Which of the following solution(s) would be a buffer? Select all that apply. 100.0 mL of a solution that contains 0.100 M benzoic acid and 0.100M potassium benzoate 100.0 mL of a 0.100 M propanoic acid to which 50.0 mL of 0.100 M sodium hydroxide has been ádded 100.0 mL of a 0.100 M formic acid solution 100.0 mL of a 0.100 M solution of acetic acid in which 0.100 g of sodium acetate is dissolved 100.0 mL of a solution that contains 0.100 M hydrochloric acid and 0.100 M sodium chloride

Which of the following solution(s) would be a buffer? Select all that apply. 100.0 mL of a solution that contains 0.100 M benzoic acid and 0.100M potassium benzoate 100.0 mL of a 0.100 M propanoic acid to which 50.0 mL of 0.100 M sodium hydroxide has been ádded 100.0 mL of a 0.100 M formic acid solution 100.0 mL of a 0.100 M solution of acetic acid in which 0.100 g of sodium acetate is dissolved 100.0 mL of a solution that contains 0.100 M hydrochloric acid and 0.100 M sodium chloride

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.30QAP

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A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL of the buffer. (b) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL pure (pH 7.00) water.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
A buffer solution was prepared by adding 4.95 g sodium acetate to 250. mL of 0.150-M acetic acid. What ions and molecules are present in the solution? List them in order of decreasing concentration. Calculate the pH of the buffer solution. Calculate the pH of 100. mL of the buffer solution if you add 80. mg NaOH. (Assume negligible change in volume.) Write a net ionic equation for the reaction that occurs to change the pH.
Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.) a. Calculate the pH of this solution. b. Calculate the pH after 0.10 mole of HCl has been added to the original solution. Assume no volume change on addition of HCl. c. Calculate the pH after 0.20 mole of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0
Predict whether 1.0 L of each solution is a buffer: (a) equal amounts (mol) of HCl and NaCl; (b) equal amounts (mol) of KOH and KCl. Explain each prediction.
Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak base pyridine is titrated with HCl. (b) Formic acid is titrated with NaOH. (c) Ethylenediamine, a weak diprotic base, is titrated with HCl. Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that o few indicators hove color changes over two different pH ranges.
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
A student must make a buffer solution with a pH of 7.00.7.00. Determine which weak acid is the best option to make a buffer at the specified pH. acetic acid, ?a=1.75×10−5,�a=1.75×10−5, 5.00 M propionic acid, ?a=1.34×10−5,�a=1.34×10−5, 3.00 M ammonium citrate, ?a=4.06×10−7,�a=4.06×10−7, 2.00 M sodium dihydrogen phosphate monohydrate, ?a=6.23×10−8,�a=6.23×10−8, 2.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. sodium acetate trihydrate, CH3COONa⋅3H2OCH3COONa⋅3H2O disodium hydrogen phosphate heptahydrate, Na2HPO4⋅7H2ONa2HPO4⋅7H2O sodium propionate, CH3CH2COONaCH3CH2COONa sodium citrate dihydrate, C6H5O7Na3⋅2H2OC6H5O7Na3⋅2H2O The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 7.00? mass = g Based on this information, what…