8. You are titrating 50.0 mL of 0.200 M propanoic acid with 0.100 M NaOH. Use the data in the table toanswer the questions.NamePropanoic acidStructureCH3CH2CO2Hpka4.874Ka1.34 × 10-5a) Assuming that the equivalence point is considered 100% completion, calculate the pH at thefollowing points: 0%, 10%, 50%, 90%, 100%, and 120%.b) Sketch the titration curve.c) What would be an ideal pKa for an indicator to use in this titration?

Answered: Image /qna-images/answer/ada05cd4-efe6-4709-8fc2-51bad8c1f827.jpg

Answered: 8. You are titrating 50.0 mL of 0.200 M…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results aregiven in the graph above.I) What is the approximate pKa of the acid? II) What specific value from the graph is needed, in addition to the information in partc above, to calculate the molar concentration of the NaOH? III) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid beingtitrated is less than the concentration of the conjugate base.
if 150. ml of 0.50 M formic acid (HCOOH) is titrated with the strong base of 0.50 M. KOH (Ka for HCOOH = 1.8 x 10-4)a) Determine the pH for the point at which 100. mL of KOH has been added Determine the pH for the equivalnce point
5. A certain acetic acid solution has pH required to reach the equivalence point in the titration of 25.0 mL of the acetic acid solution. (Ka = 1.80 x 10-5) = 2.68. Calculate the volume of 0.0975 M KOH
A chemist titrates 60.0 mL of a 0.2562M benzoic acid (HC6H5CO₂) solution with 0.0811M KOH solution at 25 °C. Calculate the pH at equivalence. The pK of benzoic acid is 4.20. a Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = X S
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) +…
Ka for ethanoic acid is 1.7*10^-5 moldm-3. Show by calculation that the initial pH in experiment B is 4.8.
A chemist titrates 80.0 mL of a 0.8628 M trimethylamine ((CH) N solution with 0.2165 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of trimethylamine is 4.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH =||
Hydrofluoric acid has a Ka of 6.6 x 10-4. 40.00 mL of 0.150 M sodium fluoride, NaF, is titrated against 0.125 M HBr. Give the pH at these four points: initial, 32.00 mL of acid have been added, at the equivalence point, and when 60.00 mL have been added.
2.74 g of canola oil were titrated with KOH. It required 13.92 mL of 0.0040 M KOH to reach the equivalence point. What is the acid number? Your Answer: Answer units
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. compound CuBr BaCO3 K Cl Does solubility change with pH? yes no yes no yes no pH = 5 highest solubility pH = 7 pH = 8
18. By mixing 1.00-mol benzoic acid (C6H$COOH), K3 = 6.3 x 105) and 1.00-mol methylamine (CH;NH2, Kb = 5.6 x 10 *) into 1-L solution, the solution pH at equilibrium will be a) greater than 7 b) equal to 7 c) less than 7 d) insufficient information.
1.What is the Ka of a weak acid, HA, that forms a buffer of pH 5.50 when combined in an equal concentration with its conjugate base, A−? Answer: Ka= ...... x 10^-6 2.Calculate the pH of 0.136 M potassium nitrite, KNO2. The ionization constant of nitrous acid, HNO2, is Ka= 5.6× 10-4 3.Calculate the pH of a solution of magnesium hydroxide, Mg(OH)2 (Ksp = 5.6 × 10−12), made by dissolving solid Mg(OH)2 in pure water until the solution is saturated.

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