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17.90 A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 30.0 mL of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After 15.0 mL of base had been added in the titration, the pH was found to be 6.50. What is the K, for the un- known acid?

17.90 A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 30.0 mL of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After 15.0 mL of base had been added in the titration, the pH was found to be 6.50. What is the K, for the un- known acid?

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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
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17.90
eof 0.1687 g of dissolved in 25.0 ml of NAOH. The acid requi equivalence point. (a) (b) After 7.25 ml of ba the pH was found to W known acid? 17.92 Mathematically prove the water, water is too acidic, seashells (which ate prin- Alcium carbonate, CaCO,). Calculate the the raindrop is 1.0 × 10-S M. 17.88 Two buffers are prepared by adding an equal number 17.87 Equal quantities of 0.010 M solutions of an acid HA and a 17.86 The acid-base indicator bromcresol green is a weak acid, stant for the reaction between HA and B? (c) What is the 17.85 Furoic acid (HC5H3O3) has a K, value of 6.76 x 10 at The yellow acid and blue base forms of the indicator are the total volume to 125 mL, (c) a solution prepared by add- tion, (b) a Solution formed by mixing 30.0 mL of 0.250 M ate (NaC5H3O3) to enough water to form 0.250 L of solu- by adding 25.0 g of furoic acid and 30.0 g of sodium furo- 25 °C. Calculate the pH at 25 °C of (a) a solution formed HC5H3O3 and 20.0 mL of 0.22 M NAC3H3O3 and diluting a pH of 5.60, assuming that the sum of all three species in and carbonate ion (CO-) that are in a raindrop that has concentrations of carbonic acid, bicarbonate ion (HC0;) 15×101 b K dto initiate the cipally Ia expression for the reaction between HA and B. (b) If K, for HA is 8.0 × 105, what is the value of the equilibrium con- base B are mixed. The pH of the resulting solution is 9.2. present in equal concentrations in a solution when the pH is 4.68. What is the pK, for bromcresol green? ing 50.0 mL of 1.65 M NaOH solution to 0.500 L of 0.0850 M a titration of a weak ae ume of added base is h alence point) is equal 17.93 A weak monoprotic requires 50.0 ml. of t alence point. After 2 solution is 3.62. Esti 17.94 What is the pH of NaOH, 0.25 mol Na and diluting to 1.00 17.95 Suppose you want for Metallic Elements HC5H3O3. calls for a pH 6.50 which you are wc H2A (Ka1 = 2 × 1 salts. You have ava ing several metal lons is treated wes 1.0 M solution of should be added 6.50? (Ignore any Atate forms. The pHis adijusted to ba Write the chemical equation and equilibrium-constant through. Agan, no precigitae t Aon is then adjusted to about & ugh. This time a precipitate foms ution is treated with (NH-HRO Thich of these metal cations are e 17.96 How many micr be added to 25.C [CH;CH(OH)C@ pH = 3.75? value of Kp for B? 17.97 Lead(II) carbon passivating lay= for PBCO3 is 7 a saturated sol of moles of formic acid (HCOOH) and sodium formate (HCOONA) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. (a) Calculate the pH of each buffer. (b) Which buf- fer will have the greater buffer capacity? (c) Calculate the change in pH for each buffer upon the addition of 1.0 mL of 1.00 M HCI. (d) Calculate the change in pH for each buf- fer upon the addition of 10 mL of 1.00 M HCI. finitely absent: AP , Na, Ag Me concentratiorm (c) Will the sC is entirely soluble in water Oh pH is lowered of lead ions in a precipitate forms. Aftr the 1, the pH is adjusted to about la lead(II) carbc limit? 17.98 For each pai which has f precipitate again forms. Ate mitate, the pH is adjusted t a o precipitate forms. N raija n of (NH,),HPO;. The remai w color in a flame test(se i observations, which ofthe 17.89 A biochemist needs 750 mL of an acetic acid-sodium acetate buffer with pH 4.50. Solid sodium acetate (b) PbCO3 Ag,SO4. (CH3COONA) and glacial acetic acid (CH3COOH) are available. Glacial acetic acid is 99% CH3COOH by mass and has a density of 1.05 g/mL. If the buffer is to be 0.15 M in CH3COOH, how many grams of CH3COONa and how many milliliters of glacial acetic acid must be used? 17.99 The solubil molar solu the acid-b= expressior constant E ight be present, which a hich are definitely absent CACO3(s) dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 30.0 mL of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After 15.0 mL of base had been added in the titration, the pH was found to be 6 50. What is the K, for the un- known acid? tosiEN pur ON/PO ualitative analysis procedie Countered (a) Zr* 2nd 1.90 A sample of 0.2140 g of an unknown monoprotic acid was (c) If we and OH (M and K (d mture might be sepuate each of the folloming D'and Co and x100 shution isslowly addedto0 Min Ca and 0.30 M orecipitate first: CasoK
Transcribed Image Text:eof 0.1687 g of dissolved in 25.0 ml of NAOH. The acid requi equivalence point. (a) (b) After 7.25 ml of ba the pH was found to W known acid? 17.92 Mathematically prove the water, water is too acidic, seashells (which ate prin- Alcium carbonate, CaCO,). Calculate the the raindrop is 1.0 × 10-S M. 17.88 Two buffers are prepared by adding an equal number 17.87 Equal quantities of 0.010 M solutions of an acid HA and a 17.86 The acid-base indicator bromcresol green is a weak acid, stant for the reaction between HA and B? (c) What is the 17.85 Furoic acid (HC5H3O3) has a K, value of 6.76 x 10 at The yellow acid and blue base forms of the indicator are the total volume to 125 mL, (c) a solution prepared by add- tion, (b) a Solution formed by mixing 30.0 mL of 0.250 M ate (NaC5H3O3) to enough water to form 0.250 L of solu- by adding 25.0 g of furoic acid and 30.0 g of sodium furo- 25 °C. Calculate the pH at 25 °C of (a) a solution formed HC5H3O3 and 20.0 mL of 0.22 M NAC3H3O3 and diluting a pH of 5.60, assuming that the sum of all three species in and carbonate ion (CO-) that are in a raindrop that has concentrations of carbonic acid, bicarbonate ion (HC0;) 15×101 b K dto initiate the cipally Ia expression for the reaction between HA and B. (b) If K, for HA is 8.0 × 105, what is the value of the equilibrium con- base B are mixed. The pH of the resulting solution is 9.2. present in equal concentrations in a solution when the pH is 4.68. What is the pK, for bromcresol green? ing 50.0 mL of 1.65 M NaOH solution to 0.500 L of 0.0850 M a titration of a weak ae ume of added base is h alence point) is equal 17.93 A weak monoprotic requires 50.0 ml. of t alence point. After 2 solution is 3.62. Esti 17.94 What is the pH of NaOH, 0.25 mol Na and diluting to 1.00 17.95 Suppose you want for Metallic Elements HC5H3O3. calls for a pH 6.50 which you are wc H2A (Ka1 = 2 × 1 salts. You have ava ing several metal lons is treated wes 1.0 M solution of should be added 6.50? (Ignore any Atate forms. The pHis adijusted to ba Write the chemical equation and equilibrium-constant through. Agan, no precigitae t Aon is then adjusted to about & ugh. This time a precipitate foms ution is treated with (NH-HRO Thich of these metal cations are e 17.96 How many micr be added to 25.C [CH;CH(OH)C@ pH = 3.75? value of Kp for B? 17.97 Lead(II) carbon passivating lay= for PBCO3 is 7 a saturated sol of moles of formic acid (HCOOH) and sodium formate (HCOONA) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. (a) Calculate the pH of each buffer. (b) Which buf- fer will have the greater buffer capacity? (c) Calculate the change in pH for each buffer upon the addition of 1.0 mL of 1.00 M HCI. (d) Calculate the change in pH for each buf- fer upon the addition of 10 mL of 1.00 M HCI. finitely absent: AP , Na, Ag Me concentratiorm (c) Will the sC is entirely soluble in water Oh pH is lowered of lead ions in a precipitate forms. Aftr the 1, the pH is adjusted to about la lead(II) carbc limit? 17.98 For each pai which has f precipitate again forms. Ate mitate, the pH is adjusted t a o precipitate forms. N raija n of (NH,),HPO;. The remai w color in a flame test(se i observations, which ofthe 17.89 A biochemist needs 750 mL of an acetic acid-sodium acetate buffer with pH 4.50. Solid sodium acetate (b) PbCO3 Ag,SO4. (CH3COONA) and glacial acetic acid (CH3COOH) are available. Glacial acetic acid is 99% CH3COOH by mass and has a density of 1.05 g/mL. If the buffer is to be 0.15 M in CH3COOH, how many grams of CH3COONa and how many milliliters of glacial acetic acid must be used? 17.99 The solubil molar solu the acid-b= expressior constant E ight be present, which a hich are definitely absent CACO3(s) dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 30.0 mL of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After 15.0 mL of base had been added in the titration, the pH was found to be 6 50. What is the K, for the un- known acid? tosiEN pur ON/PO ualitative analysis procedie Countered (a) Zr* 2nd 1.90 A sample of 0.2140 g of an unknown monoprotic acid was (c) If we and OH (M and K (d mture might be sepuate each of the folloming D'and Co and x100 shution isslowly addedto0 Min Ca and 0.30 M orecipitate first: CasoK
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