Calculate the pOH of a solution that contains 3.9 × 10-4 M H3O+ at 25 °C.9.5910.590.593.414.41

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Answered: Calculate the pOH of a solution that…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.46QE

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Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa values): 1. 0.01 M HBr 2. 0.00005 M HBr 3. 0.00002 МКОН 4. 0.01 M CH,COOH 5. 0.00001 M CH,COOH 6. 0.01 M HIO, 7. 0.01 M pyridine Calculate the pH of the following solutions: 1. 0.01 M NAHS 2. 0.005 M NaН.РО, 3. 0.005 M Na,HPO, 4. 0.005 M Na PO, 5. 0.1 ΜΝΗ,CN Calculate the pH of the following buffer solutions: 1. 1.7 g/L of NH, and 5.35 g/L of NH,Cl. 2. 50 mL of 1 M CH,COONA and 1 L 0.1 M CH,COOH. 3. 50 mL of 1 M NaOH and 1 L 0.1 M CH,COOH. 4. 10 mL 0.1 H,PO, + 25 mL 0.1 NaOH 5. 10 mL 0.1 H,PO, + 25 mL 0.1 Na,PO, 6. A buffer solution pH=5.00 contains 0.01 M CH,COOH. Calculate the concentration of sodium acetate it contains. 7. What weight of NH,Cl should be added to 1 L of 0.1 M NH, solution to get pH=9.00?
Swimming pool disinfectants produce hypochlorous acid upon dissolution. The weak acid ionizes as follows: HClO (aq) ⇄ H+ (aq) + ClO‒ (aq) Ka=3.0 x 10 ‒8 As strong oxidizing agents, both acid and its conjugate base kill bacteria. However, too high [HClO] is irritating to swimmers’ eyes and too high [ClO‒] will cause the ions to decompose in sunlight. The recommended pH to circumvent both problems is 7.8. Determine the ratio of the weak acid and its conjugate base at this pH.
Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH? -117 Hypoiodous acid (HOI), K = 2.3 x 10 Hypobromous acid (HOBr), K = 2.5 x 10 Lactic acid (HC₂H₂O₂), K = 1.3 x 10 Chlorous acid (HClO₂), K = 1.1 x 10²
1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.
The base protonation constant K, of allantoin (C4H,N,O,NH,) is 9.12 x 10 °. 9. 3 Calculate the pH of a 0.47 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = | ?
Calculate the pH and pOH of the following substances: 1. 0.3 M sulfuric acid (H2SO4) solution 2. 0.125 M potassium hydroxide (KOH) solution 3. 0.8 M hypochlorous acid (HCIO) solution (Ka = 2.9 x 10-8) 4. 0.5 M aniline (C6H5NH2) solution (Kb = 3.8 x 10-10)
Calculate the pH of the resulting solution if 31.0 mL of 0.310 M HCl(aq) is added to 41.0 mL of 0.310 M NaOH(aq). pH = Calculate the pH of the resulting solution if 31.0 mL of 0.310 M HCl(aq) is added to 21.0 mL of 0.410 M NaOH(aq). pH: = x10 TOOLS
What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is equal to 5.2 × 10–13 at 100.0 °C.
The base protonation constant K, of allantoin (C,H¸N,O,NH,) is 9.12 x 10 °. 4 3 Calculate the pH of a 0.46 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = || %D

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Calculate the pOH of a solution that contains 3.9 × 10¬4 M H3O† at 25 °C. 9.59 10.59 0.59 3.41 4.41