What is the pH of 4 ×10^-3 M-Y(OH)2 solution assuming the first dissociation to be 100 % and sec

step 1 Hello everyone, so in this question we have to calculate the pH of 4 into 10 district power minu

What is the pH of 4 ×10^-3 M-Y(OH)2 solution assuming the...

What is the $\mathrm{pH}$ of $4 \times 10^{-3} \mathrm{M}-\mathrm{Y}(\mathrm{OH})_{2}$ solution assuming the first dissociation to be $100 \%$ and second dissociation to be $50 \%$, where $Y$ represents a metal cation? $(\log 2=0.3, \log 3=0.48)$ (a) $11.78$ (b) $11.22$ (c) $2.22$ (d) $2.78$

What is the $\mathrm{pH}$ of $4 \times 10^{-3} \mathrm{M}-\mathrm{Y}(\mathrm{OH})_{2}$
solution assuming the first dissociation to be $100 \%$ and second dissociation to be $50 \%$, where $Y$ represents a metal cation? $(\log 2=0.3, \log 3=0.48)$
(a) $11.78$
(b) $11.22$
(c) $2.22$
(d) $2.78$

Key Concepts

pH and pOH Relationship

The pH is a measure of acidity and is calculated based on the concentration of hydrogen ions (H+), while pOH is based on hydroxide ions (OH-). They are related by the equation pH + pOH = 14 (at 25°C). Understanding this relationship allows one to calculate the pH of a solution when the concentration of OH- is known.

Polyprotic Bases

A polyprotic base is one that can release more than one proton (or, equivalently, form more than one hydroxide ion) in a stepwise manner when dissolved in water. The dissociation can occur in multiple stages, each with its own extent of reaction, which affects the overall concentration of hydroxide ions in the solution.

Stepwise Dissociation and Degree of Ionization

In stepwise dissociation, different hydroxide groups may be lost from the base sequentially, and each step can have a different degree of ionization or percent dissociation. Evaluating each stage individually is crucial for calculating the total concentration of hydroxide ions contributed by all dissociation steps.

Logarithmic Calculations

Logarithmic calculations are essential in pH and pOH determinations because concentrations are often expressed on a logarithmic scale. Using properties of logarithms, such as converting multiplication into addition, simplifies the process of computing the negative logarithm of ion concentrations to find pH values.

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