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Chapter 14 Part II
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| Buffer capacity definition | The amount of acid or base that can be added to a buffer without causing a large change in the pH |
| What two things cause the buffer capacity to increase? | Absolute concentrations of the buffer components increase Relative concentrations of the buffer components become more similar |
| Buffers only work when? | Buffers only work if the added base or acid is small relative to the buffer concentration |
| Buffer range definition | The pH range over which a particular acid and its conjugate base can be effective |
| What is an effective buffer range? | pKa +- 1 |
| What does the base/acid ration need to be between to avoid breaking the buffer? | Under 10 and above 0.1 |
| How do you break the buffer? | The pH is not within 1 of the pKa |
| What does an effective buffer do? | Neutralizes small to moderate amounts of added acid or base without a large change in its pH |
| What are the two factors that make a buffer more effective? | The concentrations of acid and conjugate base are equal The concentrations of acid and conjugate base are high |
| What are titrations used for? | To determine the concentrations of an unknown solution |
| Standardize definition | To determine the concentration of a solution |
| Acid-base titration definition | A laboratory procedure where a basic (or acidic) solution of unknown concentration is reacted with an acidic (or basic) solution of known concentration |
| What is an acid-base titration used for? | To determine the concentration of the unknown acid or base |
| What is used to monitor the pH in the Erlenmeyer flask? | A pH meter or an indicator |
| Indicator definition | A dye whose color depends on the pH of the solution |
| In a strong acid-strong base reaction, the equivalence point is where there is... | Equal moles of the acid and base The [H3O+] or [OH-] is 1x10^-7 pH = 7 |
| Where is the end point observed in a strong acid-strong base reaction? | [H3O+] = [OH-] |
| Titration curve definition | A plot of the pH of the solution in Erlenmeyer flask (y-axis) vs. the volume of the solution added (x-axis) |
| What is another name for a titration curve? | pH curve |
| Equivalence point definition | The point in the titration when the moles of base is stoichiometrically equal to the moles of acid |
| Before the equivalence point the solution in the Erlenmeyer flask is in .... | Excess |
| Before the equivalence point the solution in the burette is in .... | Excess |
| In a strong acid-strong base reaction, the equivalence point has... | Equal moles of strong-acid and strong-base Leads to neutral salt solution A pH equal to 7 |
| In a weak acid-strong base reaction, the equivalence point has... | Equal moles of weak acid and strong base Leads to all weak acid converted tovconjugate base A pH above 7 (owing to the conjugate base) |
| For a diprotic acid with sufficiently different Ka1 and Ka2, how many equivalence points are there? What is the relationship between them | There are two equivalence points The total volume to reach the 2nd equivalence point will be twice the total volume required to reach the 1st equivalence point |
Created by:
KristenR2025