Question

Data: Trial Initial Volume of EDTA (mL) Final Volume of EDTA (mL) 1 10ml 9ml 2...

Data:

Trial

Initial Volume of EDTA (mL)

Final Volume of EDTA (mL)

1

10ml

9ml

2

9ml

8ml

3

8ml

7ml

Calculate the concentration of Ca+2 ions per liter of water using the following equation.

Calculate the water hardness using your results from part 2 and the following equation.

Calculate the average water hardness for the three trials conducted. Show all work.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Water Hardness Lab follow up Questions Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total...
Water Hardness Lab follow up Questions Trial Initial EDTA Volume (mL) Final EDTA Volume (mL) Total Volume of EDTA Used (mL) 1 8.5 6 2.5 2 5.0 3.0 2.0 3 3.0 0.5 2.3 Average Volume of EDTA Used (mL): 2.3 Average Volume of EDTA Used (mL) Concentration Ca2+ Ions Per Liter of Water (mol/L) Water Hardness (ppm CaCO3) 2.3 0.0023 230 2.Approximately how much calcium would you ingest by drinking six, 8-oz glasses of your local water? Hint: 1 oz...
1. Standardization of the sodium thiosulfate solution Volume of 0.0100M KIO3 samples 10 mL Data Trial...
1. Standardization of the sodium thiosulfate solution Volume of 0.0100M KIO3 samples 10 mL Data Trial 1 Trial 2 Trial 3 Volume of Na2S2O3 Titrant Final Buret Reading 0.76 mL 0.73mL 0.78mL Initial Buret reading 7.00 mL 7.00 mL 7.00mL Net Volume of Na2S2O3 6.24 mL 6.27 mL 6.22 mL Calculated concentration of Na2S2O3 (?) M (?) M (?) 2. Molar Solubility of Ca(IO3)2 in pure water Temperature of the saturated solution of calcium iodate = 22.8 celcius Volume (or...
Trial #1 Trial #2 Trial #3 Total Volume of solution at equilibrium 11.9 mL 12.9 mL...
Trial #1 Trial #2 Trial #3 Total Volume of solution at equilibrium 11.9 mL 12.9 mL 12.2 mL Volume of water added to reach equilibrium 8.9 mL 9.7 mL 9.2 mL Mass of Urea 3.0570g 3.3634g 3.1331g Using the formula K = [urea] / Xsolvent: Calculate the mole fraction of water for each trial and calculate the new equilibrium constant based on the mole fraction.
Initial NaOH volume mL Final NaOH volume mL Total volume of NaOH used mL 9 0...
Initial NaOH volume mL Final NaOH volume mL Total volume of NaOH used mL 9 0 9 9 0.2 8.8 9 0.3 8.7 Three trials, average volume of NaOH used mL = 8.8 Average volume of NaOH used mL Concentration CH3COOH in vinegar mol/L % CH3COOH in vinegar 8.8 72 83 1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer...
Mass of Ca(s) 0.5 g volume of water 50.0 mL initial temp 25.6 C final temp...
Mass of Ca(s) 0.5 g volume of water 50.0 mL initial temp 25.6 C final temp 48.5 C calculate the enthalpy of dissolution of Ca in water in kJ/mol
1- A 0.0456 g sample of an unknown sample was titrated using the EDTA titrant from...
1- A 0.0456 g sample of an unknown sample was titrated using the EDTA titrant from question 1 and the procedure below. The starting burette volume was 0.05 mL. The ending burette volume was 42.35 mL. Calculate the % calcium oxide (CaO; 56.0774 g/mol) by mass in the sample. Show all work. 2-  100.0 mL of an unknown water sample was titrated using the EDTA from question 1 and the procedure below. The starting volume was 0.25 mL and the ending...
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration...
The hydroxide ion concentration, [OH-], in each of your trials can be calculated from the concentration of the hydrochloric acid, 0.050 M HCl, and the volume of both the HCl and Ca(OH)2 used in the titration. According to the net ionic equation (calcium hydroxide, Ca(OH)2 (s), in water) determine the ratio of moles of calcium ion, Ca2+, to moles of hydroxide ion, OH-, in the solution of calcium hydroxide, Ca(OH)2. Using this ratio, determine the molarity of calcium ion in...
Molarity of NaOH: 0.1388 M Unknown Acid Buret: Trial 1 Trial 2 Initial Buret Reading 27.11...
Molarity of NaOH: 0.1388 M Unknown Acid Buret: Trial 1 Trial 2 Initial Buret Reading 27.11 ml 17.91 ml Final Buret Reading 47.31 ml 42.01 ml Volume of acid added 20.10 ml 24.10 ml Results: Trial 1 Trial 2 Volume of NaOH at equivalence point 4.75 mL 14.03 mL Volume of NaOH at one-half the equivalence point 2.37 mL 7.015 mL pH at half equivalence point 4.88 4.21 pKa of unknown acid Average pKa Average Ka Moles of unknown acid...
Mass of water 200 g Volume of water 200 mL Fuel Initial mass of fuel (g)...
Mass of water 200 g Volume of water 200 mL Fuel Initial mass of fuel (g) Final mass of fuel (g) Initial temp of water (oC) Final temp of water (oC) Fuel Canister (diethylene glycol) 129.7 121.7 25 106 Tea Candle (Paraffin Wax) 12.0 11.8 25 32 Calculate the amount of energy released during the combustion of each fuel using the given equation. Show all work. Q = ΔTmcp Diethylene glycol: Tea candle: Calculate the amount of grams of each...
Trial Volume of H2SO4, (mL) Vinitial NaOH, (mL) Vfinal NaOH, (mL) Molarity H2SO4, (mol/L) Molarity of...
Trial Volume of H2SO4, (mL) Vinitial NaOH, (mL) Vfinal NaOH, (mL) Molarity H2SO4, (mol/L) Molarity of NaOH, (mol/L) 1 14.60 50.00 38.90 0.1468 0.2019 2 14.90 38.90 24.60 0.1649 0.2132 3 15.15 24.60 13.20 0.1684 0.2122 a.) Calculate the number of moles of OH- for each trial for the titration of H2SO4 with NaOH. Determine the average number of moles of OH- b.) From your calculation in part a, calculate the molarity of H+ ions in your sample of H2SO4