Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 59.5 mL of 0.436 M nitrous acid (K₂ = 4.5x10-4) by 0.436 M NaOH at the following poin (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOH

When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?

Determine the pH during the titration of 36.4 mL of 0.335 M ethylamine (C₂H5NH₂, Kb = 4.3x10-4) by 0.335 M HI at the following points. (a) Before the addition of any HI 12.1 (b) After the addition of 13.1 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.6 mL of HI

Determine the pH during the titration of 35.1 mL of 0.297 M diethylamine ((C2H5)2NH , Kb = 6.9×10-4) by 0.297 M HI at the following points.(a) Before the addition of any HI(b) After the addition of 13.1 mL of HI(c) At the titration midpoint (d) At the equivalence point (e) After adding 54.4 mL of HI

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, K₁ = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4

6. ( ) A 40 mL sample of a 0.2 M RNHz (kb = 3.7 x 10") is titrated with 0.2 M HC (eg). Calculate the pH after the addition of each of the following volume acids. a) Initial pH (b) Volume of HCI (ag): 20 mL (c) Volume of HCI (ag): 39.9 mL (d) Volume of HCI (ag): 40.0 mL (e) Volume of HCI (ag): 40.1 mL

Consider the titration of 50.00 mL of 0.100 M benzoic acid (HC7H5O2, Ka = 6.3 × 10−5) (aq) with 0.130 M LiOH(aq). What is the pH of the titration solution... a) before any LiOH is added? b) after 20.00 mL of LiOH is added? c) at the equivalence point? Also, what volume of LiOH is required to reach this? d) For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer.

A 29.9 mL sample of 0.253 M dimethylamine, (CH3)2NH, is titrated with 0.292 M hydroiodic acid. (1) Before the addition of any hydroiodic acid, the pH is (2) After adding 11.5 mL of hydroiodic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 39.1 mL of hydroiodic acid, the pH is

Determine the pH during the titration of 60.6 mL of 0.420 M hydrocyanic acid (Ka = 4.0×10-10) by 0.420 M NaOH at the following points.(a) Before the addition of any NaOH(b) After the addition of 14.0 mL of NaOH(c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 90.9 mL of NaOH

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.