1. If 1.000 gram of Na,coz is place in 0.5000 mL of water, what will be...
What is the pH of a solution of 20.00 mL of 3.00 M HCL that is titrated with 10.00 mL of a 6.00 M solution of NaOH ? (Note both acid and base are strong)
Assume that a 50.00 mL sample of 0.1000 M HCl in an Erlenmeyer flask is titrated with 0.1000 M NaOH. (a) What is the initial pH before any base is added? (6) What is the pH of the solution after 10.00 mL of NaOH? (c) What is the pH of the solution after 20.00 mL of NaOH? (d) What is the pH of the solution after 50.00 mL of NaOH? (e) What is the pH of the solution after 60.00...
A 1.28 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.203 M aqueous barium hydroxide solution. It is observed that after 7.86 milliliters of barium hydroxide have been added, the pH is 3.000 and that an additional 16.6 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of Ka for the...
A 1.53 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.234 M aqueous barium hydroxide solution. It is observed that after 16.3 milliliters of barium hydroxide have been added, the pH is 4.924 and that an additional 10.0 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for the...
A 1.20 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.485 M aqucous potassium hydroxide solution. It is observed that after 7.33 milliliters of potassium hydroxide have been added, the pH is 4.515 and that an additional 13.3 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? (2) What is the value of K, for the...
A 1.48 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.291 M aqueous barium hydroxide solution. It is observed that after 7.15 milliliters of barium hydroxide have been added, the pH is 9.104 and that an additional 13.2 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol 2) What is the value of K_a for...
A 0.660 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.370 M aqueous potassium hydroxide solution. It is observed that after 10.1 milliliters of potassium hydroxide have been added, the pH is 7.732 and that an additional 5.10 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? _______ g/mol (2) What is the value of Ka...
A 1.75 gram sample of an unknown monoprotic acid is dissolved in 40.0 mL of water and titrated with a a 0.477 M aqueous barium hydroxide solution. It is observed that after 9.85 milliliters of barium hydroxide have been added, the pH is 3.603 and that an additional 5.05 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for...
A 0.843 gram sample of an unknown monoprotic acid is dissolved in 40.0 mL of water and titrated with a a 0.496 M aqueous potassium hydroxidesolution. It is observed that after 5.16 milliliters of potassium hydroxide have been added, the pH is 9.092 and that an additional 9.84 mL of the potassium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? _______g/mol (2) What is the value of Ka for the...
You have 15.00 mL of a 0.100 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...