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+.
The concentrations of HCOOH and H+ are equal.
the addition of NaOH will increase the extent of dissociation of HCOOH as it will tend to keep the Ka value constant.
Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with NaOH. The experiment is halted when half of the acid h...
Question 6 0.1 pts Consider a titration of formic acid (HCOOH, K2 = 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. The concentrations of HCOOH and H+ are equal. The concentration of HCOOH is greater than the concentration of H+. The concentration of formate ions (HCOO-) is smaller than the concentration of H+. The concentration of HCOO-is...
Given the following information: formic acid HCOOH Ka = 1.8×10-4 triethylamine (C2H5)3N Kb = 5.2×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.167 Maqueous formic acid and triethylamine are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion. -reactant or product favored? -pH is >, <, = to 7?
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.
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
2. Consider the titration of 25.0mL of 0.100M formic acid with 0.100 M NaOH (Ka= 1.8 x 10-4). Part IV. What is the pH after adding 25.0mL of NaOH? a)5.60 b) 8.23 c) 9.80 d)13.00 Answer is B
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25.0 mL of 0.10 M formic acid (HCOOH, Ka = 1.8 x 10-4) is mixed with 20.0 mL of 0.10 M potassium hydroxide. What is the pH of the resulting solution? A. 2.37 B. 4.35 C. 13 D. 0.60
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4) with a pH = 4.00, what ratio of formic acid to sodium formate is required? (Notice that I am asking for the ratio of acid to base, not base to acid!) a) 1.25 b) 0.56 c) 0.82 d) 1.87 QUESTION 4 If you find that you need an acid to base ratio of 4.23 and you are using 50.00mL of a 1.00M acid solution, what volume...
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?