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- Consider the following reaction: $$ce {HCl + H2O -> H3O+ + Cl-}$$ Here HCl is a strong acid, thus Cl attracts the H atom less efficiently so that it can be easily dissociated. When Cl is a conjugate base in the product's side, the Cl has the same low efficiency of attracting H atom. Consequently it accepts the $ce {H+}$ ions less efficiently.
chemistry.stackexchange.com/questions/10650/why-do-strong-acids-have-weak-conjugate-basesWhy do strong acids have weak conjugate bases? - Chemistry ...
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Jul 12, 2023 · Similarly, in the reaction of ammonia with water, the hydroxide ion is a strong base, and ammonia is a weak base, whereas the ammonium ion is a stronger acid than water. Hence this equilibrium also lies to the left: \[H_2O_{(l)} + NH_{3(aq)} \ce{ <<=>} NH^+_{4(aq)} + OH^-_{(aq)} \nonumber\]
- 16.6: Polyprotic Acids
Solution. As indicated by the ionization constants, H 2 CO 3...
- 4.7: Acid Base Reactions
The reaction of a weak acid and a strong base will go to...
- 16.6: Polyprotic Acids
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.
Jul 4, 2022 · The reaction of a weak acid and a strong base will go to completion, so it is reasonable to prepare calcium propionate by mixing solutions of propionic acid and calcium hydroxide in a 2:1 mole ratio. Exercise \(\PageIndex{2}\)
ethanoic acid + sodium hydroxide → sodium ethanoate + water. CH3COOH + NaOH → CH3COONa + H2O. Weak acids such as ethanoic acid, CH 3 COOH, and hydrofluoric acid, HF, only partially ionise in water, producing solutions of pH values between 4 – 6.
May 30, 2020 · First, let reactions go to completion (in the direction that makes sense, i.e. weak base and strong acid forms weak acid and spectator ion - never the other way around). Then, check what the major species are and estimate the pH.
May 12, 2014 · Consider the following reaction: $$\ce{HCl + H2O -> H3O+ + Cl-}$$ Here HCl is a strong acid, thus Cl attracts the H atom less efficiently so that it can be easily dissociated. When Cl is a conjugate base in the product's side, the Cl has the same low efficiency of attracting H atom.
Sep 27, 2022 · Any acid that dissociates 100% into ions is called a strong acid. If it does not dissociate 100%, it is a weak acid. Acetic acid (\(\ce{HC2H3O2}\)) is an example of a weak acid: \[\ce{HC2H3O2 \overset{\sim 5\%}{\longrightarrow} H^{+}(aq) + C2H3O2^{-}(aq)} \nonumber \]
