The stinging sensation from red ants comes from formic acid, which dissociates based on the following equilibrium:
HCOOH(aq) ⇄ H+(aq) + HCO2-(aq) Ka= 1.8 x 10-4
What is the pH of a 0.50 M solution of formic acid?
The stinging sensation from red ants comes from formic acid, which dissociates based on the following...
The stinging sensation from red ants comes from formic acid, which dissociates based on the following equilibrium: HCOOH(aq) + H+ (aq) + HCO2 (aq) K=1.8 x 10-4 What is the pH of a 0.811 M solution of formic acid? pH
4) The venom of stinging ants contains formic acid (Ka = 1.8 x 10-4). Calculate the pH of a 0.25 M solution of formic acid.
The venom of biting ants contains formic acid, HCOOH (Ka = 1.8×10–4 at 25 °C). What is the pH of a 0.105 M solution of formic acid?
Calculate the pH of a solution containing formic acid, 0.50 M HCOOH, and sodium format, 0.35 M NaCOOH (Ka (HCOOH) = 1.8 x 10-4)
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
4. (2pts) Consider the following aqueous equilibrium for a formic acid solution: HCO2H (aq) = H+ (aq) + HCO2 (aq) Suppose hydrogen chloride gas is dissolved in the solution. Which statement below regarding the resulting solution is not true? (Ignore any volume changes) A. The pH decreases. B. The H concentration increases. C. The system shifts left to reestablish equilibrium. D. The concentration of HCO2 decreases, E. The value of Ka increases. Page 1 of 2
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)...
(4) 6 pts. A buffer contains 0.500 M of Formic acid (HCHO,) and 0.500 M of sodium formate (NaCHO2). Formic acid is a weak acid that dissociates in water as following: HCHO2 (aq) + H20 (1) =H30+ (aq) + CHO2 (ag) The equilibrium constant: Ks = ([H30+1X[CH02:])/[HCH02] =1.8 x 10-4 Calculate the pH of the buffer solution.
Which one of the following solutions has the lowest pH? A. a 0.1 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) B. a 0.1 M solution of ammonium chloride, NH4Cl(s) (Ka (NH4+) = 5.6 x 10-10) C. a 0.01 M solution of acetic acid, CH3COOH (Ka = 1.8 x 10-5) D. a 0.01 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) E. a 0.1 M solution of acetic acid, CH3COOH (Ka = 1.8 x...
3. Calculate the pH of a solution that contains 0.250 M HCOOH (formic acid) and 0.100 M NaCOOH (sodium formate). Given Ka = 1.8 x 10 - 4 for HCOOH. Please include the ICE table.