Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (a) The pH at the beginning of the two titrations will be the same.

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Identify the type of titrations being compared in Problem 17.35. Common types include strong acid-strong base, weak acid-strong base, strong acid-weak base, and weak acid-weak base titrations.

Understand that the pH at the beginning of a titration is determined by the nature of the solution being titrated. For example, if a strong acid is being titrated, the initial pH will be low, while a weak acid will have a higher initial pH.

Consider the initial concentrations and the dissociation constants (Ka for acids, Kb for bases) of the substances involved in the titrations. These factors influence the initial pH.

If the two titrations involve different types of acids or bases (e.g., one is a strong acid and the other is a weak acid), the initial pH values will differ due to the differences in ionization.

Conclude whether the initial pH values are the same or different based on the analysis of the types of acids or bases involved in the titrations and their respective dissociation properties.

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Key Concepts

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

Titration Basics

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant to a solution of analyte until the reaction reaches its endpoint, which is often indicated by a color change. Understanding the initial conditions of the titration, including the pH of the solutions involved, is crucial for interpreting the results.

pH and Acid-Base Chemistry

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. In titrations involving strong acids and bases, the initial pH can vary significantly depending on the nature of the acid or base being titrated. Recognizing how the pH changes throughout the titration process is essential for predicting the behavior of the solution at different stages.

Equivalence Point

The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance in the analyte solution. At this point, the reaction between the acid and base is complete, and the pH can change dramatically. Understanding the equivalence point helps in determining whether the initial pH of two different titrations will be the same or different based on the reactants used.

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01:07

At the Equivalence Point

Related Practice

Textbook Question

Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false. (a) More base is required to reach the equivalence point for the strong acid than the weak acid.

Textbook Question

The samples of nitric and acetic acids shown here are both titrated with a 0.100 M solution of NaOH(aq).

Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH1aq2 is needed to reach the equivalence point in the titration of HNO3.

Textbook Question

Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (b) The titration curves will both be essentially the same after passing the equivalence point.

Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) NaHCO₃ titrated with NaOH (c) KOH titrated with HBr.

Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) NH₃ titrated with HCl.