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# Gravimetric Analysis of water hardness - PowerPoint PPT Presentation

Gravimetric Analysis of water hardness. Have you ever noticed this?. “Hard” water has ions that are dissolved in it, but can eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets). Why is our water “hard”?.

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Presentation Transcript

### Gravimetric Analysis of water hardness

“Hard” water has ions that are dissolved in it, but can eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

Why is our water

“hard”?

Where does our water come from? eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

Where does our water come from? lakes eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

Lakes are surrounded by rock, so calcium chloride and other minerals dissolve into the water.

Where does our water come from? lakes eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

Lakes are surrounded by rock, so calcium chloride and other minerals dissolve into the water.

Isn’t our water treated before drinking?

Where does our water come from? lakes eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

Lakes are surrounded by rock, so calcium chloride and other minerals dissolve into the water.

Isn’t our water treated before drinking?

It is treated for bacteria and other things that can make us sick (mainly with chlorine), but it is not purified.

So, how hard is our water? eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

So, how hard is our water? Let’s find out. eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

In this lab we will measure the amount of calcium in the water and compare that to a “water hardness” scale.

But first, we’ll find the calcium in a standard solution to practice our techniques and determine how well they work.

### Gravimetric Analysis of a Standard solution eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

We will be starting with 20 eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).mL of a 1.0 molar solution of calcium chloride and mixing it with 20 mL of a 1.0 molar solution of sodium carbonate.

When we mix 20 mL of a clear solution of 1.0 molar calcium chloride and 20 mL of a clear solution of 1.0 molar sodium carbonate, then we should get a solution containing a white, solid precipitate of calcium carbonate.

• And then real life gets in the way of chemistry… eventually combine with other ions to form a solid, and precipitate out of the water (and on to your faucets).

• We rarely get the full amount of products. To know how well our reaction actually worked, we calculate a percent yield.

• So we have the mass of the filter alone. (precipitate) that gets caught on the filter, so we have to do some preparation.

• Then we filter.

• Then we have our precipitate caught on the filter, but there is a problem.

• So we have the mass of the filter alone. (precipitate) that gets caught on the filter, so we have to do some preparation.

• Then we filter.

• Then we have our precipitate caught on the filter, but there is a problem.

• The filter will be wet. So it will have to dry before we measure the mass.

### Gravimetric Analysis of a Unknown solution (precipitate) that gets caught on the filter, so we have to do some preparation.

• Water of unknown calcium chloride content = tap water. (precipitate) that gets caught on the filter, so we have to do some preparation.

• We will repeat the steps as with the standard solutions, but will need some additional calculations:

• Calculate theoretical amount, in molarity

• Water of unknown calcium chloride content = tap water. (precipitate) that gets caught on the filter, so we have to do some preparation.

• We will repeat the steps as with the standard solutions, but will need some additional calculations:

• Calculate theoretical amount, in molarity

• Convert molarity to Parts Per Million (ppm)

• Water of unknown calcium chloride content = tap water. (precipitate) that gets caught on the filter, so we have to do some preparation.

• We will repeat the steps as with the standard solutions, but will need some additional calculations:

• Calculate theoretical amount, in molarity

• Convert molarity to Parts Per Million (ppm)

• Then we can compare to a chart and see how hard our water is.