and NO2-, so x mole/L HNO2 will  give x mole/L of each and our table becomes\n\n.. .. .. .. .. .. HNO2 <=> H+ + NO2-\nInitial .. .. .. .. 0.5\nDissociate .. ..x\nProduce .. .. .. .. .. .. .. ..x .. .. .x\n\n4. Ka is an expression for the concentrations at equilibrium. So let's see what are those. For the reactants you will have initial-what reacted. We have only HNO2 with 0.5-x. For the products it will be the initial+what was produced. We didn't have any intial so it is only what was produced (x for both of the products). Thus the table in its final form is \n\n.. .. .. .. .. .. HNO2 <=> H+ + NO2-\nInitial .. .. .. .. 0.5\nDissociate .. ..x\nProduce .. .. .. .. .. .. .. ..x .. .. .x\nAt Equil. .. .. 0.5-x .. .. .. x .. .. .x\n\nKa= [H+][NO2-]/[HNO2] = x^2/(0.5-x)\nNow you either solve the quadratic equation and find x, or we assume that 0.5 >>x and practically 0.5-x=0.5.\nThen Ka=x^2/0.5=4*10^-14 =>\nx=squareroot(2*10^-14)= 1.4*10^-7. It is much smaller than 0.5 so our assumption is valid (otherwise we would have to solve the quadratic and get an exact solution).\n\nFor a simple level of chemistry we would now say\npH=-log[H+]= -logx =-log(1.4*10^-7) = 6.85\n\nHowever for more advanced and accurate expectations we see that the H+ coming from HNO2 is found to be in the same order of magnitude as that coming from the self dissociation of water (10^-7 for distilled water). Therefore in this case we cannot ignore the self dissociation of water (as we usually do) for calculating the pH. \nThere are 2 approaches for this case, here is one of them.\nRemember that we didn't put an initial amount for H+ since in most cases we ignore the self dissociation of water. Now we will consider that we had pure water, so the initial concentration of H+ is 10^-7 and we want to see how much the HNO2 will dissociate under these conditions so our table becomes\n\n.. .. .. .. .. .. HNO2 <=> H+ + NO2-\nInitial .. .. .. .. 0.5 .. .. .. 10^-7\nDissociate .. ..x\nProduce .. .. .. .. .. .. .. ..x .. .. .x\nAt Equil. .. .. 0.5-x .. 10^-7+x. .x\n\nand Ka=(10^-7+x)x/(0.5-x)\nNow we have to solve the quadratic so we can't do any simplification\n\n0.5Ka-Kax=10^-7x +x^2 =>\nx^2+ (10^-7+Ka)x-0.5Ka=0\n\nThe only acceptable solution is the positive one\nx=0.5(- (10^-7+Ka)+ squareroot (D))\nwhere D=(10^-7+Ka)^2-4*(-0.5Ka)=\n=(10^-7+4*10^-14)^2-4*(-0.5*4*10^-14)\n=9*10^-14\n\nand x=0.5*(-((10^-7))+4*10^-14) +3*10^-7) =10^-7\n\nso now pH=-log(10^-7+x) =-log(2*10^-7) = 6.70
415923
Yes, salt water is a sodium chloride solution with Na+ and Cl- ions. when two seperate condutors are immersed in the solution without contacting each other and a bulb or any electrical appliance is placed across the conductors the positive and negative ions migrate and conducts electricity.
871982
it would have to be "e". a strong-electrolyte is the only one that dissolves itself 100% purely in the a solution. the weak electrolyte does not do that since it cannot do that but rather ionizes itself partially in a  weak electrolyte.\n\nhope this site helps:\nhttp://en.wikipedia.org/wiki/Strong_electrolyte
336452
NaCl IS NOT TWO ATOMS (sodium and chlorine) BONDED TOGETHER!\n\nNaCl is what is known in chemistry as an ionic salt.  That means that a very positively charged Na+ ion met up with a very negatively charged Cl- ion, and because opposite charges attract, they got close to each other in what is known as an ionic bond, which isn't really a bond, just two particles hanging out together.
486231
NaOH is ionic.\n\nAll has to do with electronegativity and the difference between the two species bonded to each other.  If the electronegativity difference is less than 0.5, the bond is considered to be fairly non-polar.  Between 0.5 and 1.5 is usually a polar bond, greater than 1.5 usually means that there will be charge separation and the bond will be ionic.\n\nFor either polar or non-polar bonds, you need to know the geometry of the molecule and determine whether the sum of the individual dipoles in the molecule will cancel (vector sum).  If they do, the molecule is non-polar.  If they don't, it is.  For instance, water is polar as its polar bonds do not cancel geometrically, but CH4 is non-polar, even though each of its bonds is polar.