can you explain to me about kation and anion analysis?
153108
A cation (not kation) is an ion with a positive charge and an anion is an ion with a negative charge. What exactly do you mean analysis? Hope it is somewhat helpful.
842680
2 KBrO3 + 3 N2H4 -> 2 KBr + 3 N2 + 6 H2O\n\nYou can check by finding out the total number of atoms of both sides:\n 2 Potassium\n 2 Bromine\n 6 Oxygen\n 6 Nitrogen\n12 Hydrogen
995333
just use it frequently, and you will get familiar with those name\nBut a i have a little trick\nin the most of negative ion with -ate ending, the non-oxygen atom usually has the oxidation number with the same number with its group number\ncarbonate (CO3)2-, C's ox number=+4,\nsulphate (SO4)2-, S's ox number =+6\ntry nitrate,phosphate,etc.\nbut oxohalogen anion is exception\nperhalat (XO4)-(e.g perchlorate=(ClO4)-), halat (XO3)- (e.g chlorate (ClO3)-, halit (XO2)-, hipohalit (XO)-\nThe non-oxygen atom in negative ion with -ite ending are usually has ox number of 2 number lower than that of -ate ions
804535
Neutralization Reaction:\nHC2H3O2(aq) + KOH(aq) -->H2O(l) + KC2H3O2(aq)\nThe equation is already balanced.\n\na. False KC2H3O2(aq) and H2O are products.\nb. True\nc. False, some ions will cancel out but some will remain.\n\nThe ionic equation is as follows:\n(H^+)(aq) + (C2H3O2^-)(aq) + (K^+)(aq) + (OH^-)(aq) -->H2O(l) + (K^+)(aq) + (C2H3O2^-)(aq)\nRepeated ions are crossed off from both sides and the net ionic equation is:\n(H^+)(aq) + (OH^-)(aq) -->H2O(l)\n\nd. True\ne. False\n\nNote: the + and - signs were written with ^ to indicate that they were raised up (like a power).  Sorry if this notation is confusing.  Good luck and I hope that this helps!
862596
K2SO4\nCa(NO3)2\n\npotassium has a +1 charge and sulfate has a -2 so therefore you need 2 potassiums so that you can have a net zero charge.\ncalcium has a +2 charge and nitrate has a -1 charge so you need two nitrates to balance the charges
991396
A potassium ion has one positive charge because it is missing one valence electron.   So K can form compounds with anything that is electronegative; in other words, any atom or molecule that likes to grab electrons. Anything at the right hand end of the periodic table, like O, S or the halogens for instance.   Or a more complicated compound would be with an organic acid like stearic acid; you replace one H with a K and you get a liquid soap.   If you used Na instead of K you'd get the usual solid soap.   When I was a kid in Britain, the soap in public bogs was liquid so you couldn't steal it.
729404
They yield K3PO4 and H2CO3.... Just switch the positive ion with the negative ion and make sure the charges cancel out to zero on each new salt.
151863
Either:\n\n(a) you're not getting a very clean separation, as the peaks should be vivid\n\nor\n\n(b) your detector is insuitable for the acids you're studying.\n\nAtleast, that's my analysis. Any A-Chem experts here?
959066
Try Wikipedia.org...Qualitative inorganic analysis. I was just there.
1024740
The question makes no sense.  A single, isolated anion has no pH value.  pH refers to the H+ concentration in aqueous solutions.
387966
The classical method is called Karl Fischer titration.\nIt's a little complex, but it's the generally accepted standard way assaying water content.\n\nThe overall reaction is:\n\nI2 + 2H2O + SO2 --> 2HI + H2SO4\n\nThis is done in the presence of a nitrogenous base (usually pyridine) to neutralize the acid produced. An anhydrous alcohol (often methanol) is used as the solvent. \n\nThe KF reagent is made by dissolving the base, I2 and SO2 in the desired alcohol. The sample is dissolved separately in the same alcohol. The KF reagent is then titrated into the sample solution until the I2 is no longer consumed. If you know how much I2 was required, you can calculate how much H2O was present in the sample.\n\nIn practice, there are machines which fully automate this process, so all you have to do is add your sample and wait for the results.\n\nYou can also weight your sample, dry it in an oven, weigh it again, and assume the difference in weight is due to loss of water. While this method will give an estimate of moisture contant, it doesn't have nearly the same accuracy, precision or specificity as the KF titration.
284896
One bit to add.  The only exception to this is the polyatomic ion, ammonium. (NH4+) It acts like the cation.
634218
There really is not a set formula, as the -ite anions don't have a set formula themselves (PO3 2- for phosphite, NO2- for nitrite, SO3 2- for sulfite, Cl02- for chlorite, etc.)
217892
Apart from the precipitation reactions (AgCl and BaCO3 form insoluble compounds, although HCl will dissolve BaCO3), there is flame colouring for identifying the alkali and earth alkali metals (Na yellowish orange, Li reddish, Ba green), there are pH measurements (HCl acidic, NaOH and Na2CO3 basic, rest neutral), and you need to test an oxidant to identify the sugar solution. This ought to give you a matrix which gives only one possible identification for each test (with deionized water failing all tests).
616395
This compund has an octahedral geometry and is coordinated with 3 bidentate oxalate (C2O4) ligands.\nReaction of potassium oxalate hydrate and ferric chloride\n\n3K2C2O4ˇH2O + FeCl3 --> K3[Fe(C2O4)3]ˇ3H2O + 3KCl\n\nWater molekules do not act as ligands and potassium ions act as counter-ions
846516
Yes, it actually is that simple. Potassium bonds very well to both chloride and bicarbonate. Potassium has a +1 charge, while both chloride and bicarbonate have a -1 charge.\n\nCheck out this site for a detailed description of these three electrolytes and their effect on the body:\n\nhttp://www.medicinenet.com/electrolytes/article.htm
185295
sodium hydrogen carbonate: [Na+][HCO3-].\n\nThe anion can release a proton:\n[HCO3-] -> H+ + [CO3(2-)]\n\nTherefore it can behave like an acid when it encounters a base, e.g.:\n\n[HCO3-] + NaOH -> [Na+][CO3(2-)] + H2O