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- Now, if you had more acid than base in this reaction, not all of the acid would react, so the result would be salt, water, and leftover acid, so the solution would still be acidic (pH < 7). If you had more base than acid, there would be leftover base and the final solution would be basic (pH > 7).
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Jul 4, 2022 · Acid–base reactions require both an acid and a base. In Brønsted–Lowry terms, an acid is a substance that can donate a proton (H +), and a base is a substance that can accept a proton. All acid–base reactions contain two acid–base pairs: the reactants and the products.
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Sep 19, 2018 · If you mix equal amounts of a strong acid and a strong base, the two chemicals essentially cancel each other out and produce a salt and water. Mixing equal amounts of a strong acid with a strong base also produces a neutral pH (pH = 7) solution.
- Anne Marie Helmenstine, Ph.D.
Pure water, which is neutral, has a pH of 7. A solution with a pH less than 7 is considered acidic, and a solution with a pH greater than 7 is considered basic, or alkaline. Strong acids have a higher concentration of hydrogen ions, and they are assigned values closer to 0.
Jun 13, 2023 · The acid produces hydrogen ions, and the base produces hydroxide ions. These react together to make water. The anion that came from the acid and the cation are left, so if you evaporate the water, you would get a salt.
A number of common strong acids, including hydrochloric acid (\(\mathrm{HCl}\)), sulfuric acid (\(\mathrm{H}_{2}\mathrm{SO}_{2}\)), and nitric acid (\(\mathrm{HNO}_{2}\)), react with a strong base such as \(\mathrm{NaOH}\) or \(\mathrm{KOH}\) (which, like strong acids, dissociate completely in water) to produce water..
Jan 13, 2024 · The outcome of an acid-base reaction depends on the strength of the acids and bases. Strong Acid with Strong Base: This leads to complete neutralization, forming a neutral salt and water. Example: HCl (acid) + NaOH (base) → NaCl (salt) + H₂O (water).
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Acid: HCl (g) + H 2 O → → H + (aq) + Cl – (aq) (sometimes written as or HCl (aq)) Base: NaOH (s) + H 2 O → → Na + (aq) + – OH (aq) Acid–Base Reaction: HCl (aq) + NaOH (aq) → → NaCl (aq) + H 2 O (l) [2] Although simple, the Arrhenius model is not particularly useful when it comes to understanding the reactions considered in organic chemistry.
