Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity. b. the volume of added acid required to reach the equivalence point

Verified step by step guidance

Identify the balanced chemical equation for the reaction: \( \text{RbOH} + \text{HCl} \rightarrow \text{RbCl} + \text{H}_2\text{O} \).

Determine the moles of \( \text{RbOH} \) in the initial solution using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).

Since the reaction is a 1:1 molar ratio, the moles of \( \text{HCl} \) required to reach the equivalence point will be equal to the moles of \( \text{RbOH} \).

Calculate the volume of \( \text{HCl} \) needed using the formula: \( \text{volume} = \frac{\text{moles of HCl}}{\text{concentration of HCl}} \).

Convert the volume from liters to milliliters if necessary, as the final answer should be in milliliters.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

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

Titration

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 (a solution of known concentration) to a sample until a reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. This method is commonly used in acid-base reactions to find the concentration of an unknown acid or base.

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 present in the sample. For acid-base titrations, this means that the moles of acid equal the moles of base. It is often indicated by a color change in an indicator or by using a pH meter, marking the completion of the reaction.

Molarity and Volume Relationship

Molarity (M) is defined as the number of moles of solute per liter of solution. In titration calculations, the relationship between the molarity and volume of the reactants is crucial. The formula M1V1 = M2V2 can be used, where M1 and V1 are the molarity and volume of the titrant, and M2 and V2 are those of the analyte. This relationship allows for the calculation of the volume of titrant needed to reach the equivalence point.

Recommended video:

Guided course

01:21

Standard Molar Volume

Related Practice

Textbook Question

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. e. the pH after adding 5.0 mL of base beyond the equivalence point

Textbook Question

Consider the titration of a 20.0-mL sample of 0.105 M HC₂H₃O₂ with 0.125 M NaOH. Determine each quantity. b. the volume of added base required to reach the equivalence point

Textbook Question

Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity. c. the pH at 5.0 mL of added acid

Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 0 mL, 5 mL, 10 mL, equivalence point, one-half equivalence point, 20 mL, 25 mL. Sketch the titration curve.

Textbook Question

A 20.0-mL sample of 0.125 M HNO₃ is titrated with 0.150 M NaOH. Calculate the pH for at least five different points throughout the titration curve and sketch the curve. Indicate the volume at the equivalence point on your graph.