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Calcium in water

Index

Introduction

- N&G profile

- Research the difference in calcium ions

- Tap- and mineral water

- determination of Calcium ions

- Does this have effect on us?

  • Introduction
  • Aims and Sub-aims
  • Hypothesis
  • Theory
  • Experiment
  • Results
  • Processing of the results
  • Conclusion

Theory

Effects of hard and soft water

- 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 of water in Holland

- 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

Overview :

Hypothesis

Exact measurements

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 :

Research question

( • = 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

Conclusion

- 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

  • Variation in calcium ion concentration
  • Tap water -> less calcium ions

Cleaned with machines

  • Mineral water -> more calcium ions

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

Sub questions

questions?

  • Is tap water or mineral water better?
  • Why are there more calcium ions in mineral- or tap water?

  • More calcium mineral water -> hard water, not purified.
  • Water with calcium good for us?

indicator

EDTA molecule

EDTA

Aims and sub-aims

Research question

  • What is the difference in calcium level between mineral- and tap water?

Our sub-questions consist of :

  • Is plain tap water or mineral water better for us?
  • Why are there more calcium ions in mineral- or tap water?
  • Is hard water with calcium ions good for us instead of soft water?

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