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- The Ka for four acids are H₂CO3: 4.5 x 10-7, HCO₂H: 1.8 x 10-4, H3C6H₂O7 : 7.1 x 104, HCN: 6.2 x 10-10. If the pH's of 0.50 mol/L solutions of these acids were measured and they were placed in order from highest pH to lowest pH the results would be which of the following? A. HCN, H3C6H5O7, HCO₂H, H₂CO3 B. H₂CO3, HCN, H3C6H5O7, HCO₂H C. HCN, H₂CO3, HCO₂H, H3C6H₂O7 D. H³CH,O₁, HCO₂H, H₂CO3, HCN E. HCN, H₂CO3, H3C6H5O7, HCO₂HPerform the following to determine the pH of a lactic acid solution. Write the acid/base reaction between lactic acid, HC3H5O3 and water. Write an equilibrium expression for the reaction between lactic acid and water. If the Ka of lactic acid is 3.18 x 10-4, what is the pH of a 0.500 M solution of lactic acid?Determine the pH of a 0.095 mol/L HIO4 solution if the Ka = 1.29 x 10-2
- What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization constant is 8.97 x 10-7?Consider the following data on some weak acids and weak bases: name hydrocyanic acid acid nitrous acid 0.1 M NH4CI solution 0.1 M KBr 0.1 M CH3NH3Br 0.1 M KNO2 formula HCN Ka 4.9 × 10 HNO₂ 4.5 x 10 X - 10 -4 pH Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, '2' next to the solution that will have the next lowest pH, and so on. choose one 1 (lowest) choose one choose one name Ś base ammonia formula NH₂ Kb 1.8 × 10 -5 -4 methylamine CH3NH₂| 4.4 × 10Calculate the pH of each of the following buffered solutions. Ka (HC2H3O2) = 1.8 × 10-5 1. 0.11 M acetic acid/0.26 M sodium acetate pH = 2. 0.26 M acetic acid/0.11 M sodium acetate pH = 3. 0.020 M acetic acid/0.15 M sodium acetate pH = 4. 0.15 M acetic acid/0.020 M sodium acetate pH =
- Determine the hydroxide ion concentration and pH of 0.0942 M hypochlorous acid solution. Ka = 2.85 x 10-8Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10-4.Calculate the pH of a 0.50 M solution of oxalic acid (H2C2O4) given the equilibrium constants below. Ka1 = 5.9 × 10–2 Ka2 = 6.4 × 10–5 Enter your response in pH units to the nearest 0.01.