1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used) moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction. 3. Calculate the molar solubility (in mol/L) of OH- and Ca2+. 4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)2 6. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature value. (Ksp of Ca(OH)2 = 8.0 × 10-6 at 25°C)

1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used) moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction. 3. Calculate the molar solubility (in mol/L) of OH- and Ca2+. 4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)2 6. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature value. (Ksp of Ca(OH)2 = 8.0 × 10-6 at 25°C)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

See similar textbooks

Similar questions

The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5.…
Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration = 23.50mL Volume of 0.5N HCl consumed in blank titration = 44.50mL Percent purity (USP/NF) = Aspirin tablets contain NLT 90.0% and NMT 110.0% of the labeled amount of aspirin (C9H8O4) What is the calculated weight (in grams) of pure aspirin?..
Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. What specific type of titration is involved? A. Direct Acidemetry B. Direct Alkalimetry C. Residual Acidemetry D. Residual Alkalimetry 2. What is the analyte- titrant chemical reaction involved? A. Strong Base+Weak Acid B. Weak Acid+Strong Base C. Strong Acid+Weak Base D. Weak Base+Strong Acid 3. What is the preferred indicator for the chosen type of reaction above? A. Methyl Orange B. Penolphtalein C. Methyl Red 4. Consider that the burette was completely filled to the 0mp mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 22.2 mL C. 21.3 mL D. 22.7 mL 5. What is the unknown weight (grams) the problem? Your Answer:
Consider the titration illustrated in Figure 8.] Anhydrous sodium carbonate (Na₂CO₃) is a primary standard. When 0.364 grams of the substance is placed in a conical flask, then 20.00 cm³ of sulphuric acid (H₂SO₄) solution is required to reach the end point of the titration. What is the concentration in mol·dm⁻³ of the sulphuric acid solution? [Give the answer to 3 decimal places. Do not type in the unit. Use a decimal point.] *
Rinse and fill the buret with 0.100 M HCl solution. Transfer accurately 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) into two separate E-flasks. Add 2 drops of phenolphthalein to each flask and titrate each solution until the pink color disappears. Voume of HCl used: Trial 1= 6.80ml; Trial 2 = 6.30mL Determination of solubility and Ksp of calcium hydroxide 2. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 3. Construct an ICE table for the reaction.4. Calculate the molar solubility (in mol/L) of OH- and Ca2+.5. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol)6. Calculate the Ksp of Ca(OH)2.7. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature value.(Ksp of Ca(OH)2 = 8.0 × 10-6 at 25°C)
A sample of water from a river was analyzed by titrating a 125 mL aliquot with 0.0210 M EDTA, consuming 22.52 mL. Express the hardness of the water in ppm of CaCO3.
Based on the analysis of a vinegar solution via titration with 0.1 M NaOH. Results are as follows: Trial 1 Volume of vinegar solution used (mL) 5.00 Final burette reading (mL) 44.20 Initial burette reading (mL) 0.00 Determine the percentage mass of acetic acid in vinegar for Trial 1. The density of vinegar is 1.01 g/mL and molecular mass for acetic acid is 60 g/mol.
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction? CH3COOH + NaOH → NaCH3COO + H2O 2CH3COOH + NaOH → NaCH3COO + H2O C20H14O4 + NaOH → NaC20H14O4 + H2O CH3COOH + 2NaOH → NaCH3COO + H2O
Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. Consider that the burette was completely filled to the 0 mL mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 21.2 mL C. 21.3 mL D. 22.7 mL 2. What is the unknown weight (grams) in the problem? Your Answer:
A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible.What is the MW of calcium carbonate?102 g/mol98 g/mL100 g/mL100 g/molWhat is the molar concentration of the standardized EDTA solution?0.08m0.8M0.08N0.08MHow many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?0.18250.18521.8251.1852
When standardizing two liters of a potassium permanganate solution with a primary standard solution of sodium oxalate, approximately 0.0100 M, it was planned to use between 30.00 mL and 45.00 mL of the titrated reagent. In which mass range (in grams) the primary standard should be weighed? Data: MM KMnO4 = 158.00 g/mol; MM Na2C2O4 = 134.00 g/mol 2CO2 + 2e- ↔ C2O4 2- Eo = -0,432 V MnO4 - + 8 H+ + 5e- ↔ Mn2+ + 4 H2O Eo = 1,52 V
1. Rinse and fill the buret with 0.100 M HCl solution. Transfer accurately 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) into two separate E-flasks. Add 2 drops of phenolphthalein to each flask and titrate each solution until the pink color disappears. Using the titration data for the determination of solubility and Ksp of calcium hydroxide: Parameter Trial 1 Trial 2 Final Buret Reading (mL) 5.80 12.20 Initial Buret Reading (mL) 0.00 5.80 Temperature (in celcius) 25 25 Determine the following:a. Construct an ICE table for the reaction.b. Calculate the molar solubility (in mol/L) of OH- and Ca2+.c. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol) and the Ksp of Ca(OH)2.