In the titration of 50.0 ml of 0.200 M Sulfurous Acid (H2SO3) with 0.120 M LiOH and given the inf...
Consider a the titration of 2.5 M sulfurous acid (H2SO3, Ka1 = 1.5e-2, Ka2 = 1.0e-7) with 2.0 M NaOH. What is the pH at the first halfway point of the titration? What is the pH at the second halfway point of the titration? What is the pH at the equivalence point of the titration?
Consider the titration of 25.00 mL of 0.200 M methyl amine (CH3NH2). The titrant is 0.120 M HCl. Calculate each of the following: a. the volume of added acid required to reach the equivalence point. b. the pH at ½ the HCl needed to reach the equivalence point c. the pH at the equivalence point.
Consider the titration of a 25.0 -mL sample of 0.110 M HC2H3O2 with 0.120 M NaOH. Determine each of the following. Part A the initial pH Part B the volume of added base required to reach the equivalence point Part C the pH at 6.00 mL of added base Part D the pH at one-half of the equivalence point Part E the pH at the equivalence point
The next 9 questions are related to the titration of 20.00 mL of a 0.0700 M acetic acid solution with 0.0950 M KOH. What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration (in mL)? How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) What is the volume of the solution at the equivalence point (in mL)? What is...
What is the pH in a titration of 125 mL of 0.45 F sulfurous acid (H2SO3) with 1.23 M solution of sodium hydroxide after 15 mL of base have been added?
In the titration of a solution of weak monoprotic acid with a 0.1275 M solution of NaOH, the pH half way to the equivalence point was 4.48. In the titration of a second solution of the same acid, exactly twice as much of a 0.1275 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration? In the titration of a solution of weak monoprotic acid with...
The next 9 questions are related to the titration of 25.00 mL of a 0.1000 M acetic acid solution with 0.1000 M KOH. 1.What is the initial pH of the analyte solution? 2.What volume of KOH is required to reach the equivalence point of the titration (in mL)? 3.How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) 4.What is the volume of the solution at the equivalence point (in mL)? 5.What is...
In the titration of a solution of weak monoprotic acid with a 0.1800 M solution of NaOH, the pH half way to the equivalence point was 4.42 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1800 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
In the titration of a solution of weak monoprotic acid with a 0.1525 M solution of NaOH, the pH half way to the equivalence point was 4.40 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1525 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
These questions are related to the titration of 40.00 mL of a 0.0850 M acetic acid solution with 0.0700 M KOH. Assume that the temperature is 25 oC. The volume of KOH required to reach the equivalence point of the titration is 48.57 mL, the number of mmol of acetate present at the equivalence point is 3.40 mmol, the total volume of the solution at the equivalence point is 88.57 mL and the analytical concentration of acetate ions at the...