1) Can the five percent approximation be applied in determining
the pH of the following solutions?
2.10×10-4 M citric acid pka 3.13
9.99×10-3 M phosphoric acid pka 2.12
3.19×10-1 M propylammonium ion pka 10.71
8.88×10-4 M diethylammonium ion pka 10.77
2) Calculate the pOH (to two decimal places) for the following: 1.95×10-3 M Na2O
1) Can the five percent approximation be applied in determining the pH of the following solutions?...
Determine the pH (to two decimal places) of the following solutions. If the 5% approximation is valid, use the assumption to compute pH. 8.72×10-3 M sodium hydrogen sulfate pKa hydrogen sulfate ion is 1.92 8.73×10-3 M trifluoroacetic acid pKa trifluoroacetic acid is 0.20 8.20×10-3 M ethylamine pKa ethylammonium ion is 10.87 2.51×10-1 M sodium nitrite pKa nitrous acid is 3.37
pKa Conjugate base Acid formula Conjugate base name Acid name F3CCOOH 0.20 F3ccoo trifluoroacetic acid trifluoroacetate ion 13.80 Cl3CCOOH 13.34 0.66 Cl3CCOO trichloroacetic acid trichloroacetate ion HOOCCOOH 1.23 HOOCCOO oxalic acid hydrogen oxalate ion 12.77 Cl2HCCOOH 12.70 dichloroacetic acid 1.30 Cl2HCCOO dichloroacetate ion H2SO3 12.23 1.77 HSO3 sulfurous acid hydrogen sulfite ion 1.92SO42- HSO4 hydrogen sulfate ion sulfate ion 12.08 HCIO2 1.95 CI02 chlorous acid chlorite ion 2.12 H2PO.4 phosphoric acid H3PO dihydrogen phosphate ion 11.88 CIH2CCOOH 2.87 CIH2CCOO 11.13...
Consider the following solutions: A) 1 M phosphoric acid (pKa 2.14) B) 1 M HCl C) 1 M acetic acid (Ka 1.74x10-5 M) D) 1 M formic acid (pKa 3.75) E) 1 M trimethylacetic acid (pKa 5.03) 1. Order these solutions from the lowest to the highest pH. 2. Order these solutions from the lowest to the highest pOH.
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 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...
Estimate to ±0.1 the pH value of the following solutions: 1. 0.043 M sodium hydrogen carbonate 2. 0.017 M sodium hydrogen tartrate Blood pH is regulated to stay within the narrow range of 7.35 to 7.45, making it slightly basic. Which form of the following molecules is predominant at pH 7.4 (draw formula in ChemDraw or ChemSketch with appropriate protons shown): 1. Pyridine 2. Ethylamine 3. Acetic acid 4. Citric acid 5. Ibuprofen (pKa =4.91) 6. Glycine 7. Amphetamine (pKa...
Determine the pH (to two decimal places) of the following solutions. A table of pKa values can be found here. If the 5% approximation is valid, use the assumption to compute pH. 6.80×10-3 M butanoic acid Tries 0/13 9.74×10-1 M formic acid Tries 0/13 8.47×10-3 M methylamine Tries 0/13 6.59×10-3 M triethylamine
Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion concentrations. Solution B: [OH–] = 2.56×10-4 M
Determine the pH (to two decimal places) of the following solutions. A table of pKa values can be found here. If the 5% approximation is valid, use the assumption to compute pH. 6.80×10-3 M butanoic acid Tries 0/13 9.74×10-1 M formic acid Tries 0/13 8.47×10-3 M methylamine Tries 0/13 6.59×10-3 M triethylamine
15.32. Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. a. [OH-] = 7.69 X 10 M b. [OH-] = 2.18 x 10-'M c. [H-] = 4.0 x 10-8 M d. [H+] = 3.56 X 10-4 M