The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be `10%.` If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be :
A
`5%`
B
`10%`
C
`20%`
D
None of these
Text Solution
AI Generated Solution
The correct Answer is:
To solve the problem, we need to analyze the degree of hydrolysis of a salt formed from a weak acid (HA) and a weak base (BOH). The problem states that in a 0.1 M solution, the percentage degree of hydrolysis is 10%. We need to find the percentage hydrolysis when the molarity of the solution is reduced to 0.05 M.
### Step-by-Step Solution:
1. **Understanding Degree of Hydrolysis**:
The degree of hydrolysis (α) is defined as the fraction of the salt that undergoes hydrolysis. For a salt formed from a weak acid and a weak base, the degree of hydrolysis can be expressed as:
\[
\alpha = \sqrt{\frac{K_w}{K_a \cdot K_b}}
\]
where \(K_w\) is the ionic product of water, \(K_a\) is the dissociation constant of the weak acid, and \(K_b\) is the dissociation constant of the weak base.
2. **Independence from Concentration**:
It is important to note that the degree of hydrolysis is independent of the concentration of the solution. This means that changing the concentration of the salt solution will not affect the degree of hydrolysis.
3. **Given Information**:
- For a 0.1 M solution, the percentage degree of hydrolysis is 10%.
- We need to find the percentage degree of hydrolysis for a 0.05 M solution.
4. **Conclusion**:
Since the degree of hydrolysis does not depend on the concentration, the percentage degree of hydrolysis for the 0.05 M solution will remain the same as that for the 0.1 M solution. Therefore, the percentage hydrolysis in the 0.05 M solution will also be:
\[
\text{Percentage Hydrolysis} = 10\%
\]
### Final Answer:
The percentage hydrolysis of the salt in a 0.05 M solution is **10%**.
Salt hydrolysis is an acid - base reaction of cation or anion or both ions of salt with water . The resultant solution after hydrolysis may be acidic , basic or neutral . The anion X^(-) which is weaker base than OH^(-) and which has its conjugate acid HX stronger than water but weaker than H_(3)O^(+) shows the phenomenon of hydrolysis , e.g CH_(3)COO^(-) , NO_(2)^(-) , CN^(-) etc. The cation M^(+) which is weaker acid than H_(3)O^(+) and which has its conjugate base MOH stronger than water but weaker than OH^(-) shows the phenomenon of hydrolysis , e.g N_(2)H_(5)^(+), C_(6)H_(5)NH^(+),NH_(4)^(+) etc . The degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 0.1 .If the molarity of the solution is 0.05 M , the percentage hydrolysis of salt should be :
The degree of hydrolysis of a salt of weak acid and weak base in its 0.1M solultion is found to be 50% . If the molarity of the solution is 0.2M , the percentage hydrolysis of the salt should be:
The degree of hydrrolysis of a salt of weak acid and weak base in its 0.1M solultion is found to be 50% . If the molarity of the solution is 0.2M , the percentage hydrolysis of the salt should be:
Degree of hydrolysis for a salt of strong acid and weak base:
The degree of hydrolysis of a salt of W_(A) and W_(B) in its 0.1M solution is 50% . If the molarity of the solution is 0.2M , the percentage hydrolysis of the salt woukd be
Degree hydrolysis (h) of a salt of weak acid and a strong base is given by
Degree of hydrolysis (alpha) for a salt of strong acid and weak base is :
Hydrolysis constant for a salt of weak acid and weak base would be
The hydrolysis constant of a salt of weak acid and weak base is inversely proportional to
If concentration of the salt its aqueous solution is increased , then degree of hydrolysis of the salt will be
