A student pipettes 25.00 mL of 0.150 M CH3NH2 solution into a flask, titrating the solution with 0.150 HCl.
a. what is the pH when 0.00 mL of the titrant has been added?
b. What is the pH when 25.00 mL of the titrant has been added?
A student pipettes 25.00 mL of 0.150 M CH3NH2 solution into a flask, titrating the solution...
Please workout solution, thank you! L__ of 15 points) A student pipettes 25.00 mL of 0.150 M methylamine (CH3NH2) solution into a flask, titrating the solution with 0.150 M HCI. a) What is the pH when 0.00 mL of the titrant has been added? b) What is the pH when 25.00 mL of the titrant has been added? c)Indicate which of the following indicators should be used for the titration? Indicator pKa Indicator pka Cresol red 1.5 Erythrosin B 2.9...
1. You are titrating a 100.0 mL solution of 0.050 M HBrwith a 0.150 M solution of KOH. What will be the pH after the addition of 25.0 mL KOH? 2. You titrate 250 mL of 0.250 M acetic acid (Ka= 1.8 x 10-5) with 50.0 mL of 0.350 M NaOH. What is the pH of this solution? 3. For the titration in question 2, what would be the Kaof an ideal indicator.
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...
16. Exactly 25.00 ml of 0.0685 M HClO4 solution is placed in a flask and titrated with standardized 0.050M NaOH. A. Determine the endpoint of the titration B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution: a.) Initially, 0.00 ml NaOH. b.) 5.00 ml c.) 15.00 ml d.) 25.00 ml e.) 34.00 ml f.) At the endpoint of the titration g.)...
You have 25.00 mL of a 0.100 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). 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 5.00 mL of acid has been added? (d) What is the pH of the solution...
Exactly 25.00 ml of a 0.0685 M pentanoic acid solution,(C4H8O2), is placed in a flask and titrated with standardized 0.050 M NaOH. (the pKa of this acid is 4.84). A. Determine the endpoint of the titration B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution: a.) Initially, 0.00 ml NaOH. b.) 5.00 ml c.) 15.00 ml d.) 25.00 ml e.) 34.00 ml...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.18 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 19.03 3.54 Equivalence point 38.05 8.57 How many moles of NaOH have been added at the equivalence point? mol incorrect 0/1 What is the total volume of the solution at the equivalence point? ImL incorrect 0/1 During...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.24 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 18.73 3.60 Equivalence point 37.45 8.59 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...
A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.18 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 18.77 3.83 Equivalence point 37.54 8.73 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...
i need help with pre-lab questions Pre-Lab Questions The titration curve below (on the next page) was obtained by titrating 25.00 mL of a boric acid solution with a 1.000 M NaOH solution. Use the information given on the titration curve to answer the following questions: 1. What is the formula and value of K, for boric acid? Calculate using the half equivalence data point, and using the pH at one-quarter and three-quarter points, too. What is the average Ka...