is hbro4 acid or base?
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Perbromic acid is a strong acid and strongly oxidizing. It is the most unstable of the halogen(VII) oxoacids. It decomposes rapidly on standing to bromic acid and oxygen. It reacts with bases to form perbromate salts.
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Monoprotic acids, like HCl and HBr, contain just one hydrogen ion. Polyprotic acids, like H2 SO4 and H3 PO4, contain two or three hydrogen ions. It's tempting to think that polyprotic acid are stronger than monoprotic acids because they contain multiple hydrogen ions, but that's actually not true.
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In reactions of alkyl halides (substitution( CN reactions) or elimination) the X ion will be released and will generate a strong acid(HF,HCl,HBr,HI). So the relative acidity of an alkyl halide is due to the X ion present.
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HCl is a stronger acid than HF because fluorine is more electronegative than chlorine.
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The compound perbromic acid is the inorganic compound with the formula HBrO4. It is an oxoacid of bromine. Perbromic acid is unstable and cannot be formed by displacement of chlorine from perchloric acid, as periodic acid is prepared; it can only be made by protonation of the perbromate ion.
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The same reasoning applies for both HBr and HI. These acids are even stronger than HCl because the Br– and I– ions are even larger. As such, the H-Br and H-I bonds are even weaker, and these compounds also readily dissociate in solution.
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And since the Bronsted-Lowry definition of a base is a Proton (H^+) acceptor, it is a very strong base as the OH^- will accept a proton very readily from the acid ( which is classed as a Proton donor ) as its negative charge makes it a very strong nucleophile.
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Now as we know, a strong acid will have a weak conjugate base. Since HI is the strongest acid, Iodide ion will be the weakest conjugate base within the group. So the order for increasing basic character is I<Br<Cl<F. ... Hence it will be a better leaving group than flouride ion.
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Cl, Br, and I are all so big that they form very poor bonds to hydrogen that is why HCl, HBr and HI are strong acids. ... Only F, O, and N are the right size and have a high enough electronegativity to form hydrogen bonds (to a hydrogen that is attached to one of these on another molecule).
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Metal hydrides, metal oxides, and metal hydroxides are bases. Nonmetal hydrides, nonmetal oxides, and nonmetal hydroxides are acids. The acidic hydrogen atoms in the non-metal hydroxides in the table above aren't bound to the nitrogen, sulfur, or phosphorus atoms.
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The 7 common strong acids are: HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 (1st proton only). ... Remember what we mean by a weak acid or weak base. They simply do not ionize completely whereas a strong acid or base does.
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Chemistry. Explain why the solubility of PbF2 is pH dependent, but the solubility of PbCl2 is not. ... So the solubility equilibrium of PbF2 is shifted to the right as the concentration of F^- ions is reduced by the protonation to form HF. I know the conjugate base of PbCl2 is HCL, making a strong acid that does not ionize ...
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If one of those ions is H+, the solution is acidic. The strong acid hydrogen chloride (HCl) is one example. If one of the ions is OH-, the solution is basic. An example of a strong base is sodium hydroxide (NaOH).
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In terms of its acid–base properties, chloride is a very weak base as indicated by the negative value of the pKa of hydrochloric acid. Chloride can be protonated by strong acids, such as sulfuric acid: NaCl + H2SO4 → NaHSO4 + HCl. Ionic chloride salts reaction with other salts to exchange anions.
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Acid Strength and Bond Strength HCl, HBr, and HI are all strong acids, whereas HF is a weak acid.
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Ammonium bromide, NH4Br, is the ammonium salt of hydrobromic acid. The chemical crystallizes in colorless prisms, possessing a saline taste; it sublimes on heating and is easily soluble in water.
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Answer and Explanation: HBr, or hydrobromic acid, is a strong acid. When placed in water, HBr completely dissociates into H+ and Br-.