- Messages
- 4
- Reaction score
- 2
- Points
- 3
For why to use digital probe thermometer instead of lab thermometer, I wrote because it has less % error since lab thermometer is 1 dp and digital is 2 dp.
For why the B.P is not 100C but 99.48C, I wrote heat is lost to surroundings.
For the 2nd Q, 1st part, I wrote the more no. Of moles means Delta Twill increase. Since DeltaT is difference between temp of water, which is constant, and temp of solution, the temp of solution increases. So temperature increases as pressure decreases.
For 1st question 1 st part, I wrote Precaution as wear gloves.
For 2nd part, no change at positive electrode and red at negative.
The salt I chose in the experiment 1 and experiment 2 question (Last question of that page I guess, 2 marks) was KCl.
Mass of K2SO4 was around 1.743 g???
Volume needed to dilute was 5 cm3???
For the preparation of solution from mass Of K2SO4, I wrote: Add 1.743 g of K2SO4 To a beaker. Add 50cm3 of water using a burette. Transfer the contents to a volumetric flask. Rinse the beaker. Stopper the flask and shake thoroughly. Add 50 cm3 of water again using a burette to the volumetric flask. Stopper the flask and shake thouroughly.
For the apparatus needed to measure that 5cm3 , I wrote a graduated pipette.
For the question on Expermient1 and experiment 2, which was what happens when you increase the charge from -1 to -2 to -3, I wrote: As the charge becomes more negative, the amount of salt needed to precipitate 1dm3 sol decreases. This is because the concentration of ions increases.
For why the B.P is not 100C but 99.48C, I wrote heat is lost to surroundings.
For the 2nd Q, 1st part, I wrote the more no. Of moles means Delta Twill increase. Since DeltaT is difference between temp of water, which is constant, and temp of solution, the temp of solution increases. So temperature increases as pressure decreases.
For 1st question 1 st part, I wrote Precaution as wear gloves.
For 2nd part, no change at positive electrode and red at negative.
The salt I chose in the experiment 1 and experiment 2 question (Last question of that page I guess, 2 marks) was KCl.
Mass of K2SO4 was around 1.743 g???
Volume needed to dilute was 5 cm3???
For the preparation of solution from mass Of K2SO4, I wrote: Add 1.743 g of K2SO4 To a beaker. Add 50cm3 of water using a burette. Transfer the contents to a volumetric flask. Rinse the beaker. Stopper the flask and shake thoroughly. Add 50 cm3 of water again using a burette to the volumetric flask. Stopper the flask and shake thouroughly.
For the apparatus needed to measure that 5cm3 , I wrote a graduated pipette.
For the question on Expermient1 and experiment 2, which was what happens when you increase the charge from -1 to -2 to -3, I wrote: As the charge becomes more negative, the amount of salt needed to precipitate 1dm3 sol decreases. This is because the concentration of ions increases.
