Question

❥Notes of acidic strength❤❤
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don't post unnecessary answer​

Answer 1

Explanation:

Greater the number of H+lions produced in the aqueous solution. the stronger is the acid. Greater the number of OH_ions produced in the aqueous solution ,the stronger in the base . As greater is the dissociation constant of the weak acid (Ka) ,greater is the amount of H+ (aq) produced , therefore stronger is the acid.

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Answer 2

$\bigstar\huge\boxed{\mathtt{\red{Acidic \: strength :}}}$

• In order to explain it in simple words it is an ability of an acid to lose its H + ion

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$\rightarrow\large\boxed{\mathtt{\orange{Basic\: physical\: and\: \\chemical \: properties \: of\: acids:}}}$

• pH - below 7 ( 1 - 6 )
• They turn blue litmus paper red
• Taste - sour
• acids react with bases in order to form salts

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$\rightarrow\large\boxed{\mathtt{\orange{Strong\: acids : } }}$

• completely ionize into their constituent ions in a solution
• They act as proton donors in the solution
• corrosive in nature
• E g : HCl - Hydrochloric acid , H2SO4 -Sulphuric acid,HClO4 -Perchloric acid , HI - hydroiodic acid ,HNO3 -Nitric acid

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$\rightarrow\large\boxed{\mathtt{\orange{Weak\: acids : } }}$

• partially ionizes in the solution /aqueous medium
• mildly corrosive (present in our body and food )

• E g : citric acid(weakest) , ethanoic acid ,acetic acid etc .

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$\rightarrow\large\boxed{\mathtt{\orange{Factors\: affecting\: acidic\: strength: } }}$

• Generally the strength of the HA bond is inversely proportional to its acidity , it means that stronger is the HA  bond weaker is the acid .

1. when we go down the group the size of A increases ,due to which the strength of HA bond decreases and acidity increases .In short we can conclude that acidity goes on increasing as we go down the group
2. Bond strength plays an important role in determining acidity when we go down the group

• The greater is the polarity of HA bond stronger  is the acid

1. polarity directly affects the strength of the acid ,means that if HA is a strong acid then  the H-A bond will be highly polar that means the proton will leave the molecule easily(as H-A has weaker bond strength as discussed in point 1 )
2. polarity plays a very important role in determining the acidity as we go across the period

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$\rightarrow\large\boxed{\mathtt{\orange{Relative\: strength\: of\: inorganic\: acids : } }}$

Hydrides

• The acidic strength increases with the increase in electronegativity

eg: H-F >H-OH >H- NH2 > H- CH3

• The acidic strength increases with the increase in the atomic size

eg : HF <HCl< HBr< HI

Oxyacids :

• Among oxyacids of the same type formed by different elements the acidic nature increases with increasing electronegativity

eg: HOI < HOBr< HOCl

• In oxyacids of the same element ,acidic nature increases with its oxidation number

eg: HOCl(+1) < HClO2(+3) < HClO3(+5)  < HClO4 (+7)

• The strength of oxyacids increases from left to right across a period

eg: H4SiO4< H3PO4 <H2SO4< HClO4

• for same oxidation state and configuration of elements acidic strength decreases with increase in size of the atom

eg: HClO4 >HBrO4 >HIO4

$\rightarrow\large\boxed{\mathtt{\orange{Relative\: strength\: of\: organic\: acids : } }}$

• A compound is acidic in nature, only if its conjugate base can stabilize through resonance

1. eg : phenol (acidic )- conjugate base of phenol (C6H5O-)
2. ethanol (neutral ) conjugate base of phenol (C2H5O-)

• Hydrogen atom attached to sp hybridised carbon is more acidic than sp 2 hybridised carbon which in turn is more acidic than sp3