2. Construct a curve for the titration of 20.00 mL 0.0250 M selenious acid (H₂SeO3) by 0.0500 M NaOH solution. You may use MS Excel® for convenience. Titrant volumes: 0.00 mL, 5.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL. H₂SeO3 + H₂O HSeO3 + H3O+ HSO3 + H₂O = SeO3²- + H3O+ Ka₁ = 2.40 x 10-3 Ka₂ = 4.80 x 10-⁹
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- Construct a curve for the titration of 20.00 mL 0.0500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. MS Excel® can be used. Titrant volumes: 15.00 mL, 20.00 mL, and 25.00 mL. (CH2)2(CO2H)2 ⇌ (CH2)2(CO2H)(CO2)^− + H^+ Ka1 = 6.21 × 10^-5; pKa1 = 4.207 (CH2)2(CO2H)(CO2)− ⇌ (CH2)2(CO2)2^2− + H^+ Ka2 = 2.31 × 10^-6; pKa2 = 5.636Construct a curve for the titration of 50.0 mL of 0.100 M hydrazoic acid, HN3 (Ka = 2.2 x 10-5) with 0.200 M solution of KOH. Calculate the pH after the addition of 0.00,12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45, and 50.00 mL of titrant. Identify the specie/species present at the following regions of the curve:a. Start of the titrationb. Before equivalence pointc. At equivalence pointd. Past the equivalence point.Construct a curve for the titration of 20.00 mL 0.500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. Use MS Excel for convenience. Titrant volumes: 0.00 mL, 5.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL. (CH2)2(CO2H)2⇄(CH2)2(CO2H)(CO2)^- +H^+ Ka1= 6.21 x 10^-5; pKa1 =4.207 (CH2)2(CO2H)(CO2)^-⇄(CH2)2(CO2)2^2-+ H^+ Ka2= 2.31 x 10^-6; pKa2 =5.636
- A solution of nitrous acid (0.101 M, 25.22 mL) was titrated with 0.173 M sodium hydroxide (Ka = 4.00 x 10-4). What is the pH after the addition of the following volumes of sodium hydroxide? Part 1: 2.945 mL Part 2: 14.72 mL Part 3: 17.67 mLConstruct a curve for the titration of 50.0 mL of 0.100 M hydrazoic acid, HN3 (Ka = 2.2 x 10-5) with 0.200 M solution of KOH. Calculate the pH after the addition of 0.00, 12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45, and 50.00 mL of titrant. Identify the specie/species present at the following regions of the curve:1. Start of the titration2. Before equivalence point3. At equivalence point4. Past the equivalence point.Determining the ksp of Calcium Hydrioxides Titration of Calcium Hydroxide with HCl Mass of Erlenmeyer flask: 25.52 g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) (g): 28.44 g Mass of Calcium Hydroxide Solution (g): 2.92 g Volume of Ca(OH)2 Density = 1.000 g/mL (mL) - 2.92 mL Concentration of HCl (M) - How do you find this? HCl 0.10 M solution used Initial HCl volume = 0.79 mL Final HCl volume = 0.09 mL volume of HCl delivered = 0.70 mL Moles of HCl delieverd - how do I calculate this? Moles of OH- in sample - how do I calculate this? Moles of Ca2+ in sample - how do I calculate this? Thank you!
- Determining the ksp of Calcium Hydrioxides Titration of Calcium Hydroxide with HCl Mass of Erlenmeyer flask: 25.52 g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) (g): 28.44 g Mass of Calcium Hydroxide Solution (g): 2.92 g Volume of Ca(OH)2 Density = 1.000 g/mL (mL) - 2.92 mL Concentration of HCl (M) - How do you find this? HCl 0.10 M solution used Initial HCl volume = 0.79 mL Final HCl volume = 0.09 mL volume of HCl delivered = 0.70 mL Moles of HCl delieverd - 0.07 x 10^-3 mol Moles of OH- in sample - 0.07 x 10^-3 mol Moles of Ca2+ in sample - 0.035 x 10^-3 mol How do I calculate molar solubility and ksp? Thanks!!concentration of I3- : 0.002M d. Titration data: Final volume: 29.05 mL Starting volume: 38.10 mL Delivered volume: 25.15 mL How do you calculate g?A titration experiment, using 0.0175M Ba(OH)2 just neutralized 14.5 ml of HNO3 solution. Calculate the molarity of the HNO3 solution. The titration data is below /9 Titration data of Ba(OH)2 Burette Reading Trial 1 Trial 2 Trial 3 Initial Vol (mL) 0 13.01 25.22 Final Vol (mL) 13.01 25.22 37.5
- Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of HClO4 is 0.1000 M and that of formic acid is 0.0800 M. Calculate the pH after the addition of 0.00,10.00, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00 and 50,00 ml of KOH 0,2000 M.Consider the titration of 300.0 mL of 0.500 M NH3 (Kb = 1.8 x 10-5) with 0.500 M HNO3. What is the pH of the solution when 248 mL of 0.500 M HNO3 has been added to the base? **Report your answer to two decimal places. DO NOT worry about significant figures.**Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 M and that for hydrazine is 0.0800 M. Calculate the pH after addition of 0.00, 10.00, 25.00, 35.00, 45.00 and 50.00 mL of 0.2000 M HClO4.