Which of the following solutions will have pH | vedclass

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(D) For $pH = 1.0$,the concentration of $[H^{+}]$ must be $10^{-1} \ M = 0.1 \ M$.Option $(d)$: $M.eq. \ of \ HCl = 75 \ mL 	imes \frac{1}{5} \ M = 1

Vedclass · Accepted Answer

$75 \ mL$ of $\frac{M}{5} \ HCl + 25 \ mL$ of $\frac{M}{5} \ NaOH$

Vedclass · Answer

(D) For $pH = 1.0$,the concentration of $[H^{+}]$ must be $10^{-1} \ M = 0.1 \ M$.Option $(d)$: $M.eq. \ of \ HCl = 75 \ mL 	imes \frac{1}{5} \ M = 15 \ mmol$.$M.eq. \ of \ NaOH = 25 \ mL 	imes \frac{1}{5} \ M = 5 \ mmol$.Remaining $H^{+}$ ions $= 15 - 5 = 10 \ mmol$.Total volume $= 75 + 25 = 100 \ mL$.$[H^{+}] = \frac{10 \ mmol}{100 \ mL} = 0.1 \ M = 10^{-1} \ M$.Therefore,$pH = -\log(10^{-1}) = 1.0$.

Which of the following solutions will have $pH$ close to $1.0$?

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