concentration (HCl) = 0.0837
volume used ( from graph ) = 21 ml
volume of ammonia used = 35 ml
conc ( ammonia ) = ( 0.0837 * 21 ) / 35
= 0.050 M
This graph shows the titration of 35.0 mL of ammonia solution with a 0.0837 M HCI....
Titration of ammonia with HCl This graph shows the titration of 35.0 mL of ammonia solution with 0.0760 M HCl. Determine the molarity of the ammonia solution. concentration: pH 0 1 2 3 4 5 6 7 8 9 16 17 18 19 20 21 22 23 24 25 26 27 10 11 12 13 14 15 vol HCl (mL)
Titration of ethylamine with HCl This graph shows the titration of 35.0 mL of ethylamine solution with 0.0773 M HCl. Determine the molarity of the ethylamine solution. concentration: pH HH 11 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 vol HCl (mL)
This graph shows the titration of 15.0 mL of ethylamine solution with 0.0954 M HCI. Titration of ethylamine with HCI Determine the molarity of the ethylamine solution. concentration:
Titration of methylamine with HCI This graph shows the titration of 20.0 mL of methylamine solution with 0.0979 M HCI. Determine the molarity of the methylamine solution. concentration: WWW
This graph shows the titration of 20.0mL of ammonia solution with a 0.0860 M HCL. Determine the molarity of the ammonia solution.
3. A titration curve and a first derivative graph are given on the next page for the titration of a weak base with HCL Use these graphs to answer parts (a)- (c). a. Calculate the initial molarity of B. b. Determine the pK for B at 20.0°C. Show your work on the graph and in the space below. Based on your answer to (b), which base (ammonia, methylamine, or morpholine) was titrated with HCI? c d. Calculate K for the...
This graph shows the titration of 25.0 mL of methylamine solution with a 0.0798 M HCl. Determine the molarity of the methylamine solution.
8. A titration of 15 mL of ammonia (NH3) required 38.57 mL of 0.78 M HCI. What is the molarity of ammonia?
heading Harding 2 A Student added 49.6 mL of 0.73 M solution of HCl to a beaker. The student then added 50 mL of DI water to the beaker. The HCl was titrated with 1248 ml of 0.73 M N O solution without reaching the equivalence point. Answer questions 21 - 25 with this information 21. How many moles of HCl are in the initial solution? (3 pts) 22. What is the molarity of the initial HCl solution after adding...
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...