What is the pH of a solution obtained by reacting $ 2.0 \; mol\; HCl $ with $ 1.0 \; mol \; NaOH $ in a volume of $ 1 \; L $? What is at the end of the reaction? What are the ions then present?

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At the end of the reaction, The product of the reaction: $1.0; mole\; NaCl $ The rest: $ 1.0 \; mole\; HCl $ Ions: $Na^+$ $Cl^-$ $H^+$

Characterize these ions from the acid-base point of view !

$Na^+$ : no influence $Cl^-$ : no influence $H^+$ : strong acid

Quel est le pH de cette solution?

$[H^+]=1.0\; \frac{mol}{L}$ $pH$ $=$ $-log1.0$ $=$ $0.0$