65.0 mL of 0.125 M NaOH is titrated with 0.315 M HCl. What is the pH after the addition of 30.0 mL of HCl?
Please show clear work and clarify where all numbers came from and equations used.
65.0 mL of 0.125 M NaOH is titrated with 0.315 M HCl. What is the pH...
65.0 mL of 0.125 M NaOH is titrated with 0.315 M HCl. What is the pH after the addition of 30.0 mL of HCl?
1. A solution (50.0 mL) of 0.125 M HCl is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL KOH has been added? Can all work be shown? Equations/ Ice charts If applicable-please include them. I need to understand. Thank-you in advance.
a 30.0 mL sample of 0.250 M HClO is titrated with 0.125 M KOH. Calculate the pH of the solution after the addition of the following volumes of base. Ka= 3.5 x 10^-8 for HClO. a) 0.0 mL base added b) 25.0 mL c) 50.0 mL d) 55.0 mL e) 60.0 mL f) 65.0 mL g) 75.0 mL
10 mL of 1M NaOH solution is titrated with 0.5M HCl to a pH of 2. What volume of HCl was added? (in unit of mL) Please show all work and explain!
1. A solution (50.0 mL) of 0.125 M HCl is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL KOH has been added?
A 40.0 mL volume of 0.100 M NaOH is titrated with 0.0500 M HCl. Calculate the pH after addition of the following volumes of acid. A). 83.6 mL
A 10.00 mL sample of 0.300 M NH3 is titrated with 0.100 M HCl (aq). what is the initial pH? Calculate the pH after the addition of 10.0, 20.0, 30.0 and 40.0 mL of HCl. The Kb for NH3 is 1.8 x 10^-5
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
100. mL of 0.200 M HCl is titrated with 0.250 M NaOH. The pH is 1.30. What is the pH of the solution at the equivalence point?
2. What is the "What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. 3. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (K, for acetic acid is 1.8x10-5.)