1. What is the pOH of 2.9 × 10-7 M KOH?
2. Formic acid (HCOOH) undergoes the following dissociation reaction:
HCOOH ⟷ H+ + HCOO- Ka = 1.8 × 10-4
What would be the Kb value of its conjugate base?
1. What is the pOH of 2.9 × 10-7 M KOH? 2. Formic acid (HCOOH) undergoes...
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?
1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid? pOH = 2. What is the pH of an aqueous solution of 1.77×10-2 M nitric acid? pH = 3. What is the pOH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pOH = 4. What is the pH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pH = 5. Calculate the pH of a 0.409 M aqueous solution of nitrous acid (HNO2, Ka =...
a) What is the buffer range for a buffer made with formic acid (HCOOH)? (Ka = 1.8 x 10-4) b) What is the buffer range for a buffer made with CH3NH2 ? (Kb = 3.7 x 10-4) Be sure to think of the conjugate acid.
Calculate the pH of a 0.0167 M aqueous solution of formic acid (HCOOH, K, = 1.8x10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH [HCOOH)equilibrium [HCOO equilibrium
Calculate the pH, pOH, [H3O +] and [OH-] and formic acid (HCOOH) in a 0.0500M formic acid solution (Ka formic acid: 2.1x 10 –4).
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)...
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 0.065 M formic acid (HCOOH) solution. Formic acid is a weak acid with Ka = 1.8 × 10–4 at 25°C. 2.48 is WRONG answer!!!!!! Write your answer to two decimal places. Calculate the pH of a 0.065 M formic acid (HCOOH) solution. Formic acid is a weak acid with 1.8x 10at 25°C. pH 2.48
The value of K, for formic acid is 1.80x10-4. What is the value of Kb, for its conjugate base, HCOO“?
please show all work neatly 5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...