Three solutions of strong electrolytes, 25 ml of 0.1 M-HX, 25 ml of 0.1 M-H2 Y and 50 ml of 0.1

step 1 So in this question, an equivalent of h positive is equal to 25 into 0 .1 by 1000 ,000 into 1 pl

Three solutions of strong electrolytes, 25 ml of 0.1 M-HX,...

Three solutions of strong electrolytes, $25 \mathrm{ml}$ of $0.1 \mathrm{M}-\mathrm{HX}, 25 \mathrm{ml}$ of $0.1 \mathrm{M}-\mathrm{H}_{2} \mathrm{Y}$ and $50 \mathrm{ml}$ of $0.1 \mathrm{~N}-\mathrm{Z}(\mathrm{OH})_{2}$ are mixed. pOH of the resulting solution is (a) $1.6$ (b) $7.0$ (c) $12.4$ (d) $11.6$

Three solutions of strong electrolytes, $25 \mathrm{ml}$ of $0.1 \mathrm{M}-\mathrm{HX}, 25 \mathrm{ml}$ of $0.1 \mathrm{M}-\mathrm{H}_{2} \mathrm{Y}$
and $50 \mathrm{ml}$ of $0.1 \mathrm{~N}-\mathrm{Z}(\mathrm{OH})_{2}$ are mixed.
pOH of the resulting solution is
(a) $1.6$
(b) $7.0$
(c) $12.4$
(d) $11.6$

Key Concepts

Strong Electrolytes

Strong electrolytes are substances that completely dissociate into their ions when dissolved in water. This full dissociation is essential in acid?base reactions because the ions are free to interact, resulting in complete neutralization where appropriate. It forms the basis for calculating the mole concentrations of the reactive ions in solution.

Acid-Base Neutralization

Acid-base neutralization involves the chemical reaction between an acid and a base producing water and a salt. In such reactions, the moles of hydrogen ions (H?) from the acid react with the moles of hydroxide ions (OH?) from the base. The concept is crucial for identifying whether the resulting solution is acidic or basic based on the amounts of each reactive ion after the reaction.

Stoichiometry in Acid-Base Reactions

Stoichiometry involves calculating the moles of each reactant to determine the extent of the reaction. It helps in assessing which ion is in excess after the acid and base have reacted. This quantification is necessary for establishing the concentration of any remaining excess ions, which then feeds into pH or pOH calculations.

pOH and pH Calculations

pOH is defined as the negative logarithm of the hydroxide ion concentration and is directly related to pH through the relation pH + pOH = 14 at 25°C. Calculating pOH from the concentration of excess OH? ions enables prediction of the basicity of the solution. This concept integrates the understanding of logarithms with molarity, linking stoichiometric data to the acid-base characteristics of the solution.

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