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32 Using the following equation, determine the average concentration (moles per liter) of Ca2+ ions present in your water. Record the concentration in Data Table 2. mol Ca2+ / L = L EDTA x mol EDTA / L x 1 mol Ca2+ / 1 mol EDTA x 1 / 0.010 L water 33 Using the following equation, determine the average water hardness of your water. Record the hardness (ppm) in Data Table 2. Note: PPM is equivalent to mg/L for dilute solutions. ppm CaCO3 = mol Ca2+ / 1L x 1 mol CaCO3 / 1 mol Ca2+ x 100.06 g CaCO3 / 1 mol CaCO3 x 1000 mg / 1g Data Table 2: Water Hardness Average Volume of EDTA Used (mL) Concentration Ca2+ Ions Per Liter of Water (mol/L) Water Hardness (ppm CaCO3) Data Table 1: EDTA Titration Volume Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total Volume EDTA Used (mL) 1 9 7 2 2 10 8 2 3 12 9 3 Average Volume of EDTA Used (mL)

          32 Using the following equation, determine the average concentration (moles per liter) of Ca2+ ions present in your water. Record the concentration in Data Table 2.

mol Ca2+ / L = L EDTA x mol EDTA / L x 1 mol Ca2+ / 1 mol EDTA x 1 / 0.010 L water

33 Using the following equation, determine the average water hardness of your water. Record the hardness (ppm) in Data Table 2.

Note: PPM is equivalent to mg/L for dilute solutions.

ppm CaCO3 = mol Ca2+ / 1L x 1 mol CaCO3 / 1 mol Ca2+ x 100.06 g CaCO3 / 1 mol CaCO3 x 1000 mg / 1g

Data Table 2: Water Hardness
Average Volume of EDTA Used (mL)
Concentration Ca2+ Ions Per Liter of Water (mol/L)
Water Hardness (ppm CaCO3)

Data Table 1: EDTA Titration Volume
Trial
Initial EDTA Volume (mL)
Final EDTA Volume (mL)
Total Volume EDTA Used (mL)
1
9
7
2
2
10
8
2
3
12
9
3
Average Volume of EDTA Used (mL)

Show more…

32 Using the following equation, determine the average concentration (moles per liter) of Ca2+ ions present in your water. Record the concentration in Data Table 2.

mol Ca2+ / L = L EDTA x mol EDTA / L x 1 mol Ca2+ / 1 mol EDTA x 1 / 0.010 L water

33 Using the following equation, determine the average water hardness of your water. Record the hardness (ppm) in Data Table 2.

Note: PPM is equivalent to mg/L for dilute solutions.

ppm CaCO3 = mol Ca2+ / 1L x 1 mol CaCO3 / 1 mol Ca2+ x 100.06 g CaCO3 / 1 mol CaCO3 x 1000 mg / 1g

Data Table 2: Water Hardness
Average Volume of EDTA Used (mL)
Concentration Ca2+ Ions Per Liter of Water (mol/L)
Water Hardness (ppm CaCO3)

Data Table 1: EDTA Titration Volume
Trial
Initial EDTA Volume (mL)
Final EDTA Volume (mL)
Total Volume EDTA Used (mL)
1
9
7
2
2
10
8
2
3
12
9
3
Average Volume of EDTA Used (mL)

Added by Jill E.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Lauren Keplinger

11/01/2023

Step 1

First, we need to calculate the moles of Ca2+ ions in the water. To do this, we need to know the volume of EDTA used in the titration and the concentration of the EDTA solution. The equation for this is: mol Ca2+ = volume of EDTA used (L) x concentration of Show more…

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Using the following equation, determine the average concentration (moles per liter) of Ca2+ ions present in your water. Record the concentration in Data Table 2. mol Ca2+ / L = L EDTA x mol EDTA / L x 1 mol Ca2+ / 1 mol EDTA x 1 / 0.010 L water Using the following equation, determine the average water hardness of your water. Record the hardness (ppm) in Data Table 2. Note: PPM is equivalent to mg/L for dilute solutions. ppm CaCO3 = mol Ca2+ / 1L x 1 mol CaCO3 / 1 mol Ca2+ x 100.06 g CaCO3 / 1 mol CaCO3 x 1000 mg / 1g Data Table 2: Water Hardness Average Volume of EDTA Used (mL) Concentration Ca2+ Ions Per Liter of Water (mol/L) Water Hardness (ppm CaCO3) Data Table 1: EDTA Titration Volume Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total Volume EDTA Used (mL) Average Volume of EDTA Used (mL)

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Transcript

00:01 So here we have the data that you provided and we're asked to find the average volume of the edta used in milliliters, the concentration of calcium 2 plus ions per liter of water in moles per liter, and then the water hardness in parts per million calcium carbonate.

00:18 So in order to find the total volume edta used you're going to be subtracting the initial volume from the final volume or vice versa.

00:31 But either way you did that part correctly 9 minus 7 is 2, 10 minus 8 is 2, and 12 minus 9 is 3.

00:39 So we'll go ahead and erase these just so that we can have more space for calculations.

00:52 And so to calculate the average volume we're going to be adding up all of our values and then dividing by the number of values and here we have 3.

01:07 So 2 plus 2 plus 3 is 7, divided by 3 is 2 .33 milliliters.

01:21 And so up here we can write our answer as 2 .33.

01:33 I'll erase this just to give us more room.

01:49 Then to calculate the concentration of calcium 2 plus ions per liter of water we can do the following calculation.

02:12 So we need liters of edta, but we have milliliters.

02:18 So we're going to have to multiply that by a conversion factor and then we have to multiply that by the concentration of edta.

02:33 Which i put a little box here because that wasn't provided.

02:39 But i'm sure you know that value so you can just plug that in.

02:43 And we have a one -to -one stoichiometric coefficient.

03:01 We're also going to divide that by the volume.

03:10 And so this would give us our answer here, but because we don't have that concentration of edta we can't solve for this...

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