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A monoprotic acid can donate only one proton (+) per molecule, such as HCl. A diprotic acid can donate two protons per molecule, such as H₂SO₄. Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis acid? Define a conjugate acid-base pair. … Read more
The ionization constant (Ka) is the equilibrium constant for the dissociation of a weak acid in water. It measures the strength of an acid. A higher Ka value indicates a stronger acid. Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis … Read more
A strong acid completely dissociates in water, releasing all of its ions, whereas a weak acid only partially dissociates in water. Example: HCl is a strong acid, and CH₃COOH is a weak acid. Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a … Read more
Water is considered neutral because it has an equal concentration of hydrogen ions and hydroxide ions , both of which are present at 25°C, resulting in a pH of 7. Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis acid? Define … Read more
Acids have a pH less than 7, while bases have a pH greater than 7. A pH of 7 is considered neutral, such as pure water. Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis acid? Define a conjugate acid-base pair. … Read more
Neutralization reaction: A neutralization reaction is a chemical reaction between an acid and a base that produces water and a salt. For example, HCL + NAOH → NACL + H2O Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis acid? Define … Read more
Indicators are substances that change color to signal the endpoint of an acid-base titration. They help to visually indicate when the acid has been completely neutralized by the base (or vice versa). Related Questions: Define and give examples of Arrhenius acids? Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a … Read more
A conjugate acid-base pair consists of two species that differ by one proton (H⁺). The acid donates a proton, and the base accepts it. Example: NH3 + H2O ⇔ NH4+ + OH¯ In the reaction. NH3 and NH4+ , form a conjugate pair, as do H2O and OH¯. Related Questions: Define and give examples of Arrhenius … Read more
Because BF₃ can accept an electron pair from a donor, which is the characteristic behavior of a Lewis acid. Related Questions: Why H⁺ ion acts as a Lewis acid? Define and give examples of Arrhenius acids? Define a conjugate acid-base pair. What is the role of indicators in acid-base titrations? What is meant by the … Read more
Reason: A Lewis acid is an electron pair acceptor. The H⁺ ion has no electrons and can accept an electron pair, making it a Lewis acid. Related Questions: Why BF₃ acts as a Lewis acid? Define and give examples of Arrhenius acids? Define a conjugate acid-base pair. What is the role of indicators in acid-base … Read more