1.

The ionization constant of nitrous acid is 4.5 times 10^-4. Calculate the pH of 0.04 M solution nitrite solution and also its degree of hydrolysis.

Answer»

SOLUTION :Sodium nitrite is a salt of WEAK acid, strong base, HENCE,
`K_h=2.22 times 10^-11 K_w//K_a=10^-14//(4.5 times 10^-4)`
`h=sqrt(K_h//C)=sqrt(2.22 times 10^-11//0.04)=sqrt(5.5 times 10^-11)=2.36 times 10^-5`
INITIAL c
After hydrolysis c-ch ch ch
`[OH^-]=ch=0.04 times 2.36 times 10^-5=9.44 times 10^-7`
`pOH=-log(9.44 times 10^-7)=7-0.9750=6.03`
`pH=14-pOH=14-6.03=7.97`


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