5-30. Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 and that for hydrazine is 0.0800 M. Calculate the pH after 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 0.2000 m HCIO,.
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- Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL.AgCl: Ksp = 1.82 x 10^-10I was just wondering how you got the 4.0 x 10-4 for the acidionzation constant.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
- Construct 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.Construct 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 0.0500 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 = 5.636
- Consider the titration of 50.00 mL of 0.160 M NH3 with 0.200 M HCl. Calculate the pH at the following volumes of the titrant: VT = 0.00 (Initial Stage) VT = 20.00 VT = 30.00 Kb = 1.76 x 10-5Find the pH and fraction of dissociation of a 0.010 0 M solution of the weak acid HA with Ka = 1.00 X 10-4.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, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00, and 50.00 mL of 0.2000 M HClO4.
- Consider the titration of 50.00 mL of 0.160 M NH3 with 0.200 M HCl. Calculate the pH at the following volumes of the titrant: VT = 40.00 (Equivalence Point Stage) VT = 45.00 Kb = 1.76 x 10-5What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.875 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 30.00 mL. Ca2+ + Y4- → CaY2- 5.630 g 0.6158 g 0.1500 g 6.158 gFind the pH during the titration of 20.00 mL of 0.1000 Mtri-ethylamine, (CH₃CH₂)₃N (K(b)=5.2X10⁻⁴), with 0.1000 M HCl solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mL