Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
17 Cards in this Set
- Front
- Back
|
What are the two redox titrations? |
•manganate under acidic conditions •iodine with thiosulphate |
|
|
Describe the method of the manganate/hcl titration? |
1) add standard solution of mno4 to burette 2) add known volume of solution being analysed to conical flask with some h2so4 so that the h ions can reduce mno4 3) end point is a permanent pink colour |
|
|
Describe the method of the iodine thiosulfate test |
1) add standard solution of thisulfate to burette 2) add known volume of iodine to conical flask 3) brown colour should start fading to pale straw colour. Add starch which turns solution to black. Eventually it turns clear which means all iodine has been used up |
|
|
What is a half cell? |
Contains chemical species present in redox reactions |
|
|
What is a half cell? |
Contains chemical species present in redox reactions |
|
|
How is a voltaic cell made? |
By connecting two different half cells which allows electrons to flow therefore chemical energy can be converted into electrical energy |
|
|
What is a half cell? |
Contains chemical species present in redox reactions |
|
|
How is a voltaic cell made? |
By connecting two different half cells which allows electrons to flow therefore chemical energy can be converted into electrical energy |
|
|
Why must half cells be kept separate and not mixed together? |
Would cause an uncontrollable flow of electrons and energy would be lost as heat energy |
|
|
Describe metal/metal ion half cell |
•metal rod dipped into solution if it’s metal ions •the phase boundary (where rod meets the solution) sets up an equilibrium •when the two half cells are connected the direction of electron flow depend on the tendency to release electrons of each electrode |
|
|
Describe ion/ion half cell |
•half cells consists of ions from same element but with different oxidation state •inert metal electrode made out of platinum is used |
|
|
Describe ion/ion half cell |
•half cells consists of ions from same element but with different oxidation state •inert metal electrode made out of platinum is used |
|
|
How can we know which electrode is positive or negative? |
The most reactive metal will be the most negative electrode as it will be oxidising. The least reactive metal will be the positive electrode as it will be reducing |
|
|
What is standard electrode potential? |
Measure of tendency for an electrode to gain electrons and be reduced |
|
|
What is the standard half cell used? |
Half cell containing hydrogen gas and solution containing hydrogen ions Inert platinum electrode is used Standard conditions Exactly 0V |
|
|
What is the standard half cell used? |
Half cell containing hydrogen gas and solution containing hydrogen ions Inert platinum electrode is used Standard conditions Exactly 0V |
|
|
Equation to calculate standard electrode potential |
E positive - E negative |
