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17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.

17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.

Chemistry
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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
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17.46 parts d,e,f
DAExercises 761 strong acid g of the ti- ng acid. (c) which acid 17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated with tsl0.200 M NaOH solution. Calculate the pH of the solu- tion after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL. 17.44 A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M ere are both HCIO4 solution. Calculate the pH after the following vol- umes of acid have been added: (a) 20.0 mL, (b) 23.0 mL, (c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL. 17.45 A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is ti- trated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (a) 0 mL, (b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL. 17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL. bile 17.47 Calculate the pH at the equivalence point for titrating H;COOH(aq) 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) sodium hydroxide (NaOH), (b) hydroxylamine A (NH2OH), (c) aniline (C,H5NH2). atements con- 17.48 Calculate the pH at the equivalence point in titrating 0.100 ed to reach the 103. M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2), (c) benzoic acid (C,HsCOOH). HNO, titration alence point in Solubility Equilibria and Factors Affecting Solubility (Sections 17.4 and 17.5) ndicator for both 17.49 For each statement, indicate whether it is true or false. (a) The solubility of a slightly soluble salt can be expressed in units of moles per liter. statements con- rue or false. (b) The solubility product of a slightly soluble salt is simply the square of the solubility. (c) The solubility of a slightly soluble salt is independent of the presence of a common ion. (d) The solubility product of a slightly soluble salt is inde- pendent of the presence of a common ion. titrations will be entially the same dicator for both and MZ2, is the same, 4 x 10 mol/L. (a) Which has the larger numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M²*? (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+? 17.50 The solubility of two slightly soluble salts of M²*, MA ach of the following HCO3 titrated with I titrated with HBr. of each of the fol- H 7: (a) formic acid oxide titrated with th nitric acid. 17.51 Write the expression for the solubility-product con- stant for each of the following ionic compounds: Agl, thymol blue has two l generally be more hase? True or false: "solubility" and "solubility-product con- na number for a given compound. (b) Write WNI product constant for each UntOH), and SrSO4, Fe(OH)2, and Hg,Br2.
Transcribed Image Text:DAExercises 761 strong acid g of the ti- ng acid. (c) which acid 17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated with tsl0.200 M NaOH solution. Calculate the pH of the solu- tion after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL. 17.44 A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M ere are both HCIO4 solution. Calculate the pH after the following vol- umes of acid have been added: (a) 20.0 mL, (b) 23.0 mL, (c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL. 17.45 A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is ti- trated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (a) 0 mL, (b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL. 17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL. bile 17.47 Calculate the pH at the equivalence point for titrating H;COOH(aq) 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) sodium hydroxide (NaOH), (b) hydroxylamine A (NH2OH), (c) aniline (C,H5NH2). atements con- 17.48 Calculate the pH at the equivalence point in titrating 0.100 ed to reach the 103. M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2), (c) benzoic acid (C,HsCOOH). HNO, titration alence point in Solubility Equilibria and Factors Affecting Solubility (Sections 17.4 and 17.5) ndicator for both 17.49 For each statement, indicate whether it is true or false. (a) The solubility of a slightly soluble salt can be expressed in units of moles per liter. statements con- rue or false. (b) The solubility product of a slightly soluble salt is simply the square of the solubility. (c) The solubility of a slightly soluble salt is independent of the presence of a common ion. (d) The solubility product of a slightly soluble salt is inde- pendent of the presence of a common ion. titrations will be entially the same dicator for both and MZ2, is the same, 4 x 10 mol/L. (a) Which has the larger numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M²*? (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+? 17.50 The solubility of two slightly soluble salts of M²*, MA ach of the following HCO3 titrated with I titrated with HBr. of each of the fol- H 7: (a) formic acid oxide titrated with th nitric acid. 17.51 Write the expression for the solubility-product con- stant for each of the following ionic compounds: Agl, thymol blue has two l generally be more hase? True or false: "solubility" and "solubility-product con- na number for a given compound. (b) Write WNI product constant for each UntOH), and SrSO4, Fe(OH)2, and Hg,Br2.
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