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Answers
a). 4.92
b). 8.70
c). 13.32
Details calculation given in the attachment....
please help Calculate the pH of the solution at every stage of titration. The Ka of...
1) Calculate the pH during the titration of 30 mL of 0.50 M acetic acid HCH3CO2 (Ka = 1.8x10-5) with 0.50 M NaOH after addition of: (a) 0.0 ml NaOH (b) 10.0 mL NaOH (c) 20.0 mL NaOH (d) 30.0 mL NaOH (e) 40.0 mL NaOH
Identify each type of titration curve. Note that the analyte Is stated first, followed by the titration. Drag each graph to the appropriate bin. A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 17.0mL of KOH. A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x 10-5) is titrated with 0.500 M HN03. Calculate the pH after the addition of 21.0mL of HN03. A 52.0-mL volume of 0.35...
52. Consider the titration of 20.0 ml of 0.45 M HOCI (Ka = 1.3x10-5) with 0.15 M Ca(OH)2. a. What is the volume of 0.15 M Ca(OH)2 required to reach the equivalence point. b. What is the pH of the solution at the point which is half-way to the equivalence point? c . C. What is the pH of the solution after addition of a total of 20.0 ml of 0.15 M Ca(OH)2? d. What is the pH of the...
Please answer these 5 questions. 1) a buffer is made by dissolving (CH3NH3)Cl and CH3NH2 in water. Write equations to show how this buffer neutralizes added H3O+ and OH-. 2) If you add 15.0 mL of 1.25 M NaOH to 250. mL of a 0.200 M propanoic acid (CH3CH2CO2H) solution, what is the pH of the resulting solution? 3)If added to 500. mL of 0.20 M NaOH, which of these would form a biffer? Briefly, justify your decision for each...
ASAP please Consider the titration of 50.0 mL of 0.200 M hypochlorous acid HCIO (Ka = 3.5 x 10-8) with 0.250 M NaOH. 5- How many milliliters of NaOH are required to reach the equivalence point? a) b) Calculate the pH before titration c) Calculate the pH after adding 40.0 mL. of NaOH d) Calculate the pOH after adding 20.0 ml, of NaOH
2. Calculate the pH at the following point in the titration of 20.00 mL of0.500 M CH3COOH with 0.500 M NaOH. CH3COOH has a Ka = 1.8x10-5. (2.5 pts) a. pH before the addition of any NaOH. Include balanced chemical equation. b. pH after the addition of 8.00 mL of 0.500 M NaOH. Include balanced chemical equation. c. pH after the addition of 10.00 mL of 0.500 M NaOH. Include balanced chemical equation. d. pH after the addition of 20.00...
Titration of 100.00mL of a 0.1000M solution of a strong acid HCl with 0.100M NaOH solution. Determine the pH at the following points and sketch curve a) before addition of NaOH c) after addition of 20.0 ml NaOH e) after addition of 50.Oml NaOH e) after addition of 100 ml NaOH b) after addition of 10.0mL. NaOH d) after addition of 30.0 ml NaOH f) after addition of 80.Oml NaOH h) after addition of 110 ml NaOH Titration of 100...
1) Calculate the pH in the titration of 50.00 mL of 0.060 M acetic acid (CH3COOH) with a 0.120 M sodium hydroxide, NaOH solution after the addition of the following volumes of base: Ka for acetic acid = 1.8 x 10-5 A) 0 mL pH = B) 10 ml pH =
1. Calculate pH and % ionization of 0.25 M Naco (Ka (HCO2H) 1.8 x 10") 2- Calculate the pH of: a) 0.35 M HNO b) 0.15 M Sr(O)2 c) 0.08 M Ba(CIO4)2 3- Calculate the pH of 0.375 L buffer solution made of a 0.18 M Acetic acid HC2H:02(Ka 1.8x 10) and a 0.134 M Potassium acetate KC2Hs02 (do not use more than 3 digits beyond the decimal point) a) before adding anything b) after adding 0.010 mol Ba(OH)2 c)...
Part B: A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10?5) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25 ?C. Express the pH numerically. MasteringChemistry: ASSIGNMENT #6 (Chapter 16)-Google Chrome https://session.masteringchemistry.com/myct/itemView?assignmentProblem ID=59386 148 CHEM 101 (M03) Help | Close NMENT #6 Titration of Weak Acid with Strong Base Resources Y previous | 19 of 25 | next » ± Titration of Weak Acid with Strong Base A certain weak acid, HA...