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11 ml 6. Which of following could be used to make a buffer with sulfurous acid,...
Which of following could be used to make a buffer with sulfurous acid, H2SO3? O sulfurous acid cannot make a buffer O sulfate ion hydrogen sulfite (bisulfite) ion O sulfite ion
IT L. Na SO d. NH.CI 6) Which of the following is not a buffer sy equal concentrations of fluoride ion and hydrofluoric acid. c. chloride ion and hydrochloric acid. d. owing is not a buffer system? A solution containing roughly phosphate ion and monophosphate ion. sulfite ion and bisulfite ion. 7 .
A buffer solution is prepared by mixing 15.5 mL of 0.0229 M pyridinium chloride with 73.8 mL of 0.888 M pyridine. A table of pKa values can be found here. 1. Calculate the pH (to two decimal places) of this solution. Assume the 5% approximation is valid and that the volumes are additive. Tries 0/13 2. Calculate the pH (to two decimal places) of the buffer solution after the addition of 8.26 g of pyridine (C5H5N) to the buffer solution...
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 2.10? The K for the acids are given in parentheses. Hydrogen phosphate/phosphate (Kg = 4.2 x 10-13) Ammonium/ammonia (K- 5.8 10-10) Benzoic acid / benzoate (K, -6.3 x 10-5) Chlorous acid / chlorite (K = 1.1x102) Hydrofluoric acid / fluoride (K, = 6.6 x 10-4)
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 3.987 The K, for the acids are given in parentheses. Hydrogen phosphate / phosphate (K, -4.2 x 10-13) Ammonium / ammonia (K, - 5.8 x 10-19 Hydrofluoric acid / fluoride (K. = 6.6 x 10-4) Benzoic acid / benzoate (K, -6.3 * 10-5) Chlorous acid / chlorite (K, -1.1 x 104
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 2.10? The Kfor the acids are given in parentheses. Chlorous acid / chlorite (Ka = 1.1 10-2) Benzoic acid / benzoate (K, -6.3 * 10-5) O Hydrofluoric acid / fluoride (Ka = 6.6 x 10-4) Hydrogen phosphate / phosphate (Kg = 4.2 x 10-13) Ammonium / ammonia (K, -5.8 * 10-10)
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 9.877 The K, for the acids are given in parentheses. Hydrofluoric acid / fluoride (K. = 6.6 x 104) Benzoic acid / benzoate (K, -6.3 x 10-5) Chlorous acid / chlorite (K, - 1.1*102) Hydrogen phosphate/phosphate (K, -4.2 x 10-13) Ammonium / ammonia (K = 5.8 x 10-19
Determine the pH of the solution (to 2 decimal points) after the addition of 11.7 mL of 6.14 M hydrochloric acid (HCl) to 624 mL of 0.735 M phenylamine (aniline) (C6H5NH2). Assume that the volumes are additive and that the 5% approximation is valid. A table of pKa values can be found here. Table 10.2: pKa and pKb values at 25 °C for some common weak acids and their conjugate bases Acid name trifluoroacetic acid trichloroacetic acid oxalic acid dichloroacetic...
A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K = 1.34 x 10-6, 3.00 M O sodium bisulfate monohydrate, K = 1.20 x 10,3.00 M acetic acid, K, = 1.75 x 10-6, 5.00 M formic acid, K, = 1.77 x 10 , 2.00 M Determine which conjugate base is the best option to make a buffer at...
Explain why each of following aqueous mixtures could or could not produce a buffer. In each case where the solution is a buffer, name the common ion and calculate the pH. (Use the Ka and Kb values) a) 100 mL solution containing 0.20 M NH4Cl and 0.20 M NH3 b) 100 mL solution containing 0.20 M KOH and H2O c) 100 mL solution containing 0.10 M H2SO3 and 0.15 M NaHSO