Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH).
100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl
100.0 mL of 0.100 M HNO2 (Ka = 4.0 x 10-4) by 0.100 M NaOH
100.0 mL of 0.100 M HOCl (Ka = 3.5 x 10-8) by 0.100 M NaOH
100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl
100.0 mL of 0.100 M HI by 0.100 M NaOH
Rank the following titrations in order of increasing pH at the halfway point to equivalence (1...
1.) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M HF (Ka = 7.2 x 10-4) by 0.100 M NaOH 100.0 mL of 0.100 M HCl by 0.100 M NaOH...
1) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M KOH by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl 100.0 mL of 0.100 M HI by 0.100 M NaOH 100.0 mL of 0.100 M...
Rank the following titrations in order of increasing pH at the equivalence point of the titration (1 = lowest pH and 5 = highest pH). 1 2 3 4 5 100.0 mL of 0.100 M HNO2 (Ka = 4.0 x 10-4) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M HOCl (Ka = 3.5 x 10-8) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100...
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations a. 100.0 ml of 0.70M HC7H5O2 (Ka= 6.4x10^-5) titrated by 0.10 M NaOH pH at the halfway point = ______? pH at the equivalence point = _____? b. 100.0ml of 0.70M C2H5NH2 (Kb= 5.6x10^-4) titrated by 0.60M HN03 pH at the halfway point = ______? pH at the equivalence point = _____? c. 100.0 ml of 0.70M HCL titrated by 0.15m NaOH...
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.) (a) 101.5 mL of 0.19 M HCO2H (Ka= 1.8 ✕ 10-4) titrated with 0.19 M KOH (b) 104.1 mL of 0.18 M (C2H5)3N (Kb = 4.0 ✕ 10-4) titrated with 0.36 M HClO4 (c) 100.9 mL of 0.47 M HClO4 titrated with 0.24 M NaOH
Assume an indicator works best when the equivalence point of a titration comes in the middle of the indicator range. For which of the following titrations would methyl red be the best indicator? The pH range of methyl red is 4.8 to 6.0. Select one: a. 0.100 M NH3 (Kb = 1.8 × 10–5) + 0.100 M HCl b. 0.100 M Sr(OH)2 + 0.100 M HI c. 0.100 M HF (Ka = 7.2 × 10–4) + 0.100 M NaOH d....
1) Calculate the pH at the halfway point and at the equivalence point of the given titration 200.0 mL of 30M HC2H5O2 (Ka = 6.4 x 10-5) titrated by 0.10 M NaOh
3. The following titrations are all at their equivalence points. Rank the solutions from highest to lowest pH at the equivalence point and explain your reasoning. a. 20.00 mL of 0.10 M NaOH + 10.00 mL of 0.20 M acetic acid b. 20.00 mL of 0.10 M NaOH + 10.00 mL of 0.20 M chloroacetic acid c. 10.00 mL of 0.20 M NaOH + 20.00 mL of 0.10 M HCI
Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HOCl, Ka = 4.0 x 10-8; HCN, Ka = 6.2 x 10-10; NH4+, Ka = 5.6 x 10-10
Which one of the following titrations will have an equivalence point with a pH of 7? options: HNO3 with KOH NaC2H3O2 with RbOH HF with NaOH none of these HCl with NH3