17.46 parts d,e,f DAExercises761strong acidg of the ti-ng acid. (c)which acid17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated withtsl0.200 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 Mere are bothHCIO4 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 afterthe 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 with0.025 M HCI. Calculate the pH after the following volumesof titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.bile17.47 Calculate the pH at the equivalence point for titratingH;COOH(aq)0.200 M solutions of each of the following bases with 0.200M HBr: (a) sodium hydroxide (NaOH), (b) hydroxylamineA (NH2OH), (c) aniline (C,H5NH2).atements con-17.48 Calculate the pH at the equivalence point in titrating 0.100ed to reach the103.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, titrationalence point inSolubility Equilibria and Factors AffectingSolubility (Sections 17.4 and 17.5)ndicator for both17.49 For each statement, indicate whether it is true or false.(a) The solubility of a slightly soluble salt can be expressedin units of moles per liter.statements con-rue or false.(b) The solubility product of a slightly soluble salt is simplythe square of the solubility.(c) The solubility of a slightly soluble salt is independent ofthe 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 beentially the samedicator for bothand MZ2, is the same, 4 x 10 mol/L. (a) Which has thelarger numerical value for the solubility product constant?(b) In a saturated solution of each salt in water, which hasthe higher concentration of M²*? (c) If you added an equalvolume of a solution saturated in MA to one saturated inMZ2, what would be the equilibrium concentration of thecation, M2+?17.50 The solubility of two slightly soluble salts of M²*, MAach of the followingHCO3 titrated withI titrated with HBr.of each of the fol-H 7: (a) formic acidoxide titrated withth nitric acid.17.51 Write the expression for the solubility-product con-stant for each of the following ionic compounds: Agl,thymol blue has twol generally be morehase?True or false: "solubility" and "solubility-product con-na number for a given compound. (b) WriteWNI product constant for eachUntOH), andSrSO4, Fe(OH)2, and Hg,Br2.

Question

17.46 parts d,e,f DAExercises761strong acidg of the ti-ng acid. (c)which acid17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated withtsl0.200 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 Mere are bothHCIO4 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 afterthe 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 with0.025 M HCI. Calculate the pH after the following volumesof titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.bile17.47 Calculate the pH at the equivalence point for titratingH;COOH(aq)0.200 M solutions of each of the following bases with 0.200M HBr: (a) sodium hydroxide (NaOH), (b) hydroxylamineA (NH2OH), (c) aniline (C,H5NH2).atements con-17.48 Calculate the pH at the equivalence point in titrating 0.100ed to reach the103.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, titrationalence point inSolubility Equilibria and Factors AffectingSolubility (Sections 17.4 and 17.5)ndicator for both17.49 For each statement, indicate whether it is true or false.(a) The solubility of a slightly soluble salt can be expressedin units of moles per liter.statements con-rue or false.(b) The solubility product of a slightly soluble salt is simplythe square of the solubility.(c) The solubility of a slightly soluble salt is independent ofthe 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 beentially the samedicator for bothand MZ2, is the same, 4 x 10 mol/L. (a) Which has thelarger numerical value for the solubility product constant?(b) In a saturated solution of each salt in water, which hasthe higher concentration of M²*? (c) If you added an equalvolume of a solution saturated in MA to one saturated inMZ2, what would be the equilibrium concentration of thecation, M2+?17.50 The solubility of two slightly soluble salts of M²*, MAach of the followingHCO3 titrated withI titrated with HBr.of each of the fol-H 7: (a) formic acidoxide titrated withth nitric acid.17.51 Write the expression for the solubility-product con-stant for each of the following ionic compounds: Agl,thymol blue has twol generally be morehase?True or false: &#34;solubility&#34; and &#34;solubility-product con-na number for a given compound. (b) WriteWNI product constant for eachUntOH), andSrSO4, Fe(OH)2, and Hg,Br2.

Accepted Answer

d) 60.0 mL
Calculation of no. of mol of NH3:
nNH3=Molarity×Volume=0.050 mol/L×30.0×10-3L=0.0015 mol…

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.