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The pH of 0.004 M hydrazine solution is 9.7. Its ionization constant (Kb) is?
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The pH of 0.004 M hydrazine solution is 9.7. Its ionization constant (...
Use the formula of POH of weak Base.... then u get Pkb and by taking antilog kb can be find...
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The pH of 0.004 M hydrazine solution is 9.7. Its ionization constant (...


Introduction:


Hydrazine (N2H4) is a weak base that can ionize in water to form the hydrazine ion (N2H5+) and hydroxide ion (OH-). The ionization constant of hydrazine, also known as Kb, is a measure of the extent to which it ionizes in water.


Given:


Concentration of hydrazine solution (N2H4) = 0.004 M

pH of the solution = 9.7


Calculating the pOH:


pOH is the negative logarithm of the hydroxide ion concentration. It can be calculated using the formula:

pOH = 14 - pH


In this case, the pH is 9.7, so the pOH is:

pOH = 14 - 9.7 = 4.3


Calculating the hydroxide ion concentration (OH-):


The hydroxide ion concentration can be determined using the pOH value and the formula:

[OH-] = 10^(-pOH)


In this case, the pOH is 4.3, so the hydroxide ion concentration is:

[OH-] = 10^(-4.3)


Calculating the hydrazine ion concentration (N2H5+):


Since hydrazine (N2H4) ionizes to form the hydrazine ion (N2H5+), the concentration of the hydrazine ion can be assumed to be equal to the hydroxide ion concentration:

[N2H5+] = [OH-] = 10^(-4.3)


Calculating the concentration of hydrazine (N2H4):


To calculate the concentration of hydrazine (N2H4), we can use the equation for Kb:

Kb = [N2H5+][OH-] / [N2H4]


Substituting the known values:

Kb = (10^(-4.3) * 10^(-4.3)) / 0.004


Simplifying the expression:

Kb = 10^(-8.6) / 0.004


Calculating the value of Kb:

Kb = 2.5 x 10^(-7)


Conclusion:


The ionization constant (Kb) of the 0.004 M hydrazine solution is 2.5 x 10^(-7).
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The pH of 0.004 M hydrazine solution is 9.7. Its ionization constant (Kb) is?
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