Examples of strong acid in the following topics:
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- In water, strong acids completely dissociate into free protons and their 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.
- p-Toluenesulfonic acid is an example of an organic soluble strong acid, with a pKa of -2.8.
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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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- 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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- The stereoselectivity of Brønsted acid addition is sensitive to experimental conditions such as temperature and reagent concentration.
- Of all the reagents discussed here, these strong acid additions (E = H in the following equation) come closest to proceeding by the proposed two-step mechanism in which a discrete carbocation intermediate is generated in the first step.
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- The acid dissociation constant (Ka) is the measure of the strength of an acid in solution.
- This is because strong acids are presumed to ionize completely in solution and therefore their Ka values are exceedingly large.
- Acids with a pKa value of less than about -2 are said to be strong acids.
- A strong acid is almost completely dissociated in aqueous solution; it is dissociated to the extent that the concentration of the undissociated acid becomes undetectable. pKa values for strong acids can be estimated by theoretical means or by extrapolating from measurements in non-aqueous solvents with a smaller dissociation constant, such as acetonitrile and dimethylsulfoxide.
- Acetic acid is a weak acid with an acid dissociation constant $K_a=1.8\times 10^{-5}$ .
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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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- 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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- 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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- Diprotic and polyprotic acids contain multiple acidic protons that dissociate in distinct, sequential steps.
- As their name suggests, polyprotic acids contain more than one acidic proton.
- Two common examples are carbonic acid (H2CO3, which has two acidic protons and is therefore a diprotic acid) and phosphoric acid (H3PO4, which has three acidic protons and is therefore a triprotic acid).
- This first dissociation step of sulfuric acid will occur completely, which is why sulfuric acid is considered a strong acid; the second dissociation step is only weakly dissociating, however.
- Identify the key features that distinguish polyprotic acids from monoprotic acids.
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- Simple acids, known as binary acids, have only one anion and one hydrogen.
- So, HNO3 will be nitric acid.
- For example, instead of bromic acid, HBrO3, we have hypobromous acid, HBrO.
- Most strong bases contain hydroxide, a polyatomic ion.
- Therefore, strong bases are named following the rules for naming ionic compounds.