Consider the titration of 25.0 mL of 0.200 M HCO2H with 0.250 M NaOH. How many milliliters of base are required to reach the equivalence point? Calculate the pH at each of the following points: (c) At the equivalence point, (d) After the addition of 25.0 mL of base.

Verified step by step guidance

Step 1: Determine the moles of formic acid (HCO2H) present initially by using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).

Step 2: Calculate the volume of NaOH required to reach the equivalence point by using the stoichiometry of the reaction, which is 1:1 for HCO2H and NaOH. Use the formula: \( \text{volume of NaOH} = \frac{\text{moles of HCO2H}}{\text{concentration of NaOH}} \).

Step 3: At the equivalence point, the solution contains the conjugate base (HCO2^-) of formic acid. Calculate the concentration of this conjugate base using the total volume of the solution at the equivalence point.

Step 4: Use the hydrolysis of the conjugate base to find the pH at the equivalence point. Set up the equilibrium expression for the reaction of HCO2^- with water and use the \( K_b \) value, which can be derived from \( K_w / K_a \) of formic acid.

Step 5: For the pH after the addition of 25.0 mL of base, calculate the moles of NaOH added and determine the excess moles of NaOH. Use the concentration of excess OH^- to find the pH.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Titration and Equivalence Point

Titration is a quantitative analytical method used to determine the concentration of a solution by reacting it with a solution of known concentration. The equivalence point is reached when the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample. In this case, it occurs when all the formic acid (HCO2H) has reacted with the sodium hydroxide (NaOH).

Stoichiometry of Acid-Base Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. For the titration of HCO2H with NaOH, the balanced equation shows a 1:1 molar ratio, meaning one mole of formic acid reacts with one mole of sodium hydroxide. This relationship is crucial for determining the volume of NaOH needed to reach the equivalence point.

pH Calculation at the Equivalence Point

At the equivalence point of a titration involving a weak acid and a strong base, the resulting solution contains the conjugate base of the weak acid. The pH at this point can be calculated using the concentration of the conjugate base and its hydrolysis in water. This involves determining the Kb of the conjugate base and applying the formula for pH based on the concentration of hydroxide ions produced.

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pH at the Equivalence Point Example

Related Practice

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Consider the titration of 60.0 mL of 0.150 M HNO3 with 0.450 M NaOH.(a) How many millimoles of HNO3 are present at the start of the titration?(b) How many milliliters of NaOH are required to reach the equivalence point?(c) What is the pH at the equivalence point? (d) Sketch the general shape of the pH titration curve.

Textbook Question

Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points, and tell how many milliliters of acid are required to reach the equivalence point. (a) At the start of the titration(b) At the equivalence point (c) After the addition of a large excess of acid

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Textbook Question

On the same graph, sketch pH titration curves for the titra-tion of (1) a strong acid with a strong base and (2) a weak acid with a strong base. How do the two curves differ with respect to the following? (a) The initial pH

Textbook Question

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