is nahso3 acidic or basic?
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Since Ka > Kb, solution of NaHSO3 are acidic. Methylammonium nitrate is an acidic salt. Its cation, CH3NH3+, is a weak acid.
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One way of thinking about it is that calcium is a metal and therefore forms a basic oxide, CaO. On the other hand, sulfur is a non-metal and forms acidic oxides SO2 (or SO3). So, the reaction between CaO and SO2 can be considered an acid-base reaction.
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Nitric acid (HNO3) is considered to be a strong acid because it ionizes readily in water, dissolving into H+ and NO3- ions The H+ ion, also called a hydroxyl ion, makes the solution an acid by definition, giving it its typical acidic properties.
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HSO4- is the conjugate base of H2SO4 but it can still give its Hydrogen away, and thus it is a weak acid as well. It's weak because it doesn't part with its hydrogen as easily as H2SO4 did. What characterizes a strong acid or base?
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- Salts of weak bases and strong acids: pH less than 7 (acidic). - Salts from strong bases and weak acids: pH greater than 7 (alkaline). Based on these rules, the solution of Cu(NO3)2 dissolved in water is Acidic.
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If you see any other acid or base than one of these strong ones it will be a weak acid or base (unless I specifically say otherwise in the problem). The 7 common strong acids are: HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 (1st proton only). ... They simply do not ionize completely whereas a strong acid or base does.
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Anything less than 7 is acidic, anything greater than 7 is alkaline (or basic) and if it has a pH 7 then it's considered neutral! For example, Lemon Juice is acidic, water is neutral and toothpaste is alkaline.
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Summary of Acidic and Basic Salts Acid salts are the converse of basic salts; they are formed in the neutralization reaction between a strong acid and a weak base. The conjugate acid of the weak base makes the salt acidic. ... The ammonium ion contains a hydrolyzable proton, which makes it an acid salt.
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For example, NH4Br is the salt of a weak base (NH3) and a strong acid (HBr), so the salt is acidic. ... This means that two of the solutions are basic (NH3 and NaF), one solution is neutral (NaCl), and the other is acidic (NH4Br).
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Hence we can say that a salt of WASB (Weak acid Strong Base) on dissolution in water makes the solution basic. Simmilarly, A salt of SASB will make solution neutral as both acid and base are strong hence ionizes completely and equal concentration of H+ and OH- ions.
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HSO4- is an acidic anion because it tends to donate protons when in pure water. Notice how the first arrow is not an eqilibrium - it fully dissociates and the second only partially so some of the HSO4- will donate protons. Only in a very acidic environment would HSO4- act as a base.
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Thus H + is an acid by both definitions, and OH − is a base by both definitions. Ammonia (NH 3) is a base even though it does not contain OH − ions in its formula.
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Salts can have acidic or basic pKa depending on the strength of original acid and bases from which they are derived. In this case Zn(OH)2 is a weak base and H2SO4 is a strong acid; therefore ZnSO4 has acidic pKa.
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Acidity/basicity Ionic compounds containing hydrogen ions (H+) are classified as acids, and those containing electropositive cations and basic anions ions hydroxide (OH−) or oxide (O2−) are classified as bases. Other ionic compounds are known as salts and can be formed by acid–base reactions.
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Primary Standards for Acid-Base Titrations Nitric acid, HNO3, is NOT suitable for use as a primary standard because it always contains a little nitrous acid, HNO2, which has a destructive action on many acid-base indicators.
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FeCl3 is an acid salt because Fe(OH)3 is weak base and HCl is a strong acid. pH is less than 7.
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A substance that accepts and H+ from water is considered a base. Both NH3 and H2O are amphoteric (they have H atoms that can be donated as H+ ions and thus act as acids and lone-pair electrons that can accept an H+ and thus act as bases). Thus, either NH3 or H2O can act as an acid or a base.