ANSWER NUMBER 9 ONLY
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PH Ht! B C mL of titrating reagent in buret → 9. For the titration of 100.0 mL of 0.0500 M NH...
Sketch a titration curve for the titration of 25.0 mL of 0.100 M NaOH with 0.0500 M HCl. Locate the equivalence point for each of the titration curves in problem 1.
• example: Titration of 100.0 mL of 0.05 M NH3 with 0.10 M HCI • Calculate equivalence point volume • Calculate pH at the following volumes of acid added • 10.0 mL • 25.0 mL • 50.0 mL • 60.0 mL • Check your answers against the titration curve
3) The following plot shows two titration curves, each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. Use this graph for question 3a. [12 pts] 14 10 3 6 4 2 0 0 200 40.0 60.0 30.0 100.0 ml of 0.100 M Nadded a. i) Which point, a-d, represents the equivalence point for the titration of a weak acid? [2 pts] ii) Which point, a-d, represents the equivalence point for the titration of a...
Q2 Part B What is the pH at the equivalence point in the titration of 100.0 mL of 0.0500 M HOCI (Ka = 3.5 x 10-8) with 0.400 M NaOH? Express your answer to two decimal places. ΤΕΙ ΑΣΦ ? pH = 19.76 Submit Previous Answers Request Answer X Incorrect; Try Again A certain weak acid, HA, with a Ka value of 5.61 x 10-6, is titrated with NaOH. Part A A solution is made by titrating 8.00 mmol (millimoles)...
Consider the titration of 40.0 mL of 0.500 M NH, with 1.00 M HC a) What is the initial pH of the NHg(aq)? b) What is the pH halfway to the equivalence point? c) What is the volume of HCI needed to reach the equivalence point? What is the pH at the equivalence point? d) Sketch the titration curve. Label the point(s) where there is a A) a weak base B) weak acid C) Buffer D) Strong acid in excess,...
Consider the titration of 100.0 mL of 0.100 M /hydrazine () by 0.200 M . Assume that hydrazine is monoprotic. Determine the following: a. pH before any HNO3 is added b. volume of acid to reach the equivalence point c. pH when 20.0 mL of HNO3 has been added d. pH when 25.0 mL of HNO3 has been added e. pH when 40.0 mL of HNO3 has been added f. pH when 50.0 mL of HNO3 has been added g....
Part A What is the pH at the equivalence point in the titration of 100.0 mL of 0.0500 M HOCI (K. = 3.5 x 10-) with 0.150 M NaOH? Express your answer to two decimal places. IVO AED ? pH = 5.0 Submit Previous Answers Request Answer X Incorrect; Try Again Provide Feedback Next >
Sketch a pH titration curve if 100.0 mL of 0.125 M NH3 solution is titrated with 0.15M HCl. Note the following three items on the curve. K, for NHa 1.8 x 105 pH= Calculate the starting pH (no HCl added) vol (mL)= Calculate the volume of HCl added to reach the equivalence point pH = Calculate the pH at the equivalence point.
Consider the titration of 100.0 mL of 0.100 M methylamine (CH3NH2) with 0.500 M HNO3. Calculate the pH at the following volumes of acid added. For CH3NH3+, pKa = 10.632 (a) Find the equivalence point volume. (b) 0 mL (c) 9.0 mL (d) 10.0 mL (e) 20.0 mL (f) 30.0 mL
Which titration has an equivalence point with a basic pH? (A) titrating HCIO (aq) with Ca(OH)-(aq) (B) titrating HNO-(aq) with KOH(aq) (C) titrating HNO,(aq) with KOH(aq) (D) titrating NHs(aq) with HCl(aq) 12. 13. Identify and justify the Brønsted-Lowry acid in the reaction: NH, +HBr NH,Br (A) HBr because it is a proton donor (B) HBr because it is a proton acceptor (C) NH, because it is a proton donor (D) NH, because it is a proton acceptor 14. Which is...