What characteristic of a base enables it to ''accept'' Hydrogen Ions?

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SUMMARY

The discussion clarifies the Brønsted-Lowry definition of acids and bases, stating that a base is a compound capable of accepting hydrogen ions (H+), while an acid is one that donates H+. The reaction of hydrochloric acid (HCl) in water produces H+ and Cl− ions, and the interaction of H+ with hydroxide ions (OH−) forms water (H2O). It is emphasized that H3O+ is the conjugate acid formed when HCl protonates water, and the equilibrium of these reactions is influenced by pKa values.

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  • Understanding of the Brønsted-Lowry acid-base theory
  • Familiarity with chemical equilibrium concepts
  • Knowledge of ionization reactions in aqueous solutions
  • Basic grasp of pKa and its significance in acid-base chemistry
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  • Study the concept of pKa and its role in determining acid strength
  • Explore the equilibrium constant expressions for acid-base reactions
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  • Investigate the role of water as an acid and base in various chemical reactions
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LogicalAcid
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According to the Brønsted-Lowry definition, a base is a compound that can -keyword- accept H+, and an acid anything that can give H+.
 
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Someone please clarify this for me.

And also, here is something

HCl → H+ + Cl− ( I am guessing the arrow is referring to before and after being put in water)


The addition of H+ to the hydroxide ion (OH−), a base, produces water (H2O), its conjugate acid:

H+ + OH− → H2O ( and I am guessing this is after it ionizes and reacts with water?)
 
Be careful how you label your species here. OH- can be seen as a base (and a nucleophile) but H2O is not the conjugate acid in the sense that you mean, H3O+ would be the 'acid'. This is because (using your HCl equation) HCl does not simply become two separate ions in solution. The acid will protonate H2O to become H3O+.

But remember, all these reactions are in equilibrium and the pKa determines to what extent the different species exist.

H20 <---> H+ + OH-

HCl <---> H+ + Cl-

H2O + H+ <---> H3O+
 

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