The addition of ________ mL of 0.2000 M NaOH is required to titrate 40.00 mL of 0.2000 M HCl to the equivalence point, which occurs at a pH of ________.
The addition of ________ mL of 0.2000 M NaOH is required to titrate 40.00 mL of...
a) 28.3 mL of a 0.200 M NaOH solution is required to titrate a 200.0 mL sample containing HCl to its equivalence point. What was the concentration of HCl in the solution with which you started? b)The pH of blood is = 7.4. What is the concentration of OH- ions?
We’re going to titrate formic acid with the strong base, NaOH. There is initially 100. mL of 0.50 M formic acid and the concentration of NaOH is 1.0 M. What is the initial pH of the formic acid solution? 2) What is the percent ionization under initial conditions? 3) After the addition of 10 mL of NaOH, what is the pH? 4) After the addition of 25 mL of NaOH, what is the pH? Think about where in the titration...
3. In the lab you are going to titrate a weak acid solution (25.00 mL of 0.100 M HCHO2, formic acid) with a strong base (0.100 M NaOH). Carry out the following calculations to determine the pH for four key points throughout the titration. Part a. Calculate the volume of 0.100 M NaOH required to reach the equivalence point for the titration. Ans. 25.00 mL Part b. Calculate the initial pH of 0.100 M HCHO2 (before adding any NaOH). Ans....
4. Suppose you titrate 50.00 mL of 1.20 M pyridine, C5H5N, with 0.634 M HCl. (a) How many moles of pyridine are present in the original pyridine solution? (b) What is the initial pH? (c) What volume (in mL) of HCl solution is required to reach the equivalence point? (d) What is the pH at the equivalence point? (e) What is the pH of the solution after the addition of 104 mL of HCl?
4. Suppose you titrate 50.00 mL of 1.20 M pyridine, C5H5N, with 0.634 M HCl. (a) How many moles of pyridine are present in the original pyridine solution? (b) What is the initial pH? (c) What volume (in mL) of HCl solution is required to reach the equivalence point? (d) What is the pH at the equivalence point? (e) What is the pH of the solution after the addition of 104 mL of HCl?
What volume (in mL) of 0.1899 M NaOH is required to titrate 15.00 mL of 0.1559 M HAc to the equivalence point? (give your answer to 2 decimal places)
How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 × 10-8.
You titrate 50.0 mL of 0.400 M HClO4 (a strong acid) with 0.400 M NaOH. a. Write the balanced equation. b. What is the pH at the beginning of the titration (0.0 mL of NaOH)? c. What is the pH after adding 30.0 mL of NaOH? d. At the equivalence point, is the pH greater than, less than, or equal to 7.00? Explain briefly.
How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of 0.0990 M HBr to the equivalence point?
You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the limiting reactant?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final [H3O+]?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final pH of the solution?