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Standard IX

Chemistry

Arrehenius Theory of Acids and Bases

When 73.0 g...

Question

When $73.0$ g of HCl are added to $1$ L of an acidic buffer, its pH changes from $3.4$ to $2.9$ . The buffer capacity of the buffer solution is :

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Solution

Moles of acid added $= \frac{M a s s}{M o l a r m a s s} = \frac{73}{36.5} = 2 m o l$

Buffer capacity $= \frac{N u m b e r o f m o l e s o f a c i d o r b a s e a d d e d t o a 1 L b u f f e r}{C h a n g e i n p H} = \frac{2}{3.4 - 2.9} = 4$

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When 73.0 g of HCl are added to 1 L of an acidic buffer, its pH changes from 3.4 to 2.9. The buffer capacity of the buffer solution is :

Moles of acid added =MassMolar mass=7336.5=2 molBuffer capacity =Numberofmolesofacidorbaseaddedtoa1LbufferChangeinpH=23.4−2.9=4

When $73.0$ g of HCl are added to $1$ L of an acidic buffer, its pH changes from $3.4$ to $2.9$ . The buffer capacity of the buffer solution is :

Moles of acid added $= \frac{M a s s}{M o l a r m a s s} = \frac{73}{36.5} = 2 m o l$

Buffer capacity $= \frac{N u m b e r o f m o l e s o f a c i d o r b a s e a d d e d t o a 1 L b u f f e r}{C h a n g e i n p H} = \frac{2}{3.4 - 2.9} = 4$