Which of the following aqueous solutions contains the greatest number of ions?
461143
Well, look at each species. NaCl dissociates into two ions, giving a strength of 0.20M. In 400 mL, that'd be 0.08 moles.\n\nFeCl3 dissociates into four ions, giving a strength of 0.40M. In 200 mL, that'd also be 0.08 moles.\n\nCaCl2 dissociates into three ions, giving a strength of 0.30M. In 300 mL, that'd be 0.09 moles.\n\nKBr dissociates into two ions, giving a strength of 0.20M. In 200 mL, that'd be 0.04 moles.\n\nSo, the calcium chloride (CaCl2) solution contains the greatest number of ions.\n\n\nHope this helped.
595177
Actually, this is pretty simple.  You have a saturated  solution of lead sulfate (PbSO4) and strontium sulfate (SrSO4).  Probably the biggest hurdle here is to realize that the concentration of sulfate ion will be the same for both salts!  Therefore, the concentration of sulfate ion will be the result of the most soluble of the two salts:\n\nKsp for PbSO4 = [Pb+2]*[SO4-2] = 1.6x10^-8\nKsp for SrSO4 = [Sr+2]*[SO4-2] = 2.8x10^-7\n\nStrontium sulfate is the more soluble of the two salts, so it will control the concentration of sulfate:\n\nSrSO4 ===> Sr+2  + SO4-2, thus [Sr+2] = [SO4-2]\n\nKsp for SrSO4 = 2.8x10^-7 = [SO4-2]^2 , so \n\n[SO4-2] = sqrt(2.8x10^-7) = 5.29x10^-4 = [Sr+2]\n\nNow, to find out the concentration of Pb+2, we use the value we have just calculated for [SO4-2] and the Ksp:\n\nKsp for PbSO4 = [Pb+2] * [SO4-2] = 1.6x10^-8\n\n[Pb+2] = 1.6x10^-8/[SO4-2] = (1.6x10^-8)/(5.29x10^-4)\n[Pb+2] = 3.02x10^-5\n\nand there we have your answers:\n[Sr+2] = [SO4-2] = 5.29x10^-4 moles/liter\n[Pb+2] = 3.02x10^-5 moles/liter
261798
The aqueous solubility of AgNO3 at 20C is 67.8 (solubility is 100*m2/(m1+m2) where m2 = mass of solute and m1 = mass of solvent).\n\nRearraging the equation gives us m2 = (m1*67.8/100)/(1-67.8/100).  or\nm2 = (m1*.678)/(1-.678) = 210.56g of AgNO3 @ 20C\n\nAt 50C the aqueous solubility of AgNO3 is 79.2 so\nm2 = (m1*.792)/(1-.792) = 380.77g of AgNO3 @ 50C\n\nTo find the amount needed to make the second solution saturated we must subtract answer 1 from answer 2.\n\nWe find that 170.21g of AgNO3 must be added to make the solution saturated at 50C.
1157889
Sodium (Which retains water in the body and is an electrolyte), sugar, probably some potassium, and lots of water. \n\nElectrolytes are ions, such as sodium, potassium, or chloride, required by cells to regulate the electric charge and flow of water molecules across the cell membrane. -Which means they make it easier for your cells to work, process things, and remove waste with water.
752832
think high concentrations of ions can denaturate proteins, an d some ions in particular...
1025655
Think of the net ionic equation which is occuring.\nSince both the HCl and Ca(OH)3 are dissolved in aqueous solution, broken into ions, just focus on the H+ and OH- part of it first.\n\nH+(aq) + OH-(aq) --> H2O(l)\nThe Hydronium ion and the Hydroxide ion react to form water.\nWhat is left over are the Ca+2 and Cl- ion which drop out of the net ionic eqaution since they form the very soluble compound, Calcium Chloride (CaCl2).\n\n2 HCl (aq) + Ca(OH)2 (aq) --> 2 H2O (l) + CaCl2 (aq)
109387
Maybe you are referring to aqueous solutions of these species? If so, then a solution of glucose will be pH 7 since it does not have any proton or hydroxide to change the neutral pH of water. As for solutions of the rubidium, potassium and cesium IONS, they can accept hydroxide from water if they are stable enough to form the metal hydroxide or if they convert to metal oxides. That means hydrogen ions are also formed and this makes the solution acidic, and hence the pH drops. But large cations like Rb and Cs do not readily take in hydroxide owing to the low polarizability of the cations (see me winking here ;p  ), unlike the small K ion. So, with these clues, can you now find out by yourself the answer to your question? Don't we just love chemistry!
924596
The KCl, definitely.  Conductivity in water is greatly enhanced by the presence of ions.  Deionized water actually has fewer ions in it than ordivnary tap water, so it's a really terrible conductor.  KCl, on the other hand, dissolves into K+ and Cl- in water, so there are a whole lot of ions in a solution of KCl.
75046
Well, besides water, there's dissolved salts, made up of chloride and sulfate salts of calcium, sodium, potassium, and magnesium.  There are also many trace elements, including gold.
1143443
Able to be dissolved by water.
1168891
The balanced solution is nothing else than a special physiological salt solution.  Near the sodium chloride it generally contains CaCl2, KCl, potassium and sodium-phosphate, Mg-salt(chloride or sulphate), sodium hidrocarbonate.\nAs additional component it may contains some glucose and/or phenol red as a pH indicator.
43551
Most professional papers that I read refer to it as just water ion (in its charged form).  This a water molecule with an over-all positive charge.  I do not believe that its structure is known, but I could be wrong about this.\nSee example reference below:
726015
Water - L\nUrea - G\nUric acid - G\nPus - L\nGlucose - L\nAlbumin - L\nCreatine - L\nHydrogen ions - G\nPotassium ions - L\nRBCs - L\nSodium - L\nAmino acids - L
47023
Sodium Hydroxide (aqueous). It's a solution in water of the compound NaOH.
176528
http://www.chem1.com/CQ/ionbunk.html\n\nskim this article.
91741
What are the states of each of the substances?\n\n\nammonium chloride(aq)+potassium hydroxide(aq)---->ammonium hydroxide(aq)+potassium chloride(aq)\n\n   Complete ionic equation\nNH4+(aq)+Cl-(aq)+K+(aq)+OH-(aq)------->\nNH4+(aq)+OH-(aq)+K+(aq)+Cl-(aq)\n\n     Net Ionic Equation\nSame as complete ionic equation, every ion is a spectator ion, OR it doesn't exist.\n\nI don't think both substances are in aqueous solution.
59648
You'll probably want to know typical values for drinking water and sea water.\n\nNormally, water contains dissolved salts with Na, K, Ca, Mg and depending on quality Fe and Mn as main kations and carbonate (and hydrogen carbonate), chloride, sulfate and to (hopefully) lesser extent nitrate and phosphate ions. There are numerous possibilities to combine these ions into solid salts, making the exercise fairly pointless.\n\nIf your teacher insists, Na and K for all the anions except HCO3(1-) and CO3(2-) which usually are written as Mg and Ca salts.\n\nCommon trace elements/compunds include Al, Si, NO2(1-), Li.\n\nMore or less routinely monitored heavy metal traces include As, Cd, Cr, Co, Cu, Ni, Hg, Pb, Sb, Tl, Zn