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A buffer solution is prepared by adding 10.0 g of ammonium chloride (NH₄Cl) to 250 mL of 1.00 M NH₃ solution. What is the pH of the resulting buffer solution?
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18. Aqueous Equilibrium
Intro to Acid-Base Titration Curves
Scelta multipla
In a titration of a weak acid with a strong base, what is the pH at the equivalence point?
A
pH > 7
B
pH = 7
C
pH = 0
D
pH < 7
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Understand that at the equivalence point in a titration of a weak acid with a strong base, the moles of acid initially present are equal to the moles of base added.
Recognize that at the equivalence point, the weak acid has been completely neutralized, forming its conjugate base.
Recall that the conjugate base of a weak acid is typically a weak base, which can affect the pH of the solution.
Consider the hydrolysis of the conjugate base in water, which will produce OH⁻ ions, leading to a basic solution.
Conclude that due to the presence of the conjugate base, the pH at the equivalence point will be greater than 7, indicating a basic solution.
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