In a laboratory experiment, the pH of a solution must be maintained at around 7.5. Which of the following buffer solutions will work best for this experiment? Explain briefly your reasoning. Buffer solution pka Phosphoric acid/ Dihydrogen phosphate (H,PO,/H,PO,) 2.18 Acetic acid/ acetate ion (HC,H,0,/C,H,0,) 4.76 Dihydrogen phosphate/ hydrogen phosphate (H,P0,7 HPO,) Boric acid/tetrahydroxyborate (B(OH),/ [B(OH),1) 7.20 8.98

In a laboratory experiment, the pH of a solution must be maintained at around 7.5. Which of the following buffer solutions will work best for this experiment? Explain briefly your reasoning. Buffer solution pka Phosphoric acid/ Dihydrogen phosphate (H,PO,/H,PO,) 2.18 Acetic acid/ acetate ion (HC,H,0,/C,H,0,) 4.76 Dihydrogen phosphate/ hydrogen phosphate (H,P0,7 HPO,) Boric acid/tetrahydroxyborate (B(OH),/ [B(OH),1) 7.20 8.98

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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Unit 4: Lesson Indicators 138. According to the acid-base indicator table, what is the color of each of the following indicators in the solutions of given pH? a.) Phenolphthalein in a solution with a pH = 11.7. Titration Curves Use the following information to answer the next 5 questions. Titration of 50.0 mL of 0.130 mol/L sulfurous acid with 0.14 mol/L sodium hydroxide 14 13 12 11 10 9 8 17 6 5 4 3 2 0 0 10 20 30 40 50 80 60 70 90 100 110 120 130 140 150 160 170 180 NaOH (ML) 156. Label the first and second equivalence points on the graph. First EP pH: Second EP pH: First EP volume: Second EP volume: Species responsible for pH: Species responsible for pH: 157. Choose an appropriate indicator for each equivalence point. 42. Label the buffer region(s) on the graph
2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186
A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution if 0.11 mol of NaOH is added to 1.00 L of the solution? (Assume there is no volume change.) Round to 2 decimal places. Your Answer: Answer
A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 NEXT > The buffer was prepared by dissolving 21.5 g HC7H5O2 and 37.7 g of NaC7H5O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.178 0.880 - x 0 0.888 1 HC7H5O₂(aq) + 1.31 + x 21.5 +X 0.178 + x 37.7 -X H₂O(1) 0.888 + x 0.176 21.5-x H3O+ (aq) 0.261 37.7 + x + 0.880 0.176 - x C7H5O₂ (aq) RESET 1.31 0.261 + x
Identify the buffer system(s) - the conjugate acid-base pair(s)- present in a solution that contains equal molar amounts of the following: ???3(??????????) NaOH(sodiumhydroxide) H3PO4(phosphoricacid) NaH2PO4(sodiumdihydrogenphosphate) Group of answer choices HNO3 (nitric acid) and NaOH (sodium hydroxide) HNO3 (nitric acid) and H3PO4 (phosphoric acid) NaOH (sodium hydroxide) and NaH2PO4 (sodium dihyrdogen phosphate) NaH2PO4 (sodium dihyrdogen phosphate) and NaOH (sodium hydroxide) H3PO4 (phosphoric acid) and NaH2PO4 (sodium dihyrdogen phosphate) HNO3 (nitric acid) and NaH2PO4 (sodium dihyrdogen phosphate)
Can you help me with #2
Most carbonates are insoluble in water. Small concentrations of Mg2+ in tap water can react with bicarbonate to create scale deposits inside of tea kettles. a) Show the law of mass action for this interaction. b) Where does the bicarbonate come from in this example? c) Do you expect the solution to become slightly acidic, basic, or neutral due to this interaction? d) How will the molar solubility of magnesium bicarbonate to change if you were to place it into acidic conditions?
Which of the following aqueous solutions are good buffer systems?. 0.12 M potassium acetate + 0.20 M acetic acid 0.18 M nitrous acid + 0.18 M potassium nitrite 0.31 M ammonium bromide + 0.35 M ammonia 0.38 M hydrocyanic acid + 0.21 M potassium cyanide 0.24 M hydroiodic acid + 0.23 M sodium iodide
Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base are mixed in equimolar proportions? Acid NH4* (from ammonia) HC₂H3O2 (acetic acid) HF (hydrofluoric acid) CH3CH₂NH3 (from ethylamine) acetic acid. b) ethylamine c) ammonia d) hydrofluoric acid e) none Ka 5.69 10-10 1.75 10-5 6.810-4 2.12 10-11
Question 2 A buffer solution is prepared by mixing equal volumes of 1.0 M NH, and 1.0 M NH CI. How would adding solid KI to the buffer solution affect each of the following concentrations? [NH,] will [OH] will [NH,] will - How would adding HCl(aq) to the buffer solution affect each of the following concentrations? [NH,] wil [OH] wil ANH 1 m decrease increase remain constant
please answer both for a vote uofront. thanks (Please type answer no write by hend)