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

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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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)
Annette and Marilyn are given four reactions involving acids and bases. A dark arrow facing left (B -->) means the reaction favours the reactants. A dark arrow facing right ( Products L(aq) + HM(aq) HM(aq) +R (aq) HN(aq) + M¯(aq) HL(aq) + N(aq) Based on this information, the girls determine the correct list of BASES from strongest to weakest as: a. R¯(aq) L-(aq) N-(aq) M-(aq) b. N-(aq) M-(aq) R-(aq) L¯(aq) c. L'(aq) R-(aq) M-(aq) N-(aq) d. M (aq) N-(aq) R (aq) L (aq)
Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH, COОН(aq)+NaOH(aq) — СH, СОО" (аq) + H,О1) + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added. pH = Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
Determine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.
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)
Hippuric acid (HC3H&NO3), found in horse urine. Calculate the pH of a 0.250 M hippuric acid solution in water, if 0.155 M potassium hippurate salt, KC9H&NO3, was added. HC,H3NO3 (aq) + H20 (l) = H30*(aq) + C9H3NO3 *(aq) Ка = 2.40 x 10-4
Chemistry (Part -3) =============
The hydroxide ion concentration of an aqueous solution of 0.490 M acetylsalicylic acid (aspirin), HC,H;04. is [OH] = |M.
Adding acid to the buffer, NH3-NH4*, will produce this (net ionic) reaction: H*(aq) +OH(aq)=H₂O(1) H*(aq)+NH4*(aq) NH3(aq)+H₂(g) O H*(aq) + NH4+ (aq)=NH5²+ (aq) O H*(aq)+NH3(aq)=NH4+ (aq)
2. Dr. Dahm has prepared 250 mL of a acetate buffer which contains 0.1 mol of acetic acid (CH₂COOH) and 0.15 moles of acetate (CH₂COO). Determine the initial pH. If he then adds 0.025 moles of H* calculate the new pH. Ka = 1.8 × 10³ CH₂COOH(aq) + H₂O CH₂COO (aq) + HO (aq) 3. Dr. Dahm makes a second acetate buffer exactly the same way as in #2, but he then adds 15 mL of 0.50 M NaOH calculate the new pH.
This is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid? The reaction is: H3PO4 (aq) + 3 NaOH (aq) → Na3PO4 (aq) + 3 H2O (l)