Textbook Question
Determine the pH for the following solutions:
c. [H3O+] = 0.0001 M
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10. Acids and Bases
The pH Scale
Multiple Choice
A 345 mL bottle of antacid (Mg(OH)2) contains 1.45 × 10−2 moles of hydroxide ions. Determine pH and pOH of the antacid.
A
pH = 12.384
pOH = 1.616
B
pH = 12.623
pOH = 1.377
C
pH = 12.161
pOH = 1.839
D
pH = 12.338
pOH = 1.662
Verified step by step guidance1
Identify the given information: volume of the antacid solution is 345 mL (which should be converted to liters) and the amount of hydroxide ions (OH⁻) is 1.45 × 10⁻² moles.
Convert the volume from milliliters to liters by dividing by 1000: \(V = \frac{345}{1000} = 0.345\) L.
Calculate the hydroxide ion concentration \([OH^-]\) using the formula \([OH^-] = \frac{\text{moles of } OH^-}{\text{volume in liters}} = \frac{1.45 \times 10^{-2}}{0.345}\).
Determine the pOH using the formula \(pOH = -\log [OH^-]\) where \([OH^-]\) is the hydroxide ion concentration calculated in the previous step.
Calculate the pH using the relationship between pH and pOH: \(pH = 14 - pOH\).
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