Examples of strong base in the following topics:
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- Strong bases either dissociate completely in solution to yield hydroxide ions, or deprotonate water to yield hydroxide ions.
- A strong Arrhenius base, like a strong acid, is a compound that ionizes completely or near-completely in solution.
- Strong bases are capable of deprotonating weak acids; very strong bases can deprotonate very weakly acidic C–H groups in the absence of water.
- When writing out the dissociation equation of a strong base, assume that the reverse reaction does not occur, because the conjugate acid of a strong base is very weak.
- Unlike weak bases, which exist in equilibrium with their conjugate acids, the strong base reacts completely with water, and none of the original anion remains after the base is added to solution.
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- A weak acid will react with a strong base to form a basic (pH > 7) solution.
- Titrations are reactions between specifically selected reactants—in this case, a strong base and a weak acid.
- The titration curve demonstrating the pH change during the titration of the strong base with a weak acid shows that at the beginning, the pH changes very slowly and gradually.
- This figure depicts the pH changes during a titration of a weak acid with a strong base.
- Distinguish a weak acid-strong base titration from other types of titrations.
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- A strong acid will react with a strong base to form a neutral (pH = 7) solution.
- A strong acid-strong base titration is performed using a phenolphthalein indicator.
- In the case of a strong acid-strong base titration, this pH transition would take place within a fraction of a drop of actual neutralization, since the strength of the base is high.
- It is often wrongly assumed that neutralization should result in a solution with pH 7.0; this is only the case in a strong acid and strong base titration.
- Calculate the concentration of an unknown strong acid given the amount of base necessary to titrate it.
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- A strong acid will react with a weak base to form an acidic (pH < 7) solution.
- An example of a strong acid-weak base titration is the reaction between ammonia (a weak base) and hydrochloric acid (a strong acid) in the aqueous phase:
- In the case of titrating the acid into the base for a strong acid-weak base titration, the pH of the base will ordinarily start high and drop rapidly with the additions of acid.
- In strong acid-weak base titrations, the pH at the equivalence point is not 7 but below it.
- Recall that strong acid-weak base titrations can be performed with either serving as the titrant.
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- strong acid-weak base titration: methyl orange indicator the base is off the scale (e.g., pH > 13.5) and the acid has pH > 5.5: alizarine yellow indicator
- A strong acid will react with a weak base to form an acidic (pH < 7) solution.
- A strong acid will react with a strong base to form a neutral (pH = 7) solution.
- A weak acid will react with a strong base to form a basic (pH > 7) solution.
- It is filled with a solution of strong acid (or base) of known concentration.
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- The six common strong acids are:
- By definition, a strong acid is one that completely dissociates in water; in other words, one mole of the generic strong acid, HA, will yield one mole of H+, one mole of the conjugate base, A−, with none of the unprotonated acid HA remaining in solution.
- A strong base is the converse of a strong acid; whereas an acid is considered strong if it can readily donate protons, a base is considered strong if it can readily deprotonate (i.e, remove an H+ ion) from other compounds.
- Most alkali metal and some alkaline earth metal hydroxides are strong bases in solution.
- The alkaline earth metal hydroxides are less soluble but are still considered to be strong bases.
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- Acid names are based on the anion they form when dissolved in water; base names follow the rules for ionic, organic, or molecular compounds.
- Most strong bases contain hydroxide, a polyatomic ion.
- Therefore, strong bases are named following the rules for naming ionic compounds.
- For example, methyl amine (CH3NH2) is a weak base.
- Some weak bases have "common" names.
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- In water, strong acids completely dissociate into free protons and their conjugate base.
- where HA is a protonated acid, H+ is the free acidic proton, and A- is the conjugate base.
- Strong acids yield weak conjugate bases.
- Strong acids, like strong bases, can cause chemical burns when exposed to living tissue.
- Strong acids can accelerate the rate of certain reactions.
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- A weak base is a chemical base that does not ionize fully in an aqueous solution.
- As Brønsted-Lowry bases are proton acceptors, a weak base may also be defined as a chemical base with incomplete protonation.
- A general formula for base behavior is as follows:
- This results in a relatively low pH compared to that of strong bases.
- The pH of bases in aqueous solution ranges from greater than 7 (the pH of pure water) to 14 (though some bases have pH values greater than 14).
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- Most base reagents are alkoxide salts, amines or amide salts.
- Since alcohols are much stronger acids than amines, their conjugate bases are weaker than amide bases, and fill the gap in base strength between amines and amide salts.
- Hünig's base is relatively non-nucleophilic (due to steric hindrance), and like DBU is often used as the base in E2 elimination reactions conducted in non-polar solvents.
- Barton's base is a strong, poorly-nucleophilic, neutral base that serves in cases where electrophilic substitution of DBU or other amine bases is a problem.
- Finally, the two amide bases see widespread use in generating enolate bases from carbonyl compounds and other weak carbon acids.