Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pKa = 4.75) with 0.131 M NaOH. CH, COОН(аq)+NaOH(aq) CH;COO¯(aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =

Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pKa = 4.75) with 0.131 M NaOH. CH, COОН(аq)+NaOH(aq) CH;COO¯(aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.103QE

See similar textbooks

Similar questions

Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M inNH3(aq) and 0.100 M in NH4Cl(aq). ΔpH= Calculate the change in pH when 7.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. ΔpH=
in the titration of 50.0 mL of 0.0200 M C6H5COOH(aq) with 0.100 M NaOH(aq), what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO₂H, in enough water to make 5.00 x 10² mL of solution and then titrate the solution with 0.168 M NaOH. C6H5CO₂H(aq) + OH(aq) → C6H5CO₂ (aq) + H₂O(l) What are the concentrations of the following ions at the equivalence point? 0.0037 1.30e-8 Na+, H3O+, OH™ C6H5CO₂ X M Na+ ✓ MH 30+ X MOH™ 7.66e-7 0.0037 XM C6H5CO₂ What is the pH of the solution? 7.86
Consider the titration of 25.0 mL of 0.124 M acetic acid (CH₂COOH, pK, = 4.75) with 0.125 M NaOH. CH3COOH(aq)+NaOH(aq) CH₂COO (aq) + H₂O(l) + Na+ (aq) Determine the initial pH of the 0.124 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.125 M NaOH is added. pH = Determine the volume of 0.125 M NaOH required to reach halfway to the stoichiometric point of the titration. volume NaOH: - Determine the pH of the solution when enough NaOH has been added to reach halfway to the stoichiometric point. pH = Determine the volume of 0.125 M NaOH that is required to reach the stoichiometric point of the reaction. volume NaOH: Calculate the pH of the solution when the stoichiometric point of the titration has been reached. pH = mL mL
A volume of 500.0 mL of 0.160 M NaOH is added to 525 mL of 0.250 M weak acid (K₁ = 3.24 × 10-5). What is the pH of the resulting buffer? pH = HA(aq) + OH¯(aq) H,O(l) + A(aq)
A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined. 2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.
Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?
PHASE 1: How to calculate the pH of a buffer solution Calculate buffer pH Complete the following steps: 1) Calculate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH3COONa, in 85.0 mL of 0.10 Macetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5. 1 Calculate pH of buffer solution pH =
Calculate the molar solubility of Mg(OH)2 in 1.00 M NH4Cl (aq).
A 20.00 mL aliquot of sorbic acid solution (HC6H7O2) was titrated with 0.0985 M NaOH * (aq) using both an indicator and a pH meter. Ka (HC6H7O2) , is 1.7*10^ -5 . A total of 25.34 mL of 0.0985 M NaOH * (aq) was required to reach the equivalence point a) Calculate the molarity of the sorbic acid solution. b) Calculate the pH of the sorbic acid solution (use the RICE table) . c) .Calculate the pH and [C6H 7 O 2-] at the half-equivalence point . d) Calculate the pH at the equivalence point of the titration . (use Kb for hydrolysis of sorbate anion and RICE table ). e)Suggest an appropriate indicator for titration . Explain your choice . f) Calculate the pH of the solution after 10.00 mL of 0.0985 M NaOH * (aq) was added . (find moles of sorbic acid and sorbate and use Henderson Haselbalch equation ) Indicator pKa Phenolphthalein 9.3 Bromothymol blue 7.0 Methyl red. 5.0 Thymol blue. 2.0 Methyl violet…
In a titration of acetic acid by sodium hydroxide, what is the pH of a 100.0 mL of a 0.1000 M CH3CHO2H(aq) solution after 25.00 mL of 0.2000 M NaOH(aq) has been added? The Ka of acetic acid is 1.75 x 10-5,
A solution is prepared by adding 100 mL of 1.0 M HC,H,O,(aq) to 100 mL of 1.0 M NaC,H,O,(aq). The solution is stirred and its pH is measured to be 4.73. After 3 drops of 1.0 M HCl are added to the solution, the ph of the solution is measured and is still 4.73. Which of the following equations represents the chemical reaction that accounts for the fact that acid was added but there was no detectable change in pH? (A) H;O*(aq) + OH (aq) → 2 H,O(1) (B) H;O*(aq) + CI (aq) → HCI(g) + H,O(1) (C) H,O*(aq) + C,H,O, (aq) → HC,H,0,(aq) + H,0(1) (D) H;O*(aq) + HC,H,O,(aq) - H,C,H,0,*(aq) + H,O()