18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

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Suppose 40.0 mL of an acetic acid solution of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution?
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What is the initial concentration of formic acid (HCOOH) in the solution before titration?
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20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.
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Calculate the pH of the solution resulting from the mixing of 55.0 mL of 0.100 M NaCN and 75.0 mL of 0.100 M HCN with 0.0090 moles of NaOH.
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In order to create a buffer, 7.510 g of sodium cyanide is mixed with 100.0 mL of 0.250 M hydrocyanic acid, HCN. What is the pH of the buffer solution after the addition of 12.0 mL of 0.300 M NaH? K_a = 4.9 × 10⁻¹⁰.
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Calculate the pH at the equivalence point for the titration of 20.0 mL of 0.500 M HC₂H₃O₂ with 0.350 M KOH. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.
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A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10⁻⁵) was titrated with 0.50 M NaOH. Calculate the pH after the addition of 30.0 mL of NaOH at 25 °C.
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A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 23.0 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴
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Consider the titration of a 24.0 mL sample of 0.110 mol/L CH3COOH (Ka=1.8×10⁻⁵) with 0.125 mol/L NaOH. What volume of NaOH is required to reach the equivalence point?
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A 35.0-mL sample of 0.150 M acetic acid (CH3COOH, Ka=1.8×10⁻⁵) is titrated with 0.150 M NaOH solution. Calculate the pH after 35.0 mL of the base have been added.
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A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10^-4.
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Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 × 10^-5) with 0.200 M NaOH. What is the pH of the solution after the addition of 15.00 mL of NaOH solution?
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20.0 mL of 0.500 M HC2H3O2 is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. Ka for HC2H3O2 = 1.8 × 10⁻⁵.
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In a titration of a weak acid with a strong base, how is the pH determined before reaching the equivalence point?
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What is the pH at the equivalence point for a titration involving 25 mL of 0.1 M acetic acid and 0.2 M KOH, given that the acid dissociation constant (Ka) for acetic acid is 1.8 × 10^-5?
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