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)...
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 of 0.114 M HCl is needed to titrate 25.0 mL of 0.172 M pyridine (C5H5N) to its equivalence point? For pyridine, pKb = 8.77.
A titration of 60.0mL of 0.30M pyridine, C5H5N, required 90.0mL of 0.20 M HCl to reach the equivalence point. What is the pH at this equivalence point? Kb(C5H5N) = 2.0x10^-9
The following 8 questions are related to the titration of 153.0 mL of 0.276 M A with 0.698M HCI at 25°C. (K, of A = 2.18E-4, A is a monoprotic base) 1. What would you estimate the initial pH of A to be prior to the addition of any acid? Choose one. A) pH = 7 B) pH is less than 7 C) pH is greater than 7 2. What is the pH after the addition of 15.3 mL of...
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...
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Consider the titration of 30.0 mL of 0.170-M of KX with 0.110-M HCl. The pKa of HX = 7.42. Give all pH values to 0.01 pH units. a) What is the pH of the original solution before addition of any acid? b) How many mL of acid are required to reach the equivalence point? c) What is the pH at the equivalence point? d) What is the pH of the solution after the addition of 26.4 mL of acid? e)...
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1))))Weak Base Titration: At the Equivalence Point a))A 11.30 mL solution of 2.47 M pyridine (C5H5N, a weak base) is titrated to the equivalence point with 22.4 mL of HNO3. What is the pH at the equivalence point? Kb for pyridine is 1.7 X 10-9. b))))Click on all of the dominant species that you would expect to find in solution at the equivalence point. Do not include H3O+ and OH-ions unless they are coming from another source other than the...