Please show your work. Thanks in advance.
A 100.0 mL solution of 0.5 M histidine in its tribasic form, A3- , (pKa1 = 1.70, pKa2 = 6.02, pKa3 = 9.08) is titrated with 1.0 M HCl titrant.
(a) calculate the pH after the addition of 50.0 mL of titrant,
(b) calculate the pH after the addition of 62.0 mL of titrant,
Please show your work. Thanks in advance. A 100.0 mL solution of 0.5 M histidine in...
Please show your work. Thanks in advance. A 100.00 mL volume of 0.0400 M propionic acid (CH3CH2COOH; Ka = 1.34 ´ 10-5 ) was titrated with 0.0837 M NaOH. Calculate the pH after the addition of: 0 Ve, 0.25 Ve, Ve, and 1.1 Ve mL of titrant where Ve is the volume of NaOH required to reach the equivalence point.
Please show your work. Thanks in advance. A 100.00 mL volume of 0.0400 M propionic acid (CH3CH2COOH; Ka = 1.34 ´ 10-5 ) was titrated with 0.0837 M NaOH. Calculate the pH after the addition of: 0 Ve, and 0.25 Ve, of titrant where Ve is the volume of NaOH required to reach the equivalence point.
You dissolve some solid Na2C2O4 in water to make 100.0 mL of 0.1M solution. You add 50.0 mL of 0.20M HCL. What is the pH of the resulting solution? What is the pH after 75.0mL of HCl (total) is added? pka1 = 1.25, pka2 = 4.27
You dissolve some solid Na2C2O4 in water to make 100.0 mL of 0.1M solution. You add 50.0 mL of 0.20M HCL. What is the pH of the resulting solution? What is the pH after 75.0mL of HCl (total) is added? pka1 = 1.25, pka2 = 4.27
A 50.0 mL solution of 0.174 M potassium alaninate (H2NC2H5CO2K) is titrated with 0.174 M HCl. The pKa values for the amino acid alanine are 2.344 (pKa1) and 9.868 (pKa2), which correspond to the carboxylic acid and amino groups, respectively. a. Calculate the pH at the first equivalence point b. Calculate the pH at the 2nd equivalence point
A 0.1983 g sample of Na2CO3 was dissolved in 100.00 ml H20. That solution was titrated with 0.1531 M HCL as titrant. The PKa1 and PKa2 of carbonic acid (the conjugate acid of the carbonate ion) are 6.351 and 10.329, respectively. 1.) What is the initial pH of the sodium carbonate solution. 2.) What is the first equivalence point (in ml HCL)? What is the pH at 1st eq.? 3.) What is the second equivalence point (in ml HCL)? What...
. A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution at the following conditions below: a. before the addition of any LiOH. b. after the addition of 30.0 mL of LiOH. c. after the addition of 50.0 mL of LiOH. d. after the addition of 66.67 mL of LiOH e. after the addition of 75.0 mL of LiOH. f. after the addition of 100.0 mL of LiOH.
It is titrated with 0.1 M HCl 25 mL of a solution which contains a mixture of salts: NaHA and Na2A. Two points are known from the valuation curve: 1) when adding 1.25 mL of HCl the pH is 6.0 and 2) Add 12.5 mL of HCl the pH is 4.5. Calculate the volume of the 0.1 M HCl solution necessary for the complete evaluation of both salts H2A (pKa1 = 3.0, pKa2 = 6.0). ANSWER 35 mL
A: 48.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 24.0 mL of KOH at 25 ∘C B: Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C. C: A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10−5) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25...
The pK, of hypochlorous acid is 7.530. A 50.0 mL solution of 0.118 M sodium hypochlorite (NaOCl) is titrated with 0.348 M HCl. Calculate the pH of the solution after the addition of 6.48 mL of 0.348 M HCl. pH = 8.754 Incorrect Calculate the pH of the solution after the addition of 18.1 mL of 0.348 M HCl. pH = 2.274 Incorrect Calculate the pH of the solution at the equivalence point with 0.348 M HCl.