Chemistry
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Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). [Ka = 6.5 x 10-5 for benzoic acid]
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- Calculate the pH of a buffered solution that is 0.100 M in C6H5COOH (Ka = 6.4 x 10–5) and 0.100 M in C6H5COONaarrow_forwardSuppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).arrow_forwardWhat is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 40.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.arrow_forward
- You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?arrow_forwardAssuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 3.2–3.5 a - NaNO 2 / HNO 2 (K a = 4.5 × 10 –4) b - NaOCl / HOCl (K a = 3.2 × 10 –8) c - NaCl / HCl d - NH 3 / NH 4Cl (K a = 5.6 × 10 –10) e - CH 3COO 2Na / CH 3COOH (K a = 1.8 × 10 –5)arrow_forwardCalculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). (K₂ = 6.5 × 10-5 for benzoic acid) aarrow_forward
- 5. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4 a. What is the pH of this buffer? b. If 0.075 mol HCI is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes) c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)arrow_forwardHow do I complete problem 1 in a step by step?arrow_forwardWhich acid, along with it's corresponding salt, would be best to make a buffer of pH 7? hydrofluoric acid, Kg = 6.8 x 104 O hypochlorous acid, K, = 3.5 x 10o-8 O hydrocyanic acid, K, = 4.9 x 10-10 O acetic acid, K, = 1.8 x 105arrow_forward
- A buffer solution is 0.462 M in HCN and 0.283 M in KCN. If Ką for HCN is 4.0 × 10-¹0, what is the pH of this buffer solution? pH =arrow_forwardWhat is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10-5) when 100.0 mL of a 0.0.75 M HCl solution is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ?Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.arrow_forward6a. Draw the Lewis Dot structure for the following diprotic acid: HOOC-CH,-COOH. 38.5 mL of a 1.15 M solution of this acid is titrated to the equivalence point with 0.69 M KOH. Write the balanced equation for this reaction and determine the volume of base needed to completely neutralize the acid.arrow_forward
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