At 90^∘ C, the hydronium ion concentration in pure water is 10^-6 M. If 100 ml of 0.5 M-NaOH sol

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At 90^∘ C, the hydronium ion concentration in pure water is...

At $90^{\circ} \mathrm{C}$, the hydronium ion concentration in pure water is $10^{-6} \mathrm{M}$. If $100 \mathrm{ml}$ of $0.5 \mathrm{M}-\mathrm{NaOH}$ solution is mixed with $250 \mathrm{ml}$ of $0.2 \mathrm{M}-\mathrm{HNO}_{3}$ solution at $90^{\circ} \mathrm{C}$, $\mathrm{pH}$ of the resulting solution will be (a) $7.0$ (b) $6.0$ (c) $8.0$ (d) $0.85$

At $90^{\circ} \mathrm{C}$, the hydronium ion concentration in pure water is $10^{-6} \mathrm{M}$. If $100 \mathrm{ml}$ of $0.5 \mathrm{M}-\mathrm{NaOH}$ solution is mixed with $250 \mathrm{ml}$ of $0.2 \mathrm{M}-\mathrm{HNO}_{3}$ solution at $90^{\circ} \mathrm{C}$,
$\mathrm{pH}$ of the resulting solution will be
(a) $7.0$
(b) $6.0$
(c) $8.0$
(d) $0.85$

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Key Concepts

Stoichiometry in Acid-Base Reactions

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. In acid-base reactions, understanding the molar amounts and concentrations of the reacting species allows one to determine if there is an excess of acid or base, which directly influences the pH of the resulting solution.

Ionic Product of Water (Kw)

The ionic product of water, Kw, is a measure of the concentrations of hydronium and hydroxide ions in water. It is temperature-dependent, meaning that as the temperature increases, Kw increases, which can shift the neutral pH value from the standard 7.0 observed at room temperature.

Neutralization Reaction

This concept involves the reaction between an acid and a base, resulting in the formation of water and a salt. The stoichiometry of the reaction determines the extent to which the acid or base is neutralized, affecting the final concentrations of hydronium and hydroxide ions in the solution.

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