A 11.3-mL sample of an HCl solution has a pH of 2.085. What volume of water...

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Question

A 11.3-mL sample of an HCl solution has a pH of 2.085. What volume of water must be added to change the pH to 4.170? (in mL)

science chemistry

Answer 1

Answer #1

pH = 2.085 ,. [H⁺]₁= 10^-pH = 10^-2.085 = 8.222×10^-3M

pH = 4.170, . [H⁺]₂ = 10^-4.170 = 6.76×10^-5M

Since addition of water doesn't change the moles of H⁺ ions in the solution. We can apply M₁V₁= M₂V₂

8.222×10^-3M × 11.3ml = 6.76×10^-5 M × V₂

V₂ (ml) = 8.222×10^-3 ×11.3/(6.76×10^-5) = 13.7439×10²ml = 1374.39ml

Volume of water added to change the desired pH = 1374.39ml - 11.3ml = 1363.09ml = 1363.1ml (answer)

Answer 2

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