First see balance reaction between formic acid and NaOH -
HCOOH + NaOH HCOONa + H2O
From balance reaction it is clear that one mole of formic acid required one mole of sodium hydroxide.
So experiment is halted after exactly half of addition of formic acid. That's means half of formate ion(HCOO-) gets formed and half of formic acid should be remain as it is (HCOOH). So option '4 ' is only correct .
Question 6 0.1 pts Consider a titration of formic acid (HCOOH, K2 = 1.8 x 10-4)...
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+....
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?
Consider the titration of formic acid (HCOOH) with potassium hydroxide (KOH) . Which species will be present at the equivalence point? Select all that apply. Titration of 0.1200 M HCOOH with 0.2000 M KOH Consider the titration of formic acid (HCOOH) with potassium hydroxide (KOH). Which species will be present at the equivalence point? Select all that apply. 14.00 - 12.00 Check all that apply. 10.00 "OH(0) 8.00 pH > 7.00 at equivalence point PH Kol 6,00 4.00 OK HCOOH(aq)...
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)...
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.
69. A solution of formic acid (HCOOH, K, = 1.8 X 10^4) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
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...
Name Formula К. Acetic acid CH3COOH 1.8 x 10-5 Formic acid HCOOH 3.0 x 10 Hydrazoic acid HN3 1.0 x 10-5 Hydrocyanic acid HCN 6.2 x 10-10 Hypochlorous acid HOCI 6.8 x 10-8 Nitrous acid HNOL 7.4 x 104 20. (7 pts) Use the table above to answer the following questions. A. Rank the following solutions in order from the lowest to highest pH. 0.10 M CH3COO- 0.10 M HCOO 0.10 M N 0.10 M OCI pH value: B. Write...
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
Consider a titration of 100-mL of .25 M formic acid (Ka-1.8 x 10^-4) with .2 M KOH What is the pH after 100 mL of base has been added?