5) Using the following pKb (pKb = 4.11) of an unknown base, calculate the Ka of the corresponding conjugate acid and use the Ka value to identify the unknown base. Be careful to show all the steps used to convert pKb to Ka. (See attachment for data) 6) Potassium hydrogen phthalate (KHP, K+OOC-C6H4-COOH) is a carboxylic acid
By using samples of the same cerium solution throughout each trail and precise volumetric pipettes, accuracy, along with precision, the potential change of the reaction and the determination of the molar concentration of iron (II) ions in a sample of unknown concentrations were determined by potentiometric titration of the react
Titration of Strong and Weak Acids. Determination and assessment of equivalence points. Calculation of molarity. Estimation of acid/base equilibrium constant, pKa
Procedure 1 Add 25 mL HCl (of unknown concentration) to the flask. Add 2 drops of phenolphthalein to the flask. Fill a burette with 50 mL of 1M NaOH solution. Record this initial volume (50mL). Record the pH of the solution in the flask. (0.22). Continue to add NaOH in 1 mL increments. Record the pH for each milliliter added.
1. Write the complete ionic and net ionic equations for the reaction between AgNO3 and K2CrO4. Molecular equation: 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq) 2. Write the complete ionic and net ionic equations for the reaction between AgNO3 and NaCl. Molecular equation. AgNO (aq)+NaCl(aq)---à AgCl(s)+NaNO (aq)
1) Plot the pH titration of tyrosine, whose structure is shown attached at pH = 7.0. Show: a) The pH value at each equivalence points and each 1/2 equivalence point b) The charge at each equivalence and 1/2 equivalence point c) The isoelectric point of the amino acid and give its value d) The approximate shape of the titrat
A 30 mL sample of 0.35 M of lactic acid is titrated with a 0.25 M NaOH solution. Calculate the pH before NaOH is added. After 20 mL of NaOH is added. After 42 mL. After 45 mL. After 60 mL. After 80 mL. Graph the titration curve.
C6H5COOH ( benzoic acid ) = C6H5COO- (aq) + H+ (aq) Ka = 6.46 x 10^-5 Benzoic acid dissociates in water as shown in the equation above. A 25.0 ml sample of an aqueous solution of pure benzoic acid is titrated using standardized 0.150 M NaOH A) After addition of 15.0ml of the 0.150 M NaOH , the pH of the resulting solution is
Calculate Titration. See attached file for full problem description. 19. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 25.0 mL of 0.200 M HA with 0.100 M NaOH. Ka = 2.0 * 10^-5. 20. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 50.0 mL of 0.100 M N
I am having trouble with this one problem. It is a couple of steps but I am very confused. The problem states that there is 25 mL of a propionic acid where the concentration is unknown and it was titrated with .104M KOH. I got the Ka=1.34*10^-5 for the propionic acid. It also tells you that the equivalence point was reac
Please give simple, step by step solutions. Thanks! 1) Write the molecular, ionic, and the net ionic equations for the reaction between aqueous potassium carbonate and aqueous lead(II) chloride to form aqueous potassium chloride and a precipitate of lead(II) carbonate. Molecular equation: Ionic equation: Net ionic e
What's the pH at the first equivalence point of 0.100M of malonic acid of 25mL with 0.140M of NaOH? What's the pH after 25mL of NaOH were added?
A sample of 0.0054 mol propanoic acid was dissolved in water to give 50ml solution. This solution is titrated with 0.150 M of NaOH. Draw the expected titration curve labeling the equivalence point (including the volume of NaOH added and the pH) and show the pKa point (labeling the pH value and volume of NaOH added)
Outline a titration procedure for determining the exact concentration of the aqueous nitric acid. Assume that aqueous sodium carbonate of concentration 0.500 mol dm3 is available.