The pH of 0.1 M-N2 H4 solution is (For N2 H4, Kbl=3.6 ×10^-6, Kb 2=6.4 ×10^-12 log2=0.3, log3=0.

step 1 Hello everyone so in this question we it is given this n2 h4 the concentration is 0 .55 one mala

The pH of 0.1 M-N2 H4 solution is (For N2 H4, Kbl=3.6...

The $\mathrm{pH}$ of $0.1 \mathrm{M}-\mathrm{N}_{2} \mathrm{H}_{4}$ solution is (For $\mathrm{N}_{2} \mathrm{H}_{4}, K_{\mathrm{bl}}=3.6 \times 10^{-6}, K_{\mathrm{b} 2}=6.4 \times 10^{-12}$
$\log 2=0.3, \log 3=0.48)$
(a) $3.22$
(b) $2.72$
(c) $10.78$
(d) $11.22$

Key Concepts

Acid–Base Equilibrium

This concept involves understanding the reaction between a weak base and water, in which the base partially accepts a proton from water to form its conjugate acid and hydroxide ions. The equilibrium constant (Kb) quantifies the extent of this reaction, and it is used to calculate the concentrations of all species at equilibrium, which ultimately allows for the determination of pH or pOH in the solution.

Weak Base Approximation

When dealing with weak bases, the degree of ionization is typically very small compared to the initial concentration. This approximation simplifies the mathematical treatment of the equilibrium, as the change in concentration (often denoted as x) can be considered negligible relative to the starting concentration, allowing a more straightforward calculation of hydroxide ion concentration.

pH and pOH Relationship

In aqueous solutions at 25°C, pH and pOH are related by the equation pH + pOH = 14. By first calculating the concentration of hydroxide ions formed from the weak base equilibrium, one can determine the pOH and then use this relationship to find the pH of the solution.

Stepwise Ionization in Polybasic Compounds

For compounds that can accept more than one proton, such as molecules with more than one basic site, ionization occurs in a stepwise manner. The first ionization typically has a much higher equilibrium constant than the second, meaning the initial protonation step dominates the behavior of the solution. Recognizing this allows one to focus on the primary equilibrium when calculating the pH.

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