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What is the significance of the Henderson-Hasselbalch equation in acid-base chemistry, and how does it relate to the pH of a solution?
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- An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1.The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2.Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the pH.3.Some CH3CO2–(aq) will react with H3O+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium. b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3Determine the pH of 0.082 M ammonia, NH3 (aq) and percent ionization of base.The pH of 0.40 M HF(aq) is 1.93. Calculate how the pH changes when 0.356 g of sodium fluoride is added to 50.0 mL of the solution. Assume that the volume change is small and can be neglected
- The pH of an aqueous solution of 0.176 M ammonium bromide, NH,Br (aq), is This solution isThe pH of an aqueous solution of 0.289 M ammonium iodide, NH4I (aq), is This solution is6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.
- 24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?The pH of an aqueous solution of 0.124 M ammonium nitrate, NH,NO3 (aq), is This solution isThe pH of an aqueous solution of 0.291 M ammonium perchlorate, NH4C1O4 (aq), is This solution is (Assume that K (NH3) = 1.80 × 10-5.)
- Calculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5.A brand of window-cleaning fluid is composed of ammonia solution, water, a colouring agent, and a very small quantity of soap. It has 0.15 mol/L concentration of NH3(aq). What is the pH of this fluid?The pH of an aqueous solution of 8.39×10-2 M ammonium nitrate, NH4NO3 (aq), is