Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate the pHpH at the equivalence point for titrating 0.240 MM solutions of each of the following bases with 0.240 MHBrMHBr.
sodium hydroxide (NaOH)(NaOH)
Express your answer using two decimal places.
pH=
hydroxylamine (NH2OH)(NH2OH)
Express your answer using two decimal places.
pH=
aniline (C6H5NH2)(C6H5NH2)
Express your answer using two decimal places.
pH=
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- 5. You use a 0.1380 M HCI to standardize an NaOH solution. The burets below show initial and final volume readings for the titration to the perfect endpoint. Calculate the appropriate volume ratio (Va/Vb or Vb/Va ratio) and the [NaOH]. Acid Buret Reading (mL) initial final cumpasın INHI IN ||| Base Buret Reading (mL) initial final ייייייי |||||arrow_forward+ pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as HA (aq) → H¹ (aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base is added, the base will react with H+, reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into H+ and A™. In both instances. [H] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: A] pH =pK₂ +log HA ▼ Part A pH = What is the pH of a buffer prepared by adding 0.607 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K₁ of HA is 5.66 x 10-7 Express the pH numerically to three…arrow_forwardCalculate the pH for each of the cases in the titration of 35.0 mL of 0.140 M LiOH(aq) with 0.140 M HBr(aq). Note: Enter your answers with two decimal places. before addition of any HBr: after addition of 25.5 mL HBr: after addition of 42.5 mL HBr: after addition of 13.5 mL HBr: after addition of 35.0 mL HBr: after addition of 50.0 mL HBr:arrow_forward
- Calculate the pH for each of the cases in the titration of 35.0 mL of 0.170 M LiOH(aq) with 0.170 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCI: after addition of 21.5 mL HC1: after addition of 45.5 mL HCl: after addition of 13.5 mL HCl: after addition of 35.0 mL HCl: after addition of 50.0 mL HC1: []arrow_forwardBuffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 105 mL of a buffer that is 0.260 M in both benzoic acid (CH₂COOH) and its conjugate base (CH₂COO¯). Calculate the maximum volume of 0.270M HCl that can be added to the buffer before its buffering capacity is lost. volume: mLarrow_forwardA 10.0mL solution of 0.720 M NH3 is titrated with a 0.240 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00mL, 10.0mL, 30.0mL, and 40.0mL. Be sure your answer has the correct number of significant digits. 0.00 mL added, pH = 10.0 mL added, pH = 30.0 mL added, pH = 40.0 mL added, pH =arrow_forward
- Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 2.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-What is the pH of the solution?arrow_forwardA chemist titrates 90.0 mL of a 0.2182M acetic acid (HCH3CO₂) solution with 0.8569M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K of acetic acid is 4.76. 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 = 0 X 3 ?arrow_forwardCalculate the pH for each point in the titration of 25.0 mL of 0.250 M pyridine, C,H,N(aq), with 0.250 M HBr(aq). pH before the addition of any HBr: pH after the addition of 12.5 mL HBr: pH after the addition of 24.0 mL HBr: pH after the addition of 25.0 mL HBr: pH after the addition of 32.0 mL HBr:arrow_forward
- The p?b values for the dibasic base B are p?b1=2.10 and p?b2=7.34. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.60 M B(aq) solution with 0.60 M HCl(aq). What is the pH before addition of any HCl? What is the pH after addition of 25.0 mL HCl? What is the pH after addition of 50.0 mL HCl? What is the pH after addition of 75.0 mL HCl? What is the pH after addition of 100.0 mL HCl?arrow_forwardCalculate the pH for each of the cases in the titration of 25.0 mL of 1.25 M pyridine, C5H5N(aq) with 0.250 M HBr(aq) at 25°C. The Kb of pyridine is 1.7×10−9. Report all your answers to 2 decimal places. Before the addition of any HBr: After the addition of 10.0 mL of HBr: After the addition of 62.5 mL of HBr: After the addition of 125.0 mL of HBr: After the addition of 135.0 mL of HBr:arrow_forward0 The pK, values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.67. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.60 M B(aq) solution with 0.60 M HCl(aq). What is the pH before addition of any HCI? What is the pH after addition of 25.0 mL HC1? What is the pH after addition of 50.0 mL HC1? What is the pH after addition of 75.0 mL HC1? What is the pH after addition of 100.0 mL HC1? pH = pH pH = pH = pH = 12.76 11.9 9.2 6.33 1.4 Incorrectarrow_forward
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