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The degree of dissociation of weak elect...

The degree of dissociation of weak electrolyde is inversely proportional to the square root fo concentration. It is called Ostwald's dilution law.
`alpha = sqrt((K_(a))/(c))` As the tempertaure increases, degree of dissociation will increase.
`(alpha_(1))/(alpha_(2)) = sqrt((K_(a_(1)))/(K_(a_(2))))` if concentration is same.
`(alpha_(1))/(alpha_(2)) = sqrt((c_(2))/(c_(1)))` if acid is same.
`a_(1)` and `a_(2)` are in ratio of `1:2, K_(a_(1)) = 2xx10^(-4)`. What will be `K_(a_(2))`?

A

`8 xx 10^(-4)`

B

`2xx10^(-4)`

C

`4 xx 10^(-4)`

D

`1xx10^(-4)`

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To solve the problem, we will use the provided relationships and the given information step by step. ### Step 1: Understand the given information We know that: - The degree of dissociation (α) of a weak electrolyte is inversely proportional to the square root of its concentration (c). - The relationship is given by Ostwald's dilution law: \[ \alpha = \sqrt{\frac{K_a}{c}} \] - We have two acids with degrees of dissociation α₁ and α₂, where α₁:α₂ = 1:2. - The dissociation constant for the first acid is given as \( K_{a1} = 2 \times 10^{-4} \). ### Step 2: Set up the ratio of degrees of dissociation From the problem, we have: \[ \frac{\alpha_1}{\alpha_2} = \frac{1}{2} \] ### Step 3: Use the relationship for the same concentration Since the concentration is the same for both acids, we can use the formula: \[ \frac{\alpha_1}{\alpha_2} = \sqrt{\frac{K_{a1}}{K_{a2}}} \] ### Step 4: Substitute the known values into the equation Substituting the values we have: \[ \frac{1}{2} = \sqrt{\frac{2 \times 10^{-4}}{K_{a2}}} \] ### Step 5: Square both sides to eliminate the square root Squaring both sides gives: \[ \left(\frac{1}{2}\right)^2 = \frac{2 \times 10^{-4}}{K_{a2}} \] \[ \frac{1}{4} = \frac{2 \times 10^{-4}}{K_{a2}} \] ### Step 6: Rearrange to solve for \( K_{a2} \) Rearranging the equation to solve for \( K_{a2} \): \[ K_{a2} = 2 \times 10^{-4} \times 4 \] \[ K_{a2} = 8 \times 10^{-4} \] ### Conclusion Thus, the value of \( K_{a2} \) is: \[ K_{a2} = 8 \times 10^{-4} \]

To solve the problem, we will use the provided relationships and the given information step by step. ### Step 1: Understand the given information We know that: - The degree of dissociation (α) of a weak electrolyte is inversely proportional to the square root of its concentration (c). - The relationship is given by Ostwald's dilution law: \[ \alpha = \sqrt{\frac{K_a}{c}} ...
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