The following substances act as Brønsted acids in water. Write a chemical equation for each that illustrates its reaction with water. \n\na.hydrofluoric acid, HF\nb.ammonium ion, NH4 \nc.carbonic acid, H2CO3 \nd.nitrous acid, HNO2
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A Bronsted acid is a substance which releases H+ in water.\n\nHF + H2O --> F- + H3O+\n\nNH4+ + H2O --> NH3+ H3O+\n\nH2CO3 + H2O --> HCO3- + H3O+\n\nHNO2 + H2O --> NO2- + H3O+\n\nNote that the final result is always the hydronium ion \n(H3O+)
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It will be clearer if you write the reaction as the sum of two reactions.\n\nWhen HN3 is dissolved in water, it reacts with the water to form ammonium ion (NH4+) and hydroxide ion (OH-).  Omitting the reaction NH3(g) = NH3(aq), we have:\n\nNH3 (aq) + H2O (L) = NH4+(aq) + OH-(aq)\n\nThe equilibrium constant for this reaction is:\n\nKb = [NH4+]*[OH-]/[NH3]\n\nThe hydroxide produced in this reaction reacts with the manganese ion to form insoluble manganese hydroxide (Ksp ~ 2*10^-13)\n\nMn++(aq) + 2OH-(aq) = Mn(OH)2(s)\n\nThe equilibrium constant for this reaction is:\n\nK = 1/Ksp = 1/([Mn++]*[OH-]^2) \n\nThe reaction you wrote is the sum of 2 times the first reaction plus the second reacton.  Note that as written, the first reaction produces OH- ions while the second one consumes them.  \n\nIf we add an acid like HNO3 to the solution, we are adding H+ ions.  Adding H+ ions is really like subtracting OH- ions because the concentrations of H+ and OH- are inversely proportional to one another through the water dissociation reaction (H2O = H+ + OH-, [H+]*[OH-] = Kw = 10^-14).\n\nWe can therefore write the two equilbrium constants above in terms of the concentration of H+ instead of OH-:\n\nKb = [NH4+]*[OH-]/[NH3] = Kw*[NH4+]/([NH3]*[H+])\n\nK = 1/([Mn++]*[OH-]^2) = ([H+]^2)/(Kw^2 * [Mn++])\n\nThis means that if we add acid (i.e., HNO3) to the solution, we will drive the first reaction in the forward direction; the concentration NH4+ will increase and the concentration of NH3(aq) will decrease.  Adding H+ will drive the second reaction in the reverse direction; Mn(OH)2(s) will dissolve, and the concentration of Mn++ will increase.
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HCL acid  is acting as a substitution,neutralization or a gas formation reaction on each ion in the compound:\n\n    given reactants :\n\nNaAl(OH)2CO3(s) and HCl(aq)\n\nreactions:\n \n1. Na+(aq) + HCl(aq)->NaCl(aq) + 2H+(aq)\n\n2. Al3+(aq) + 3HCl(aq)->AlCl3(aq) +  2H+(aq) \n\n3. 2OH-(aq) + 2H+(aq)->2H2O(l)\n\n4. CO3-2(aq) + 2H+(aq)->CO2(g) + H2O(l)\n\nadding equations 1 thru 4  and canceling on both sides \nwill give you the overall equation,\n\nNaAl(OH)2CO3(s) + 4HCl(aq)-> NaCl(aq) + AlCl3(aq) + 3H2O(l) + CO2(g)
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b,\n\nall the others are ionic compounds.
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Here is the right equation for nitric acid and sodium bicarbonate\n\n\nHNO3 + NaHCO3 ---> NaNO3 + H2O + CO2\n\nIf you do not like the sodium:\n\nHNO3 + HCO3(-) --> NO3(-) + H2O + CO2
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Baking soda is sodium bicarbonate. Bicarbonate is a form of carbon dioxide reacted with water. Gases, such as carbon dioxide remain in liquids more readily at colder temperatures. So adding baking soda and ice to water will, in effect, carbonate the water.
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CO2\nCarbon Dioxide\nHere is the reaction:\nHC2H3O2(aq) + NaHCO3(aq) ----> NaC2H3O2(aq) + H2O(l) + CO2(g)
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Li2O + CO2 ---> LiOH\nNa2O2 + CO2 ----> Na2CO3 + O2\nKO2 + CO2 ---->  K2CO3  + O2
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When a salt derived from a strong acid and a weak base dissolves in water, the solution becomes acidic. For example, consider the process\n \nNH4Cl(s) ----H2O ---> NH4+(aq) + Cl-(aq)\n\nThe Cl- ion has no affinity for H+. The ammonium ion NH4+ is  a weak conjugate acid of the base NH4+(aq) and ionizes as follows \n\nNH4+(aq) + H2O(l) <=> NH3(aq) + H3O+(aq)\n\nor simply  \n\nNH4+(aq) <=> NH3(aq)  + H+(aq)\n\nThe equilibrium constant ( or ionization constant) for this process is given by \n\n\n\nKa = Kw / kb  =   1.0*10^-14 / 1.8*10^-5 = 5.6*10^-10\n\n\n      x^2 / .10 =  5.6*10^-10\n\n           x^2  =   5.6*10^-11\n\n             x  =    7.5*10^-6 M  =  [H+]\n\npH  =  -log [H+]\n    \n    =  5.12\n\n     my answer is  C , NH4Cl
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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)
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The first reaction is simply wrong.  Nitrous acid does not ionize to nitrate.\n\nThe second reaction is a precipitation reaction, showing the net ionic equation.  The compound is ionic.\n\nThe third reaction is an example of SN2 displacement, not elimination.  Only single bonds are formed.
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1) b)\n\n2) [H2O]^2 / 2[H2] [O2]\n  \n   [NO]^2 / [N2] [O2]\n\n3) b)\n\n4) b)
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In the first reaction, the base is NH2-, and the conjugate acid is NH3 (ammonia).\n\nIn the second reaction, the acid is HClO4 (perchloric acid) and the conjugate base is ClO4- (perchlorate).\n\nIn the third reaction, the acid is HSO4- (hydrogen sulfate) and the base is CO3-2 (carbonate). The conjugate base of HSO4- is SO4-2 (sulfate) and the conjugate acid of CO3-2 is HCO3- (hydrogen carbonate).
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NaOH (Base) + HNO3 (Acid) -> NaNO3 (Salt) + H2O (Water)\n   H  H H\n   |  | |\nH-C-C-C-H\n   | | |\n   H H H\n\nReplace the last H by an -O-H\n\nDraw the carbon skeleton first.
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It's easy. Just remember that carbon dioxide can dissolve in water to form carbonic acid. i.e. CO2(gas) + H2O(aqueous) => H2CO3 (aqueous)
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H2SO4 will dehydrate and remove water.\n\n\n(CH3)2 CH - CH2-CH=CH-(CH3)2
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H2+O2-->H2O\nNaOH+HCl-->NaCl+H2O\nKOH-->(on heating,deomposition)K2O+H2O\ni guess this is what u want\nand i f u didn't get it i am sorry......