what does it mean if i say "Sulfuric Acid, 1.00 N Solution" or  "Sulfuric Acid, 0.255 N Solution"
970448
N = Normality...in this case the concentration of Sulfuric Acid in a solution.\n\nThe concentration of Sulfuric Acid in the 1.00 N Solution is almost 4 times as concentrated as the 0.255 N Solution.\n\nIn practice Normality is "similar" to Molarity, except Normality takes into account the actual number of protons exchanged in a reaction.  Normality = Molarity times the number of protons exchanged.  In Sulfuric Acid, two protons are available for exchange...therefore, a one molar solution would be a two normal solution.  It is useful when doing titrations to determine concentrations.
320845
Having equal amounts of positive and negative charges.\n\nOr\n\nA mixture of equal acid and base with pH=7.00000
1074861
less than 7 is Acidic...lower the value more acidic it is.\nAbove 7 it is basic.
216402
It's:\n\nBaSO4(s)---water <--> Ba2+(aq)  +  SO4 2-(aq)\n\nthe solubility for this compound is very low  per  g/L\n\n\n about 0.0023g/L
866680
OK - chemists are basically lazy (that's why we use symbols for elements and formulas for compounds; we don't really like to write that much.)\n\nThe mole is a shortened way to indicate a really big number.\n\nIf I said to you, 1 dozen, you would know I am talking about 12 of something (doesn't matter what, its still 12).\n\nIf I said to you, 1 pair, you would know I am talking about 2 of someting (doesn't matter what, its still 2)\n\nIf I said to you, 1 mole, you would know I am talking about\n602200000000000000000000 of something (doesn't matter what, its still that much.) This is usually written as 6.022 x 10(23)\nbecause we are not about to keep track of all those zeroes.  If I told you your allowance was 1 mole of dollars you would be very rich because you would have 6.022 x 10(23) dollars. (Remember me in your will).\n\nAtoms are too small to see so we have to work with A LOT of them and everyone has agreed on a "standard" number of atoms, 1 moles worth, also called "Avogadro's number".  You could have less than that (0.5 moles, 0.456 moles) or more (10 moles, 540 moles etc.) but the "standard" for comparison is 1 mole.\n\nSo, for your project, figure out how many "whatevers" it takes to go around the world and then divide that number by 6.022 x 10(23) and you will know how many moles of your "whatever" you need.
706856
Acidic.\nBecause sodium nitrate is a salt solution, and is neutral. Since you are adding an acid to a neutral soution, the end reault will be an acidic mixture.
683322
Well, I suppose 1.25 g is 1250 mg, so seeing there's 1250 mg in each ml of solution, taking out 0.2 ml of the solution will net you 250 mg of the substance.
307574
No, it's Ag2S. The 2 is a subscript, denoting 2 Silver atoms to 1 Sulphur atom. Silver has a valency of 1+, while Sulpur has a valency of 2-, hence 2 Silver atoms are needed to balance with 1 Sulphur atom to form a compound. Besides, the equation would make sense then. 2 Silver atoms and 1 Sulphur atom on both sides of the equation, the equation is now balanced. 10 marks please, thank you!
730290
You have remember that sulfuric acid is a strong acid and that it is diprotic.  Meaning that it has two hydrogen ions per formula unit of sulfuric acid.  \nNOTE:  There will be a negligible amount of HSO4- ions in solution, and since this is a strong acid, strong base equation, they can be omitted.\n\nH2SO4 + 2NaOH --> Na2SO4 + 2H2O\nOR (in net ionic)\nH+ +OH- --> H2O\n\nFirst start off with what you know, and molar masses you can calculate\n200g NaOH x (1 mol NaOH)/(40 g NaOH) x (1 mol H2SO4)/(2 mol NaOH)\n=\n5/2 moles = 2.5 moles\n\nset up equation to find how many liters of 2.5 M = 2.5 mol H2SO4\n? L x (2.5 mol/L)=2.5 mol\n?=1.0 liter of H2SO4\n\nthere is really no need to convert to units of meters when talking about molarity and volume.  Technically, a cubic decameter is the same as a liter; however, it is customary to keep volume in terms of liters.
928965
molarity  = moles / liters\n\nmoles = given mass / molecular mass\n\n10 g H2SO4 / 98 g per mole = about  0.1 moles\n\n0.1 moles / 1 L = 0.1 M solution
204256
The number always comes after the element, so two hydrogen and one oxygen.\n\neg if you have a more complex compound like Sulphuric Acid,\nH2SO4 that would be 2 hydrogen, one sulphur (or Sulfur in the USA) and 4 Oxygen
810972
Cool stuff, I used to get confused by ugly chemistry calculations, too :D\n\nYou have 3.88 g acid in 250cm3, so in the 25 cm3 you titrated there are 0.388 g of the acid. You need to know how many moles that is, so that you can calculate molar mass.\n\nThe amount of NaOH used up is 46.5 cm3 × 0.095 mol/dm3, that is 0.0465 dm3 × 0.095 M, which equals 0.00442 mol (It's not exactly that much, but I'll stick with three significant figures).\n\nSince NaOH reacts with monoprotic acids in a 1:1 ratio, that means that there was exactly the same amount of acid in the solution.\n\nNow we know that 0.388 g of the acid is 0.00442 mol, so we can divide the mass by the number of moles to get molar mass. That is 0.388g/0.00442 mol = 87.8 g/mol.\n\nRelative molecular mass is simply molar mass in grams, but without the unit, so Mr of the acid is 87.8.
872765
It won't matter how much you started with or how much higher the solution was heated.  When the solution cools to 20C it will hold 0.22g/100mL of solvent (water).\n\nSo if you start with 1.75g and 0.22g remain in solution, the amount crystallized at 20C will be the difference, 1.53g.
809077
I would assume that one of your .01s in column A is something like 0.012.\n\nChange your number  format to General and see what happens.
75905
From what I can find out, it appears to be slightly acid, approaching neutral, pH 5-7\n\nHow cool is that?! It's like that question was designed just for someone with my name!
715311
HNO3 (nitric acid) is a strong acid, which means that when HNO3 is dissolved in water, essentially all the HNO3 molecules dissociate into hydrogen ions and nitrate ions:\n\nHNO3(aq) -> (H+) + (NO3-)\n\nEach mole of HNO3 that reacts produces 1 mole of H+ ions.\n\npH is defined (approximately) as:\n\npH = - log[H+]\n\nwhere [H+] means the molar concentration of hydrogen ions, and "log" means the base-10 logarithm.\n\nFor this problem, then,\n\npH = - log(2.5*10^-5) = 4.60\n\n[Strictly speaking, the pH is defined as the negative logarithm of the thermodynamic activity of the hydrogen ion, not the concentration.  For dilute solutions, though, the activity (which is a unitless quantity) is approximately equal to the numerical value of the molar concentration.  This is not something that is generally dealt with in introductory chemistry classes, though.]
169137
We have 48 gallons of a solution 64% acid\nSo the acid quantity = 48*0.64\n\nWe will add X gallons of a solution 16% acid\nSo the acid quantity = X*0.16\n\nThe Total acid quantity= 48*0.64 + X*.016\nThe Total Volume = 48 gallons + X gallons\n \nThe Average Percantage of acid= Total acid quantity/total volume\n=[48*0.64 + X*0.16]/[48+X] ===== 0.52 as given\n\n48*0.64 + X*0.16 = 0.52*(48+X)\n48*(0.64 - 0.52) = (0.52 - 0.16)*X\n48*0.12 = 0.36*X\nX=48 * 0.12/0.36= 48/3 = 16 gallons\n\nWe must add 16 gallons of solution 16% acid