1. Calculate and formulate an ophthalmic buffer solution of boric acid (pKa=9.24) and sodium borate. To make it pH 9.0 with buffer capacity of 0.02, the molar concentrations of boric acid should be ____Mol/L.
2. And the molar concentration of and sodium borate should be ___Mol/L.
1. Calculate and formulate an ophthalmic buffer solution of boric acid (pKa=9.24) and sodium borate. To...
Calculate and formulate an ophthalmic buffer solution of boric acid (pKa=9.24) and sodium borate. To make it pH 9.0 with buffer capacity of 0.02, the molar concentrations of boric acid should be ____mMol/L. And the molar concentration of and sodium borate should be ___mMol/L.
Calculate and formulate an opthalmic buffer solution of boric acid (pKa= 9.24) and sodium borate. To make it pH 9.0 with buffer capacity of 0.02, the molar concentrations of boric acid and sodium borate should be ___ Mol/L.
Calculate the pH of a 10-5 mol L-1 solution of boric acid. H3BO3 (pKa = 9.24). Solution: 6.90.
a. One desires to adjust a solution of pH 8.8 by the use of a boric acid/sodium borate buffer. What approximate ration of acid and salt is required? pKa of boric acid = 9.24?
1. What is the pH of a buffer solution prepared with a 0.4 M sodium citrate and 1% citric acid (pka for citric acid - 3.13, MW - 192 g/mol)? 8. A buffer solution is prepared using 0.4 mole of a weakly basic drug (pka - 10.1) and an unknown quantity of its salt. The final solution has a pH of 8.99. How much of the salt was used? 9. A buffer solution with a desired pH of 8.15 needs...
pH of 9.2 using ammonium nitrate: pKa= 9.24 2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conjugate base A- and the monoprotic acid HA. In cq. (1), pH-_ log[H+], pK, =-log Ka, and [J]i and [JIe are the initial and equilibrium molar concentration of the Jth species, respectively. The buffering capacity of the buffer is given by [1] Ka H+ where K,e-1.0 ×...
You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.
1. Calculate the pKa of lactic acid, given that when the concentration of lactic acid is 0.010 M and the concentration of lactate is 0.087 M, the pH is 4.80 B. Calculate the ratio of the concentrations of acetate and acetic acid required in a buffer system of pH 5.30 C The pH of a 0.20 M sodium acetate buffer is 5.1. The pKa of acetic acid is 4.76. Explain in details (showing all calculation) how to prepare the buffer...
1) How would you make 300 ml of a 0.1 M sodium phosphate buffer, pH 7.0 (pKa = 7.2) phosphate dibasic (the conjugate base). 2) What are the concentrations of acetate and acetic acid in a 0.2 M acetate buffer pH 5.3? The pKa for acetic acid is 4.76. 3)You have 100 ml of 0.1 M acetate buffer pH 5.2 (pKa 4.76). You add 10 ml of 0.1 M NaOH. Calculate the resulting change in pH and the buffering capacity...