In the titration of 25.00 ml of 0.10 M HF with 0.10 M NaOHn given ka = 3.5 x 10-4 find
initial PH, PH at the equivalence point and Ph at half equivalence point
In the titration of 25.00 ml of 0.10 M HF with 0.10 M NaOHn given ka...
QUESTION 9 Calculate the pH during the titration of 25.00 ml of 0.1000 M HF(aq) with 0.1000 M ROH(aq) after 9 mL of the base have been added. Ka of HF = 7.4 x 10-4
A titration is performed on 50mL of a 0.10 M solution of HN3 (Ka+1.9x10-5) with 0.10 M NaOH as the titrant. (a) What is the initial pH of the HN3 solution? (b) Calculate the pH of the solution after 25 ml of NaOH have been added (c) How many mL of NaOH are required to reach the equivalence point and what is the pH of the solution at the equivalence point.
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.22 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 18.34 4.06 Equivalence point 36.68 8.84 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following...
(3) 30.00 mL of 0.085 M Hydrofluoric acid (HF) is titrated with 0.10 M NaOH. What is the pH of the acid solution before any base is added? (Ans: pH = 2.11) What is the pH of the titration mixture at half the equivalence point? (Ans: pH = 3.35) What is the pH of the titration mixture at the equivalence point? (Ans: pH = 7.92) What is the pH of the mixture after 40.00 mL of base are added? (Ans:...
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...
Find the pH of a mixture that is 0.150 M HF and 0.10 M HClO. Ka = 3.5 x 10^-4.
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
Titration of 25.00 mL of an unknown diprotic acid solution required 15.09 mL of 0.10 M NaOH to reach the first equivalence point and 29.82 mL of 0.10 M NaOH to reach the second equivalence point. What is the concentration of the diprotic acid solution?
In the titration of 50.0 ml of 0.200 M Sulfurous Acid (H2SO3) with 0.120 M LiOH and given the information below, answer the following questions. 1. Ka,-1.7 x 10-2 Ka2- 6.4x 10-8 SO32- H+(aq) ← → HISO3_ (ag) + (ag) What is the initial pH of the analyte (sulfurous acid)? a. or What is the pH at the first equivalence point of the titration? b. What is the pH at the first half-way point of the titration? c. What volume...