II. Determination of Total Hardness of Water Source of water sample: Volume of water sample 22.00 mL Final volume reading (EDTA solution) Initial volume reading (EDTA solution) Volume consumed (EDTA solution) Molarity of standard EDTA solution used 34.60 mL 20.54 mL 14.06 mL 0.25 M Total hardness of water (ppm CaCO3)
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Find the total hardness of water and its average using the table below. Please indicate your solution
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- Concentration of Acetic Acid in a Vinegar Solution. Average molarity of NaOH Volume HC₂H30₂ sample Final buret reading Initial buret reading Volume NaOH (Show all units and all calculations) Molarity of HC₂H30₂ (unrounded) Average molarity of HC₂H302 (unrounded) Deviations Average deviation Best estimate for molarity of HC₂H302 Average mass percent HC₂H302 46.4mL Oml Ran out of Base ↓ ↓ ↓ ↓ 10.014 HOA je beart giov isults weari?! ferottelucuny Cambia) 10 Kousad Question 1. A Rolaids tablet contains calcium carbonate that neutralizes stomach acid. If 44.55 mL of 0.448 M hydrochloric acid is required to neutralize one tablet, how many milligrams of calcium carbonate are in a Rolaids tablet? CaCO, (s) + 2HCl(aq) → CaCl₂ (aq) + H₂O (1) + CO₂ (g)TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 2 TRIAL 3 Weight of KHP, g 0.1012 0.1004 0.09987 Initial volume of NaOH, mL 5.00 10.01 Final volume of NaOH, mL 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL 1.00 1.00 1.00 14.98 22.90 30.87 Final volume of NaOH, mL 22.84 30.77 38.75 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acidPart Il: Determination of Standard Solutions mL of 0.200 mL H20 added M Cuso, diluted Tube # M Cuso4-5 H20 added Absorbance about 3 0.200 1.346 3. 4.00 1.00 0.945 4 3.00 2.00 0.715 2.00 3.00 0.469 6. 1.00 4.00 0.281 show calculation for Tube #3 diluted concentration:
- Determine the total hardness of water (ppm CaCO3; MM: 100.09 g/mole) if 100.0mL sample of drinking water required 38.41mL of 4.65 x 10-3 M EDTA for titration. 179 ppm CaCO3 357 ppm CaCO3 452 ppm CaCO3 733 ppm CaCO3Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300 mL with water. A 20 mL aliquot was titrated with 5.02 mL of 0.5352 M HCl to reach PHP endpoint. Another 20 mL aliquot was titrated to the BCG endpoint, using up 18.87 mL of titrant in the process. Note: Answer in two decimal places only. If there is no answer, type in 0.00. Use the molar masses 105.989 ?/??l ??2cO3 and 84.007 g/mol NaHCO3 indicated. The volume of titrant needed to neutralize NaOH is _________ mL.The volume of titrant needed to neutralize Na2CO3 is _____________ mL.The volume of titrant needed to neutralize NaHCO3 is _____________ mL. The mass of NaOH is ___________ g.The mass of Na2CO3 is __________ g.The mass of NaHCO3 is __________ g. The percent weight of NaOH is __________ %.The percent weight of Na2CO3 is __________ %.The percent weight of NaHCO3 is __________ %.
- Which of the following will result to a brightly lit light bulb when subjected to the conductivity test? a. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 b. 70% (v/v) ethanol c. 1.0 M citric acid d. Glacial acetic acidA. Standardlzatlon of thlosulfate solutlon Trial 1 Trial 2 Trial 3 Initial volume of thiosulfate (mL) 0.00 20.05 2.3 Final volume of thiosulfate (mL) 20.05 40.05 22.15 Volume of thiosulfate used (mL) Molarity of thiosulfate Average Molarity of thiosulfate Calculate the molarity of the thiosulfate solution using the formula: 6 mmol S20,²- 1 mmol 10, Ms,0,2- 0.004167 M 10,- 20.00 ml Vol S20,²- used (mL)Part III: Determination of Saturated Solutions Molarity (saturated) Tube # Temperature (°C) Molarity (dilute) Absorbance 2 0.6 0.157 20.1 0.291 4 37.6 0.351 50.1 0.500 6. 70.9 0.714 show calculation for Tube #2, Molarity (dilute) (use graph equation): show calculation for Tube #2, Molarity (saturated): 1. Is the relationship between solubility and temperature direct or inverse? Explain.
- Calculate the activity coefficient of Li* ion in a solution of 0.005 mol/L ionic strength. (a =0.6 nm) 0 2. 0.36 O b. 0.93 c. 0.29 d. 0.52 e. 0.73 الننتنامى كلية العلومsolute 0.147 g C6H7NaO6 molar mass 198.11, dissolves in 50.00 mL, absorbance of solution 0.862, absorbance of standard 0.863 calculate moles of solute, volume of solution (L), %m/v, M, % errorA sample of sodium carbonate; NazCO3 (MW=105.9 g/mole) weighing 0.3125 g was dissolved in 40.0ml distilled water and titrated with HCl solution and required 23.6 ml to reach the endpoint. Calculate the molarity of the HCI solution. 6.96 M 6.96 x10 -5 M. 0.125 M 0.25 M