6) 15 mL of 0.325 M NaOH is delivered into a 35 mL HOBr solution of...
4) 5.65 mL of 0.23 M Ba(OH)2 is delivered while titrating of 28.0 mL of 0.390 M HCN. The volumes are additive and the temperature of the solution is 25°C. Ka for hydrocyanic acid is 6.2 x 100. a. How many moles of OH were added? b. Find [H] in the final solution. (Hint: You could find pH first, then [H'] from pH.) C. Find [OH] in the final solution. (Hint: Use Kw)
6) A 35 mL solution of 0.241 M HCl is titrated with 0.127 M NaOH: a) How many milliliters of NaOH solution are required to reach the equivalence point? b) What is the pH at the midpoint of the titration? c) What is the pH at the endpoint of the titration?
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of unknown molarity starts at a buret reading for NaOH of 0.33 mL The phenolphthalein indicator turns light pink the acid solution for over 30 seconds at a buret reading of 24.19 mL 2) What was the volume of HCl you started with? 3) How many moles of HCl were in the original solution? 4) Write the balanced chemical equation for the titration reaction. 5)...
For 300.0 mL of a buffer solution that is 0.325 M in CH3CH2NH2 and 0.300 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.005 mol of NaOH.
167 mL of 4.7 M HBr solution is mixed with 176 mL of NaOH solution of unknown concentration. The H+ concentration in the final solution is 0.09M. What was the NaOH concentration of the unknown solution?
Question two A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
10.00 mL Nitric acid was titrated with NaOH of 0.100 molarity until the equivalence was reached. 15.2 mL of NaOH were required. Find: A) Concentration of nitric acid before titration B) pH of solution before titration C) pH of solution after 15.1 mL of sodium hydroxide is added D) pH of solution after 15.3 mL of sodium hydroxide is added
Titration of 5.00 mL of a solution labeled 0.237 6 M HCI requires addition of 40.02 mL of an NaOH solution to reach the equivalence point. 1. How many moles of HaO were used in the titration? 2. At the equivalence point, how many moles of OH had been added? 3. Calculate c in the titrant. OH in the OH 4. Another 1.00 mL of the NaOH solution is added after the equivalence point. Calculate c reaction mixture.
Concentration 1.00 M of NaOH Volume of Solution 2.5 mL added to solution 4.0 mL added to solution 2.00 M of Caci, 2.0 mL added to solution 0.75 M of K,POL Each of these three solutions are mixed into a beaker, find the molarity of each of the three individual solutions in the entire solution.
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]