Please also explain how you calculate the initial moles, because I do not get the correct number.Calculate the $\mathrm{pH}$ of the resulting solution at 25 degrees $\mathrm{C}$, when $50,1 \mathrm{ml}$ of $0,100 \mathrm{~mol} / \mathrm{lsodium}$ hydroxide solution $\mathrm{NaOH}$ has been added to $50,0 \mathrm{ml}$ of;
a) $0,100 \mathrm{~mol} / \mathrm{l}$ hydrochloric acid $\mathrm{HCl}$ solution.
b) $0,100 \mathrm{~mol} / \mathrm{l}$ ethanoic acid $\mathrm{CH} 3 \mathrm{COOH}$ solution. pKa of ethanoic acid $=4,76$.

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***A*** ∻Key Concept∻ ⚹Neutralization Reaction⚹ ∻Explanation∻ ⚹When NaOH is added to HCl, a strong acid and a strong base neutralize each other to form water and salt (NaCl). The resulting solution is neutral with a pH of 7.⚹ ***B*** ∻Key Concept∻ ⚹Buffer Solution and Henderson-Hasselbalch Equation⚹ ∻Explanation∻ ⚹When NaOH is added to ethanoic acid, a weak acid, it partially neutralizes the acid, forming its conjugate base (acetate ion). The pH of the resulting buffer solution can be calculated using the Henderson-Hasselbalch equation: $ ext{pH} = ext{pKa} + \log \left( \frac{[ ext{A}^-]}{[ ext{HA}]} ight) $.⚹◊How can you calculate the initial moles of different reactants in the given chemical reactions⍭ Generate me a similar question◊

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