Harriet Rowki prepared 100.0 mL of 2.50 M H3BO3-NaH2BO3 buffer solution (pH = 8.50). The pKa value of H3BO3 is 9.24. A. Write the net ionic equation describing the buffer system. B. By writing the chemical reactions involved, show how the buffer system resists the drastic change in pH after adding 1 drop 0.100 M HCl or 1 drop 0.100 M of NaOH.

Harriet Rowki prepared 100.0 mL of 2.50 M H3BO3-NaH2BO3 buffer solution (pH = 8.50). The pKa value of H3BO3 is 9.24. A. Write the net ionic equation describing the buffer system. B. By writing the chemical reactions involved, show how the buffer system resists the drastic change in pH after adding 1 drop 0.100 M HCl or 1 drop 0.100 M of NaOH.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. b. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer. c. Calculate its pH.
10. What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate base? The pKa for the acid is 5.53.
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12.A buffer was prepared by mixing 65.0 mL of 0.179 M NaHSO3 with 90.0 mL of 0.150 M NazSO3. Ka = 6.4 x 108 a. Determine the pH of this buffer. b. If 0.005 mol of NaOH was added to this buffer, indicate whether the following values would decrease, increase, or remain the same. %3D i. Moles of NaHSO3 ii. Moles of NazS03 pK, value pH value ii. iv.
A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7. The relevant pKa value can be obtained from your textbook. What is the [HCO3-]/[CO32-] ratio in this buffer solution? What volume of 0.198 M NaHCO3 must be added to 765 mL of a 0.123 M Na2CO3 to obtain this pH? What volume of 0.089 M HCl must be added to 765 mL of 0.123 M Na2CO3 to obtain this pH?
A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.7. The relevant pKa value can be obtained from your textbook. What is the [HCO3-]/[CO32-] ratio in this buffer solution? What volume of 0.198 M NaHCO3 must be added to 765 mL of a 0.123 M Na2CO3 to obtain this pH? What volume of 0.089 M HCl must be added to 765 mL of 0.123 M Na2CO3 to obtain this pH? part 3 please
Strong base is dissolved in 665 mL of 0.600 M weak acid (K₁ = 4.09 × 10−5) to make a buffer with a pH of 3.96. Assume that the volume remains constant when the base is added. HA(aq) + OH(aq) H,O(l) + A-(aq) Calculate the pKa value of the acid, and determine the number of moles of acid initially present. pK₂ = initial amount: When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A-] [HA] = How many moles of strong base were initially added? amount added: mol HA mol OH-
8. Calculate the volume of a 0.10 mol dm³ sodium ethanoate solution needed to be added to 1 dm³ of 0.10 mol dm³ ethanoic acid to produce a buffer solution with pH = 4.0. [pka for CH3COOH = 4.74]
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3. A buffer is prepared by adding 0.50 mol of acetic acid (HC₂H3O₂) and 0.75 mol of sodium acetate (NaC₂H302) to enough water to form 2.00L solution. (pKa for acetic acid is 4.74) Calculate the pH of the buffer.