A 40.0 mL solution of 0.100 mol/L acetic acid, CH,COOH (K, = 1.8 x 105), is titrated with 0.100 mol/L sodium hydroxide at 25 °Č. At the equivalence point: %3D А. The pH is equal to 7.00. В. The pH is less than 7.00. С. Equal moles of H,O* and NaOH have reacted together. D. Equal moles of CH;COOH and NaOH have reacted together. Е. More than one of the above choices is correct.

A 40.0 mL solution of 0.100 mol/L acetic acid, CH,COOH (K, = 1.8 x 105), is titrated with 0.100 mol/L sodium hydroxide at 25 °Č. At the equivalence point: %3D А. The pH is equal to 7.00. В. The pH is less than 7.00. С. Equal moles of H,O* and NaOH have reacted together. D. Equal moles of CH;COOH and NaOH have reacted together. Е. More than one of the above choices is correct.

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...

See similar textbooks

Similar questions

the strong acid hydrobromide acid, HBr(aq) is titrated with strong base sodium hydroxide, NaOH(aq). The neutralization reaction is given by: HBr (aq) + NaOH (aq) -> NaBr (aq) + H2O (l). Pick from the options listed below to get the best indicator to identify the equivalence point of the titration. A-Bromocresol purple B- m-Nitrophenol C- Methyl orange D- Bromothymol Blue E- Thymol blue
A 1.00 liter solution contains 0.32 M hydrocyanic acid and 0.24 M potassium cyanide. If 30.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water.) v A. The concentration of HCN will decrease. v B. The concentration of CN will increase. vC. The equilibrium concentration of H;O will increase. v D. The pH will remain the same. v E. The ratio of [HCN] [CN]will decrease.
In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker. After 22.04 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution? Report your answer with 3 sig figs
In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.65 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?
GW 18b 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH. Determine: (a) pH of the acid solution before any base is added; (b) volume (in mL) of base needed to get to the equivalence point; (c) pH halfway to equivalence point; (d) pH at equivalence point; (e) pH when 0.100 mL NaOH is added beyond the equivalence point. (K₂ of HF = 7.1 × 104)
A chemist titrates 160.0 mL of a 0.6712M benzoic acid (HC6H5CO₂) solution with 0.6137M NaOH 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 NaOH solution added. pH = X
1.0 L of a buffer solution is created which is 0.363 M in hydrocyanic acid, HCN, and 0.303 M sodium cyanate, NaCN. Ka for HCN = 4.0 × 10-10 What is the pH after 0.107 mol of NaOH is added to the buffer solution? O a. 9.928 O b.9.602 O c. 9.319 O d. 9.193 O e. 9.398
A 27.0 mL solution of 0.110 M CH3COOH is titrated with a 0.210 M KOH solution. Calculate the pH after the following additions of the KOH solution: Note: Reference the K of acids at 25 °C table for additional information. a Part 1 of 2 0.00 mL KOH added. Be sure your answer has the correct number of significant digits. pH ==== 2.85 Part 2 of 2 5.00 mL KOH added. Be sure your answer has the correct number of significant digits. Check pH = => 4.48 X Save For Later Submit Assignment
A 1.00 liter solution contains 0.45 M ammonia and 0.35 M ammonium nitrate. If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of NH, will increase. B. The number of moles of NH, will remain the same. v C. The equilibrium concentration of H;0 will increase. D. The pH will remain the same. E. The ratio of [NH3] [NH,]will remain the same.
A 1.00 liter solution contains 0.28 M ammonia and 0.36 M ammonium chloride. If 0.180 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) A. The number of moles of NH3 will remain the same. B. The number of moles of NH4* will decrease. C. The equilibrium concentration of H₂O* will remain the same. D. The pH will increase. E. The ratio of (NH3)/ [NH4*] will increase. Submit Answer Retry Entire Group 5 more group attempts remaining
A chemist titrates 100.0 mL of a 0.0714M nitrous acid (HNO,) solution with 0.3683M KOH solution at 25 °C. Calculate the pH at equivalence. The p K, of nitrous acid is 3.35. 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 = |
In titrating HC2H3O2 (aq) with 0.1 M NaOH, the equivalence point in pH units will be A. lower than 7 due to hydrolysis of HC2H3O2 B. lower than 7 due to hydrolysis of Na+ C. higher than 7 due to hydrolysis of C2H3O2- D. equal to 7 since the acid and base are completely neutralized at the equivalence point.