A 45.60-mL sample of a 0.476 M solution of acetic acid (HC2H3O2) which is a weak acid with an acid ionization constant of 1.70 X10-5 at 25°C is being titrated by a 0.652 M solution of NaOH which is a strong base. Calculate the pH at the equivalence point. HC2H3O2(aq) + H2O(L) = C2H3O2° (aq) + H3O* (aq) 8.87 8.40 9.43 9.10

A 45.60-mL sample of a 0.476 M solution of acetic acid (HC2H3O2) which is a weak acid with an acid ionization constant of 1.70 X10-5 at 25°C is being titrated by a 0.652 M solution of NaOH which is a strong base. Calculate the pH at the equivalence point. HC2H3O2(aq) + H2O(L) = C2H3O2° (aq) + H3O* (aq) 8.87 8.40 9.43 9.10

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

A buffer solution contains 0.35 mol of arsenous acid (H3ASO3) and 0.62 mol of sodium dihydrogen arsenite (NaH₂AsO 3) in 4.40 L. The K₂ of arsenous acid (H3ASO3) is K₂ = 5.1e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.22 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.18 mol of HI? (assume no volume change) PH =
You prepare a MOPS buffer by adding 0.10 mol MOPS to water then adding 0.040 molNaOH and diluting to a final volume of 500. mL.Calculate the pH of this buffer C7H14NO3SOH (aq) + NaOH (aq) → C7H14NO3SO− (aq) + Na+ (aq) + H2O (l)
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
Calculate the pH during the titration of 20.0 mL of 0.1000 M methylamine, (CH3)NH2(aq) with 0.2000 M HCI(aq) after 3.47 mL of the acid have been added. Kb of methylamine = 3.6 * 10^-4.
What is the pH of the buffer containing 0.025 moles of sodium acetate and 0.030 mole of acetic acid? KaHAc = 8x10-5 CH3COOH (aq) + H2O(l) <-------------> H3O+(aq) + CH3COO-(aq) Calculate the pH of the buffer solution.
Calculate the pH at the equivalence point in titrating 0.066 M solutions of each of the following with 0.061 M NAOH. (a) periodic acid (HIO4) pH = (b) benzoic acid (HC;H502), K, 6.3e-05 pH = (c) acetic acid (HC2H302), K - 1.8e-05 pH -
Determine the volume in mL of 0.233 M KOH(aq) needed to reach the equivalence (stoichiometric) point in the titration of 28.32 mL of 0.117 M HClO(aq). The Ka of HClO is 3.0 x 10-8.
How to calculate the pH of a buffer solution 1) Calculate the pH of a solution prepared by dissolving 1.45 g of sodium acetate, CH3COONa, in 53.5 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. pH =
Acid Ka HF 6.7 x 10^-4 HC2H3O2 1.8 x 10^-5 A student titrated 50.0mL of 0.100 M HC2H3O2 with 0.100 M NaOH(aq), calculate the pH of the solution at the equivalence point.
A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff: A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte. B. pH of the resulting solution at the equivalence point. C. pH of the resulting solution at 5.0 ml added titrant beyond the equivalence point.
The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other hall still remains unreacted if 0.360 moles of a monoprotic weak acid (K, = 4.8 x 10^-5 ) is titrated with NaOH, what is the pH of the solution at the half -equivalence point? pH =
A 1.32 L1.32 L buffer solution consists of 0.303 M0.303 M propanoic acid, C2H5COOH and 0.193 M0.193 M sodium propanoate, C2H5COONa. Calculate the pH of the solution after the addition of 0.071 mol HCl0.071 mol HCl. The ?a�a of propanoic acid is 1.34×10−51.34×10−5.