5-21. The pH of a finished water from a softening process is 10.74. What amount of 0.02000 N sulfuric acid, in milliliters, is required to neutralize 1.000 L of the finished water? Assume the buffering capacity is zero. 5-22. How many milliliters of 0.02000 N hydrochloric acid would be required to perform the neutralization in Problem 5-21?

5-21. The pH of a finished water from a softening process is 10.74. What amount of 0.02000 N sulfuric acid, in milliliters, is required to neutralize 1.000 L of the finished water? Assume the buffering capacity is zero. 5-22. How many milliliters of 0.02000 N hydrochloric acid would be required to perform the neutralization in Problem 5-21?

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 chemist titrates 100.0 mL of a 0.0714M nitrous acid (HNO,) solution with 0.3683M KOH solution at 25 °C. Calculate the pH at equivalence. The p K, of nitrous acid is 3.35. 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 KOH solution added. pH = |
Increasing acid strength You are making a buffer solution made from a weak acid, HA, and the sodium salt of the conjugate base, NaA. You want the buffer to have a pH approximately equal to 4.0, choose an acid from the list, and use a 0.350 M solution of the acid solution, and 30.0 g of the sodium salt 8. (NaA). Calculate the pH of the buffer. Table 13-2 | Values of K, for Some Common Monoprotic Acids Formula Name Value of K. HSO, HCIO, HC,H,CIO, Hydrogen sulfate ion Chlorous acid 12 x 10 12 x 10 135 X 10 7.2 x 10 4.0 x 104 18 X 10- Monochloracetic acid Hydrofluoric acid Nitrous acid Acetic acid Hydrated aluminum(I) lon Hypochlorous acid Hydrocyanic acid Ammonium lon Phenol HF HNO, HC,H,0, [ANH,O)J" HOCI 14 X 10 3.5 x 10- 62 x 10-10 5.6 X 10- 16 x 10 HCN NH," HOCH *The units of K, are customarily omitted.
You have a 18 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.35. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.03. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 18 mL sample.
What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.
Recently graduated from the ESST programme in UWI, you land a job as a technical officer in the EMA. A proposal to allow an industry to release hydrochloric acid into a small lake crosses your desk; the proposal can only be approved if the pH of the water in the lake will remain within the regulated pH range of 6 – 9 after the hydrochloric acid has been released. To assist the EMA in making their decision, the buffer capacity of the lake water is determined. Buffer capacity is a parameter similar to alkalinity, in that it indicates how much acid or base can be added to the water to achieve a pH change of 1 unit. (a) The buffer capacity of the lake is measured, and is found to be 7.95×10-4 mol/L. Given that the volume of the lake is 5.0×1010 m3, how many moles of H+can the lake absorb before the pH of the water drops by 1 pH unit?
Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO and combine them into a beaker. This is the buffer solution Measure out 50.0 mL of the buffer in part D (that you just made) and pour it into a clean beakerand add 2.0 mL of 1.0 M NaOH to it. What is the calculated/expected pH of this solution after the addition of the NaOH?
The pH of unbuffered water, such as rain, is decreasing consistently over time as atmospheric CO2 concentrations increase. a) What will be the atmospheric CO2 level (in ppm) when the pH of rain water reaches 5.50 at 25 °C? b) What would be the pH of buffered water (over CaCO3 limestone at 25 °C) at the CO2 level in part a)? c) Determine the concentrations of HCO3– and CO32– ions in the buffered water of part b) and then determine the alkalinity of the solution in ppm CaCO3.
Suppose you want to prepare a solution with a pH of 4.00 using acetic acid, CH3COOH, and sodium acetate, CH3CoOONa. What should the ratio of sodium acetate to acetic acid, CH3CO0-| : [CH3COOH], be in your buffer solution? Hint: The Ka for acetic acid is 1.8x105. 0.18:1 O 1.9:1 0.84:1 O 5.5:1 O 1:1
10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
Rainwater is slightly acidic due to dissolved CO₂. Use the following data to calculate the pH of unpolluted rainwater at 22.6°C: vol % in air of CO₂ = 0.063 vol%; solubility of CO2 in pure water at 22.6°C and 1.09 atm is 79.29 mL CO2 per 100 mL, K₁1 of H₂CO3 = 5.27x10-7. Express the pH with 2 decimals. You might have to solve a quadratic.
Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. H2NNH2(aq) +HNO3(aq) ⟶ [H2NNH3]+1(aq) + NO3-1(aq) 1. 4.80 2. 9.60 3. 4.70 4. 9.39 5. 3.22 6. 3.32
- Calculate the pH of a 1.00 L buffer solution containing 0.143 mol of acetic acid (HC₂H30₂) and 0.180 mol of sodium acetate (NaC₂H₂O₂). The Ka of acetic acid is 1.8 × 10-5. pH = Calculate the pH of the buffer solution after 0.0315 mol of HCl is added to the buffer. Assume the volume of the solution does not change. pH = Calculate the pH after 0.0315 mol of HCl is added to 1.00 L of pure water. pH =