An acid-base titration is a quantitative analysis for estimating the concentration of an acid/base that has been suitably neutralized with a standard solution of a known concentration of acid or base. The endpoint and progress of the acid-base reaction are monitored using a pH indicator. Titration can be done with practically any chemical reaction that has a known balanced chemical equation.
Why are strong acids generally used as standard solutions in acid base titration?
- The salts of strong acids do not hydrolyse
- The pH at the equivalence point will always be 7
- They can be used to titrate both strong and weak bases
- Strong acids form more stable solutions than weak acids
The correct option is 3: They can be used to titrate both strong and weak bases
Explanation:
Strong acids are generally used as standard solutions in acid-base titrations since strong acids can react with both strong and weak bases, they are commonly employed as standard solutions in acid-base titrations.
The following are some examples of strong acids used in the acid-base titration.
- Hydrochloric acid (HCl)
- Sulfuric acid (H2SO4)
- Nitric acid (HNO3)
- Perchloric acid (HClO4)
- Hydrobromic acid (HBr)
- Hydroiodic acid (HI)
- Chloric acid (HClO3)
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