2. A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH...
A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa hasa pH of 3.77. What will the pH be after 0.010 mol of NaOH has beenadded to 100.0 mL of the buffer? correct answer: 3.95 please show me step by step how to solve this problem, i couldn'tget the right answer above. Thanks in advance!
A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? (Assume the addition cause negligible volume change.)
23. A 1.0 L buffer solution is prepared with 0.25 M formic acid (HCOOH) and 0.50 M sodium formate (HCOONa). HCOOH(aq) + H2O(aq) – HCOO (aq) + H30+(aq) pKa = 3.74 What is the pH of this buffer solution? (A) 3.74 (B) 4.04 (C) 4.50 (D) 4.20
the pH of a 0.010 M solution of formic acid, HCOOH, at 25 degrees celcius is 3.78. Calculate Ka for formic acid at this temperature.
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)
5. A buffer solution contains 10.0 mmol of formic acid (HCOOH) and 15.0 mmol of formate (HC00°). If the solution pH is 3.95, then what is the Ka of formic acid? (a) 7.5 x 10-5 (b) 1.1 x 104 (c) 4.1 x 10-2 (d) 1.7 x 104 6. At 298 K, the equilibrium constant for the below reaction is 4.17 x 10'. What is the concentration of Cl" at equilibrium? Pb2+ (aq) + 2 C1- (aq) = PbCl, (s) (a)...
a 100 ml solution of 0.250 M formic acid (HCOOH) was titrated to its equivalence point with 50 mL of sodium hydroxide. The complete molecular equation for the reaction is shown below HCOOH (aq) + NaOH (aq)---------> HCOONa (aq) +H20 (l) Ka of HCOOH= 1.7 x 10 ^-4 calculate the pH at the equivalence point
You have 2.50 L of a 0.450 M HCOOH and 0.550 M HCOONa buffer solution. (Ka for HCOOH is 1.8x10^-4) a) Calculate the pH of the buffer solution. b) Determine the pH of the buffer solution after the addition of 0.150 mol of NaOH (assume no change in volume).
A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The volume of the buffer is 100 mL ; with [HCOOH] = 0.110 mol L-1 and [HCOO- ] = 0.101 mol L-1 . The pKa of HCOOH = 3.74. What is the pH of this buffer? Write down the balanced chemical equation that describes the reaction of this buffer when an HCl solution is added. c) What is the resultant pH of this solution after...
Calculate the pH of a buffer solution that is 0.30 M formic acid (HCO2H) and 0.50 M sodium formate (HCO2Na). Ka of HCO2H is 1.8 x 10-4