11-C. Calculate the pH at each point listed for the titration of 100.0 mL of 0.100 M cocaine (Section 9-4, Kp = 2.6 × 10-6) with 0.200 M HNO,. The points to calculate are V, = 0.0, 10.0, 20.0, 25.0, 30.0, 40.0, 49.0, 49.9, 50.0, 50.1, 51.0, and 60.0 mL. Draw a graph of pH versus V.
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- 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 =5.636Construct 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.A 50ml aliquot of 0.0500 M NaCN (Ka, HCN = 6.2x10^-10) is titrated with 0.1000 M HCl. Discuss which of the following indicators would be best used for the titration of 0.05000 M NaCN with 0.1000 M HCl: bromocresol green (transition range pH: 3.8-5.4), bromothymol blue (transition range pH: 6.2-7.6), or phenolphtalein (8.3-10.0)
- Titration is performed on 30 mL of 0.04 M Hydrazine (NH2NH2) (Kb: 2.10-6 ) with 0.02 M HCl in the following volumes . Find the pH values.)(ka:1,4x10-5) (volumes:30 mL ; 45 mL ; 90 mL ; 120 mL; DN)Consider the titration of 110.0 mL analyte solution containing 0.15 mol L-1 NH3 with 0.10 mol L-1 HCI titrant. Determine the pH of the solution after adding 25.0 mL of titrant. (Kb(NH3) = 1.8 x 10-5, T= 250C).10.00 mL of 0.2099 M iodic acid {Ka = 1.70 xx 10^(-1)} is titrated with 0.1057 M NaOH. a) What is the pH after 14.61 mL of NaOH are added to the solution?
- 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.The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?A student titrated a 5.00-mL saturated borax sample at 15.7°C. The titration reaction is as follows: B4O5(OH)42–(aq) + 2 HCl(aq) + 3 H2O(l) → 4 B(OH)3(aq) + 2 Cl–(aq) What is the KSP of borax (Na2B4O5(OH)4) if the titration required 8.26 mL of 0.2004 M HCl?
- 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 = 5.636Find the pH during the titration of 20.00 mL of 0.2850 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.2850 M NaOH solution after the following additions of titrant. (a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 20.00 mL(e) 25.00 mLWrite the reaction between formic acid (Appendix B) and KOH. What is the equivalence volume (Ve) in the titration of 50.0 mL of 0.050 0 M formic acid with 0.050 0 M KOH? Calculate the pH at the points Vb 0.0, 10.0, 20.0, 25.0, 30.0, 40.0, 45.0, 48.0, 49.0, 49.5, 50.0, 50.5, 51.0, 52.0, 55.0, and 60.0 mL. Draw a graph of pH versus Vb. Without doing any calculations, what should the pH be at Vb5 12 Ve? Does your calculated result agree with the prediction?