CHAPTER 21- FURTHER ASPECTS OF EQUILIBRIA 🤎 Flashcards
Define a conjugate acid and conjugate base for two marks each
❤️
What is an equilibrium reaction? (AS level recap)
❤️
Along with the definition of a conjugate acid and conjugate base, use an equation for the reaction between ammonia and water to explain which is the conjugate acid and which is the conjugate base
❤️
Use an equation for the reaction between hydrochloric acid and water to explain the concept of conjugate base pairs
❤️
Define pH, write it’s formula and the formula for finding the concentration of hydrogen ions
-Calculate the value of pH and [H+] using the examples in your notes
❤️
Explain how to calculate the pH values of strong acids using an example in your notes
-which assumption is made when calculating the ph of strong acids?
❤️
Explain how to calculate the pH values of strong bases using an example in your notes (include the definition + equilibrium expression for Kw as well as the equation for the calculation of [H+] from Kw)
-which assumption is made when calculating the ph of strong bases?
❤️
What is pKa? what is the formula for pKa? -Explain what high and low pKa values mean
❤️
Explain how to calculate the pH of a weak acid by finding Ka using examples in your notes (include the definition + equilibrium expression for Ka as well as the equation for the calculation of [H+] from Ka)
-Explain what high and low Ka values mean
❤️
Define a buffer solution, state three ways a buffer solution can be made
❤️
Explain how a buffer solution can be made by mixing a weak acid with one of it’s salts in detail, using an example
❤️
Using an equation, explain how buffer solutions control pH IN DETAIL
❤️
State three uses of buffer solutions
❤️
Use an equation to explain the use of hydrogen carbonate ions as buffer solutions in our blood IN DETAIL
❤️
Use a formula to explain how we calculate the pH of a buffer solution when it’s made from a weak acid and it’s salt, practice this using an example in your notes (include the formula relating [H+] and Ka)
❤️
Use a formula to explain how we calculate the pH of a buffer solution when it’s made from a weak acid and a strong base, practice this using an example in your notes (include the formula relating [H+] and Ka)
❤️
Define solubility product (Ksp) and write it’s formula
❤️
Define solubility
-Explain the concept of equilibrium in the case of an ionic solid coming into contact with a saturated salt solution (use a formula + an expression for Kc in your explanation)
❤️
Write an expression for the solubility product of Fe2S3 and work out it’s units
❤️
Calculate Ksp from concentration and concentration from Ksp using examples in your notes
❤️
Explain how Ksp can be used to predict if a precipitate will be formed using an example in your notes
❤️
Further practice: perform more calculations involving Ksp using practice questions in your notes
❤️
Define the common ion effect
-With an example in your notes, use equilibrium to explain why a precipitate forms when a solution is added to a saturated solution (common ion effect)
❤️
Explain how the solubility of a compound varies when added to a solution containing a common ion using an example in your notes
❤️
Define partition co-efficient (Kpc)
❤️
Calculate and explain the calculation of Kpc using an example in your notes
❤️
Explain some factors affecting the value of Kpc and solubility, use two examples to explain these factors in detail (ammonia and iodine)
❤️
Give the general equilibrium expression for a solute partitioned between two solvents, state the conditions that need to be met when using this equation
❤️
