A 5.5 L sample of a 0.25 M HNO₃ solution is mixed with 1.2 L of a 0.34 M HCl solution. What is the pH of the mixture A) 0.23 B) 0.57 C) 1.07 D) 0.50 E) 0.84

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Quizplus · Accepted Answer

The pH of the mixture can be calculated by first determining the total moles of H+ ions contributed by each solution, then finding the concentration of H+ in the final mixture, and finally calculating the pH. For HNOS (assuming it's a strong acid for this calculation):- Moles of H+ from HNOS = 0.25 M * 5.5 L = 1.375 molesFor HCl (also a strong acid):- Moles of H+ from HCl = 0.34 M * 1.2 L = 0.408 molesTotal moles of H+ = 1.375 + 0.408 = 1.783 molesTotal volume of the mixture = 5.5 L + 1.2 L = 6.7 LConcentration of H+ in the mixture = 1.783 moles / 6.7 L = 0.266 MpH = -log(0.266) ≈ 0.57

A 55 L Sample of a 0