An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would (Given log ⁡2=0.30 )

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Correct answer: A. (a) An aqueous solution of HCl initially has a pH of 1.0, meaning the hydrogen ion concentration is (H^+ )=10^-1M. When we dilute the solution by adding an equal volume of water, the concentration of hydrogen ions will be halved: (H^+ )_ new= 10^-12=5 10^-2M To find the new pH , we use the pH formula: pH=- log (H^+ ) Substituting the new hydrogen ion concentration gives: pH=- log(5 10^-2) Using the logarithm property log ⁡ (a b )= log ⁡a+ log ⁡b : pH=-( log ⁡5+ log ⁡10^-2)=- log ⁡5+2 Given log2=0.30, we need log5, which can be calculated as: log10= log(2 5)= log2+ log5 ⇒ log5= log10- log 2 = 1 – 0.30 = 0.70 Thus: pH=- (0.70 )+2=1.3 Therefore, the pH of the solution increases to 1.3.

$An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would (Given log 2 = 0.30)$

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