a) Calculate the pH of a 0.8M solution of HCOOH (Ka = 1.8 x 10-4) in 0.4M Li+ HCOO-.
b) Calculate the pH of a solution of 0.4M NH4Cl and 0.5M NH3 (pKa NH4+ = 9.2).
c) Calculate the pH of a titration of 100 mL 1.5M HCl when 75 mL 1.25M NaOH has been added.
d) What volume of 1.25M NaOH must be added to 100 mL of 1.5M HCl to reach equivalence?
a) Calculate the pH of a 0.8M solution of HCOOH (Ka = 1.8 x 10-4) in...
a) Calculate the pH of a titration of 100 mL 1.5M HCl with 1.25M NaOH at equivalence. WHY is the pH what it is (if it’s 7, why is the solution neutral? If not 7, why?) b) Calculate the pH of a titration of 100 mL 1.5M HCOOH (Ka = 1.8 x 10-4) when 75 mL 1.25M NaOH has been added. c) What volume of 1.25M NaOH must be added to 100 mL of 1.5M HCOOH to reach equivalence?
Calculate the pH of a titration of 100 mL 1.5M HCl with 1.25M NaOH at equivalence. WHY is the pH what it is (if it’s 7, why is the solution neutral? If not 7, why?)
Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with NaOH. The experiment is halted when half of the acid has been titrated. Which statement correctly describes the composition of the titration solution? Check all that apply. Group of answer choices The concentration of HCOOH is greater than the concentration of H+. The concentration of HCOO− is approximately equal to the concentration of HCOOH. The concentration of formate ions (HCOO−) is smaller than the concentration of H+....
Calculate the pH of a 0.0140 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4). pH =
Calculate the hypothetical pH AFTER addition of 15.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. QUESTION 7 10 poir Calculate the hypothetical pH AFTER addition of 40.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. Calculate the hypothetical pH AFTER addition of 46.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with...
0. A solution of formic acid (HCOOH, Ka 1.8 x 10) has a pH of 2.70. Calculate initial concentration of formic acid in this solution.
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
In this assignment, you will calculate the pH of a solution during the course of a titration. The titration under study will be: 50 mL 0.5 M acetic acid (Ka = 1.8 x 10-5) is titrated with 0.25 M sodium hydroxide. a) Write a reaction for this titration b) Calculate the equivalence volume, and the pH at this point. c) Calculate the initial pH of the acetic acid solution Calculate the pH of the solution after d) 5 mL NaOH...
In regard to the picture: 1) A) Calculate the pH of a 1 MNH4Cl solution. B) Calculate the pH of the solution that results following addition of 10 mLof 1 MNaOH to 40 mL of 1 MNH4Cl. C) Calculate the pH of the solution that results following addition of 30 mLof 1 MNaOH to 40 mL of 1 MNH4Cl. Please explain too! Thanks! 13 12 NH 10 of NH NH At the midpoint of the titration where half the acid...