Following five solutions of KOH were prepared as: first, 0.1 mole in 1 L ; second. 0.2 mole in

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Following five solutions of KOH were prepared as: first, 0.1...

Following five solutions of $\mathrm{KOH}$ were prepared as: first, $0.1$ mole in $1 \mathrm{~L} ;$ second. $0.2$ mole in $2 \mathrm{~L}$; third, $0.3$ mole in $3 \mathrm{~L}$; fourth, $0.4$ mole in $4 \mathrm{~L} ;$ fifth, $0.5$ mole in $5 \mathrm{~L}$. The $\mathrm{pH}$ of resultant solution, when all these solutions are mixed, is (a) 2 (b) 1 (c) 13 (d) 7

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Key Concepts

pH and pOH Relationship

The pH of a solution is intrinsically related to its pOH by the equation pH + pOH = 14 at 25°C. For solutions containing strong bases, once the hydroxide ion concentration is calculated, pOH is obtained using the logarithmic relationship, and the pH is determined by subtracting pOH from 14.

Dilution Principle

The dilution principle involves combining solutions where the total amount of solute remains constant while the volume changes. The resultant concentration is obtained by dividing the combined moles of solute by the sum of the volumes, which is essential when dealing with mixture problems.

Strong Base Dissociation

KOH is a strong base that dissociates completely in aqueous solution, meaning that every mole of KOH produces one mole of hydroxide ions. This property simplifies the calculation as the concentration of KOH directly determines the hydroxide ion concentration without needing to consider equilibrium constants.

Molarity Calculation

Molarity is defined as the number of moles of solute per liter of solution. When different solutions are mixed, their total moles of solute and total volume are summed up to find the overall concentration. This approach is fundamental to any calculation involving the concentration of a solution after mixing.

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