Introducing
Your new presentation assistant.
Refine, enhance, and tailor your content, source relevant images, and edit visuals quicker than ever before.
Trending searches
Introduction
- N&G profile
- Research the difference in calcium ions
- Tap- and mineral water
- determination of Calcium ions
- Does this have effect on us?
- Hard water has many health benefits
- Calcium and magnesium and important nutrients.
- Calcium ions -> build bones/teeth, keep them strong, etc.
- Hard water -> less incidences of heart disease, lower cholesterol.
- Hard water can dry out your hair
- Little scales will stand up
- Make your hair feel rough and damaged
- What does hard and soft water mean?
- Hard water -> Large amount of minerals
- Soft water -> small amount of minerals
- Rainwater is soft, but on the ground it will take up minerals from the soil.
- Calcium is a mineral that occurs in water naturally.
- It may be dissolved into the water from rocks such as limestone (kalk).
- Hardness in the water
- South-West the water is harder than North and Centre of Holland
- Soil and rocks contain more minerals
- Hardness of Warnsveld (11.10), Not too soft or too hard.
- Limescale (kalk) caused by Calcium carbonate
- Found in waterboilers or showerheads
Results
First experiment :
25ml tap water from Gorssel
Average = 23,6 mL EDTA used
Second experiment :
25ml mineral water Lidl ( Saskia )
Average = 2,7 mL EDTA used
Third experiment :
25ml AH mineral water
Average = 7,7 mL EDTA used
Fourth experiment :
25ml tap water from Warnsveld
Average = 14,5 mL EDTA used
Processing of the results
9,07 • 10^ -3 mg CaCO3 / L
2,84 • 10^ -3 mg CaCO3 / L
6,2 • 10^ -3 mg CaCO3 / L
8,4 • 10^ -4 mg CaCO3 / L
- the formula we used to calculate the amount of calcium :
( • = multiply )
( x = the amount )
1:1 mole ratio with EDTA , CA 2+ and CaCO3
x mL EDTA • 0,100 mole EDTA/ 100mL • 1 mole CaCO3/ 1 mole EDTA • 100g CaCO3/ 1 mole CaCO3 • 1000mg/1g = x mg CaCO3
x mg CaCO3/y mL water • 1000ml/1L = your mg CaCO3/L
- Tap water consists of more calcium ions
- color change is slower
- Takes longer to take up calcium ions up if there is more calcium
- Both healthy for us
- Tap water a lot more EDTA
- precise calculations
Cleaned with machines
Directly bottled up
- 3 trails
- 25mL water into an Erlenmeyer
- 7 drops of indicator
- 10mL of Ammonia buffer
- Titration with EDTA
- changes color quickly -> less calcium ions
Experiment
- Titration method
- EDTA, a molecule that wraps around calcium ions
- Ammonia buffer solution, removes H ions
- Colorless in water
- Indicator, change color when all the calcium ions are taken up by EDTA
- Color change from red/pink -> royal blue end point
indicator
EDTA molecule
EDTA