Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10-5. NEXT 3 4. Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. 2. 1. + C4H,O2 (aq) (1)O?H OH (aq) HC,H;O2(aq) + Before (mol) Change (mol) After (mol) ORESET c.OL x 00'7- c.0L x 00'L- 6OL x 00'7 c.01 x 00'L 007'0 00L'O c.OL x 00'8 e0L x 00'8- cOL x 00'2 c.0L x 00'L- cOL x 00'9 e.OL x 00'9-

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10-5. NEXT 3 4. Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. 2. 1. + C4H,O2 (aq) (1)O?H OH (aq) HC,H;O2(aq) + Before (mol) Change (mol) After (mol) ORESET c.OL x 00'7- c.0L x 00'L- 6OL x 00'7 c.01 x 00'L 007'0 00L'O c.OL x 00'8 e0L x 00'8- cOL x 00'2 c.0L x 00'L- cOL x 00'9 e.OL x 00'9-

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
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Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
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10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most
b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.
A buffer was made by mixing 0.1404 moles of HN3 with 0.1025 moles of KN3 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2367 M HBr to 50.00 mL of the buffer? Ka(HN3) = 1.900e-5. Note: only a portion of the original buffer is used in the second part of the problem.
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A sample of vinegar weighing 10.52 g is titrated with NaOH. The end point is overstepped, and the solution is titrated back with HCl. From the following data, calculate the acidity of the vinegar in terms of percentage of acetic acid, CH3COOH Standardization Data:1.050 mL HCl ≡ 1.000 mL NaOH1.000 mL NaOH ≡ 0.06050 g benzoic acid, C6H5COOH (122.12 g/mol) Analysis Data:Volume NaOH used = 19.03 mLVolume HCl used for back titration = 1.50 mL