Multiple Choice
A 25.00 mL sample of 0.175 M HCl is being titrated with 0.250 M NaOH. What is the pH when 0 mL of NaOH has been added?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
An aqueous solution has a pH of 3.0. Calculate the pOH. Be sure your answer has the correct number of significant digits.
A
10.0
B
9.0
C
11.0
D
8.0
Verified step by step guidance1
Understand the relationship between pH and pOH: The sum of pH and pOH in any aqueous solution at 25°C is always 14. This is derived from the ion product of water (Kw = 1.0 x 10^-14), where pH + pOH = 14.
Identify the given value: The problem states that the pH of the solution is 3.0.
Set up the equation to find pOH: Use the relationship pH + pOH = 14. Substitute the given pH value into the equation: 3.0 + pOH = 14.
Solve for pOH: Rearrange the equation to isolate pOH on one side. This gives pOH = 14 - 3.0.
Determine the number of significant figures: The pH value given is 3.0, which has two significant figures. Therefore, the calculated pOH should also be reported with two significant figures.
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