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Weak and strong should not be mistaken for dilute and concentrated. A dilute acid has the acid molecules mixed with a large amount of water, so that there is only a low concentration of H + ions.
A dilute acid or base solution is therefore one that has much fewer acid or base molecules per dm 3 of solution, hence the pH value would lie between 5 and 9; It does not necessarily mean that the acid or base is strong as it may be made from a weak acid or base which does not dissociate completely but a lot of it was added to the solution
Jan 7, 2011 · Strong and weak acids of the same concentrations react differently with reactive metals; This is because the concentration of H + is greater in strong acids compared to weak acids; The greater H + concentration means that more H 2 gas is produced . The diagram shows the reaction of 0.1 mol dm-3 of a strong acid (HCl) with Mg.
Sep 16, 2022 · Contributions & Attributions. 14.7: Strong and Weak Acids and Bases is shared under a CK-12 license and was authored, remixed, and/or curated by Marisa Alviar-Agnew & Henry Agnew. Acids are classified as either strong or weak, based on their ionization in water. A strong acid is an acid which is completely ionized in an aqueous solution.
Jul 4, 2022 · A neutralization reaction (a chemical reaction in which an acid and a base react in stoichiometric amounts to produce water and a salt) is one in which an acid and a base react in stoichiometric amounts to produce water and a salt (the general term for any ionic substance that does not have OH− as the anion or H+ as the cation), the general ...
Jul 12, 2023 · Thus the conjugate base of a strong acid is a very weak base, and the conjugate base of a very weak acid is a strong base. The conjugate base of a strong acid is a weak base and vice versa. We can use the relative strengths of acids and bases to predict the direction of an acid–base reaction by following a single rule: an acid–base ...
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When a weak acid and a strong base are mixed, they react according to the following net-ionic equation: HA(aq) + OH⁻(aq) → A⁻(aq) + H₂O(l). If the acid and base are equimolar, the pH of the resulting solution can be determined by considering the equilibrium reaction of A⁻ with water. If the acid is in excess, the pH can be determined from the concentrations of HA and A⁻ after the ...
