14- 13 Titration of weak acid CH,COOH 12 Equivalence point pH, 8.72 10 Phenolphthalein [pH range Equivalence point pH, 7.00 Litmus pH range 6. Methyl orange [pH range 4 3 Titration of strong acid HCI 1 - 10 15 20 25 30 35 40 45 50 Volume of 0.100 M NaOH added (mL) Figure 14.23 The graph shows a titration curve for the titration of 25.00 mL of 0.100 M CH3CO,H (weak acid) with 0.100 M NaOH (strong base) and the titration curve for the titration of HCI (strong acid) with NaOH (strong base). The pH ranges for the color change of phenolphthalein, litmus, and methyl orange are indicated by the shaded areas. 11 Hd

You are titrating 90.0 mL of a weak base solution (A-) with a concentration of 0.0515 M, using an HCl solution with a concentration of 0.0662 M. Note that the Ka Value for the conjugate acid , HA, is 5.6 x 10-10 . a) What is the pH of the initial weak base solution? b) What is the pH of the solution at the equivalence point? c) What is the pH of the solution when an additional 10 mL of HCl solution is added after reaching the equivalence point?

Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.

A buffer solution is made that is 0.417 M in HC1O and 0.417 M in KC1O. If K, for HC1O is 3.50 × 10-8, what is the pH of the buffer solution? PH = Write the net ionic equation for the reaction that occurs when 0.110 mol HNO3 is added to 1.00L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30* instead of H*)

A 200mL solution of 0.3 M weak acid is titrated with 40 mL of 1.5 M NaOH. If the Ka of the acid is 5.37 x 10-10, what is the pH at this point in the titration?

Near the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.

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?

Calculate 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) a

In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x 10-5), with 0.100 M NaOH. At the equivalence point, the concentration of the primary species in solution is approximately What is the pH of the solution at the equivalence point? At the equivalence point, what percentage of the analyte has been titrated?

A buffer solution is made that is 0.339 M in HF and 0.339 M in KF. If K, for HF is 7.20 × 10-4, what is the pH of the buffer solution? pH =| Write the net ionic equation for the reaction that occurs when 0.088 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +