Please answer these 5 questions.
1) a buffer is made by dissolving (CH3NH3)Cl and CH3NH2 in water. Write equations to show how this buffer neutralizes added H3O+ and OH-.
2) If you add 15.0 mL of 1.25 M NaOH to 250. mL of a 0.200 M propanoic acid (CH3CH2CO2H) solution, what is the pH of the resulting solution?
3)If added to 500. mL of 0.20 M NaOH, which of these
would form a biffer? Briefly, justify your decision for each and
every option below.
(a) 0.050 mol CH3COOH
(b) 0.15 mol CH3COOH
(c) 0.10 mol CH3COOH
(d) 0.050 mol HCl
(e) 0.15 mol Na CH3COO
4) Suppose you titrate 0.0300 L of 0.100 M HClO4 with
0.0750 M KOH. Calculate the pH after the addition of the following
volumes of KOH solution.
(a)
0.0 mL
(b)
25.0 mL
(c)
40.0 mL
(d)
55.0 mL
What might be a good indicator to use in order to detect the
endpoint of this titration?
5) Suppose you titrate 0.0450 L of 0.200 M
trimethylamine (CH3)3N with 0.300 M HNO3. Calculate the pH after
the addition of the following volumes of HNO3 solution.
(a) 0.0 mL
(b) 10.0 mL
(c) 30.0 mL
(d) 45.0 mL
What might be a good indicator to use in order to detect the
endpoint of this titration?
Please answer these 5 questions. 1) a buffer is made by dissolving (CH3NH3)Cl and CH3NH2 in...
1) A buffer can be prepared by mixing two solutions. Determine if each of the following mixtures will result in a buffer solution or not. 1) Mixing 100.0 mL of 0.1 M HCl with 100.0 mL of 0.1 M NaOH [ Select ] ["No, it will not result in a buffer solution.", "Yes, it will result in a buffer solution."] 2) Mixing...
Answer all assigned questions and problems, and show all work. Determine the pH of (a) a 0.40 MCH3CO2H solution, (b) a solution that is 0.40 MCH3CO2H and 0.20 MNaCH3CO2. (8 points) (Reference: Chang 16.5) Which of the following solutions can act as a buffer? (a) KCl/HCl, (b) KHSO4/H2SO4, (c) KNO2/HNO2.(5 points) (Reference: Chang 16.9) Calculate the pH of the buffer system made up of 0.15 MNH3/0.35 MNH4Cl. (5 points) (Reference: Chang 16.11) The pH of a bicarbonate-carbonic acid buffer is...
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.
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...
Part B: A 50.0 mL volume of 0.15 mol L−1 HBr is titrated with 0.25 mol L−1 KOH. Calculate the pH after the addition of 14.0 mL of KOH. Express your answer numerically. Part C: A 75.0 mL volume of 0.200 mol L−1 NH3 (Kb=1.8×10−5) is titrated with 0.500 mol L−1 HNO3. Calculate the pH after the addition of 28.0 mL of HNO3. Express your answer numerically. Part D: A 52.0 mL volume of 0.350 mol L−1 CH3COOH (Ka=1.8×10−5) is...
1) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 16.0 mL of KOH.Express your answer numerically. pH=_______ 2) A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3.Express your answer numerically. pH=_______ 3) A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x10-5 ) is titrated with 0.40 M NaOH. Calculate...
3] You are charged with producing a buffer with a pH 7.65, by dissolving a weighed amount of sodium hypochlorite (NaCIO, FM-74.44) in 1.5 L of 0.35 M hypchlorous acid (HOCI, pka 7.46) (a) What mass (in g) of NaCIO is required (4 points (b) What is the resulting pH if 20 mL of 0.08 M HCI is added to 80 mL of this buffer? (4 points (c) Could i make a second NaCIO/HOCl buffer with a pH = 5.0?...
5. A buffer is made up of 355 ml each of 0.200 M NaHCO, and 0.134 M Na,CO3. Assuming that volumes are additive and the k, = 4.7 x10-1 calculate: a) the pH of the buffer b) the pH of the buffer after the addition of 0.0300 moles of HCI to 0.710 liters of buffer. c) the pH of the buffer after the addition of 0.300 moles of KOH to 0.710 liters of buffer.
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
-e-laboratory Assignment Name: ead the experiment and answer the following questions as directed by your instructor A student is performing a titration. Diagrams of the buret at the beginning and the end of the titration are shown at right. To the correct number of significant figures, what is the initial volume, the final volume, and the volume of solution added during the titration? 16 2) Formic acid (HCOOH) is a weak acid with K. - 1.8 x 10-4. a) Write...