2. What volume of 0.1500M KMnO, would be required to react with 1.000g of formic acid,...
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
The equivalence point for titration of 50 ml of 0.1 M formic acid, HCO,H (a weak acid) requires what volume of 0.2 M sodium hydroxide? O 25 ml. O 50 ml. less than 25 ml as formic acid is a weak acid. 100 ml. Ostween 25 and 50 ml as formic acid is a weak acid.
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, PK: - 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution 6. After the addition of 20.00 mL of NaOH solution C. After the addition of 25.00 mL of NaOH solution d. At what volume of added NaOH will pH -pK
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, pK, = 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution. b. After the addition of 20.00 mL of NaOH solution c. After the addition of 25.00 mL of NaOH solution. d. At what volume of added NaOH will pH =pK,
1. what is the volume of 2.00M solution of sulfuric acid required to react with 250g of carbonate of magnesium according to the following reaction? MgCO3 + H2SO4 -> MgSO4 + CO2 + H2O
References What volume of 0.125 M oxalic acid, H,C,04, is required to react with 50.9 mL of 0.764 M NaOH? H,C,04 (aq) + 2 NaOH(aq) Na2C,04 (aq) + 2 H30() Volume =
A solution buffered at pH 3.90 is needed for a reaction. Would formic acid (HCOOH = HA) and its salt, sodium formate, NaHCO2 = NaA), make a good choice for this buffer? If so, what ratio of moles of A- and HA is needed? Use the Henderson Hasselbalch Equation. Ka formic acid = 1.8 x 10-4
For the given reaction, what volume of O 2 would be required to react with 7.0 L of SO 2 , measured at the same temperature and pressure? 2 SO 2 ( g ) + O 2 ( g ) ⟶ 2 SO 3 ( g )
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)...
An analytical chemist is titrating 207.5 mL of a 0.5100 Msolution of formic acid (H,CO, with a 0.4800 M solution of KOH. The pK of formic acid is 3.74 Calculate the pH of the acid solution after the chemist has added 233.7 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places....