Initial EDTA Volume (mL) Final EDTA Volume (mL) Total volume of EDTA used (mL) T
ID: 879656 • Letter: I
Question
Initial EDTA Volume (mL)
Final EDTA Volume (mL)
Total volume of EDTA used (mL)
Trial 1
10 mL
7.5
2.5
Trial 2
11 mL
6.5
4.5
Trial 3
13 mL
10
3
Average Volume of EDTA Used (mL) : 3.33
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Data Table 2. Water Hardness.
Average volume of EDTA used (mL)
Concentration Ca2+ ions per liter of water (mol/L)
Water hardness (ppm CaCO3)
Please use the following information to fill out this table: show work so i can understand please!
10 mL is the volume of water, and 0.01 is molarity of EDTA
Initial EDTA Volume (mL)
Final EDTA Volume (mL)
Total volume of EDTA used (mL)
Trial 1
10 mL
7.5
2.5
Trial 2
11 mL
6.5
4.5
Trial 3
13 mL
10
3
Average Volume of EDTA Used (mL) : 3.33
33. Using the following equation, determine the average concentration (moles per liter) of Ca ions present in your water. Record the concentration in Data Table 2 of your Lab Report Asslstant moles Ca2+ = (molarity EDTA) x (mL EDTA) mL of water sample 34. Using the following equation, determine the average water hardness of your water. Record the hardness (ppm) in Data Table 2 moles Ca2+ moles Ca2+ Ca × 1 mol CaCO, 100.06 g CaCO. 1 000 mg 1 mol CaC0 100.06 g CaC0 1000 mg ppm CaCO × 1mol Ca2+ 1 mol CaCO3Explanation / Answer
Solution :-
For table 2
Average volume of the EDTA used = 3.33 ml
Molarity of EDTA = 0.01 M
Q33 . Now lets calculate the average concentration of the Ca^2+ in mole per liter
Formula
Moles of Ca^2+ / L = molarity of EDTA * ml of EDTA / ml of water sample
So lets put the values in the formula. Then we get
Moles of Ca^2+ = 0.01 * 3.33 ml / 10.0 ml = 0.00333 mol / L
Q34. Now lets calculate the hardness of water
Ppm CaCO3 =(moles of Ca^2+/1L)*(1 mol CaCO3/1mol Ca^2+)*(100.06g/1 mol CaCO3) *(1000 mg /1g)
= 333.2 ppm
Therefore for the table 2 values for each part are as follows
Average volume of EDTA used = 3.33 ml
Concentration of Ca^2+ ion per liter of water = 0.00333 mol / L
Water hardness = 333.2 ppm