Pls answer 12 & 13 11. What effect will addition of excess of HCI have on the pH of a solution of NH3?a. increase the pHb. decrease the pHC. no effectd. cannot tell from information given> Answer and brief explanation:12. A buffer solution may be a mixture ofa. a weak acid and its saltb. a weak base and its saltC. an excess of a weak acid with a strong based. all of the above> Answer and brief explanation:13. The ammonium ion would be classified as a Bronsteda. acidb. base> Answer and brief explanation:

Few questions based on equilibrium concept, which is to be accomplished.

Answered: 12. A buffer solution may be a mixture…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter20: Acidity And Pka Of Phenols

Section: Chapter Questions

Problem 3CTQ

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a). What are acids, bases and buffers?b) What are the different types of buffers? Describe the mechanism howbuffers resist pH change in a system.c) Elaborate all chemical reactions in the standardization of NaOH withKHP?d) Why do you need to use KHP in the standardization of NaOH?e) Why is phenolphthalein used as an indicator in this experiment?f) Compare and contrast: endpoint vs equivalence point.g) Discuss the role of acids, bases, buffers and pH in water qualitymonitoring and post-harvest fisheries.
How did diluting the buffer affect the pH of the buffer solution itself? ( pls explain it asap!) Thank you
Which of the following solutions represent(s) a buffer solution? Explain.(a) 15 cm3 of 0,1 mol.dm–3 NaOH(b) 15 cm3 of 0,1 mol.dm–3 HC2H3O2(c) 30 cm3 of 0,1 mol.dm–3 NaOH and 30 cm3 of 0,1 mol.dm–3 HC2H3O2(d) 30 cm3 of 0,1 mol.dm–3 NaOH and 60 cm3 of 0,1 mol.dm–3 HC2H3O2
Did either buffer F or G reach buffer capacity? How do you know? Explain your reasoning.
Based on that experimental titration curve of the IU unknown sample, can you sketch out the titration curve if both the starting weak acid solution and the NaOH solution are diluted 10 times? What about diluting another 10 times on top of that? Particularly, you should pay attention to the size of the pH jumps around each equivalence point, as well as the relative positions of the flat regions before or after the pH jumps. For the sake of simplicity, no need to consider activity in this exercise.
Identify the buffer system(s) - the conjugate acid-base pair(s)- present in a solution that contains equal molar amounts of the following: ???3(??????????) NaOH(sodiumhydroxide) H3PO4(phosphoricacid) NaH2PO4(sodiumdihydrogenphosphate) Group of answer choices HNO3 (nitric acid) and NaOH (sodium hydroxide) HNO3 (nitric acid) and H3PO4 (phosphoric acid) NaOH (sodium hydroxide) and NaH2PO4 (sodium dihyrdogen phosphate) NaH2PO4 (sodium dihyrdogen phosphate) and NaOH (sodium hydroxide) H3PO4 (phosphoric acid) and NaH2PO4 (sodium dihyrdogen phosphate) HNO3 (nitric acid) and NaH2PO4 (sodium dihyrdogen phosphate)
I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)
H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion
Can someone please explain why and how the step 1 was done? What was its purpose? Why was only the pKa2 value was used in the second step 2? I don't understand shortcuts and I would appreciate it if it's explained step by step. This was the solution to my previous question in which I asked: What is the pH of a buffer prepared by mixing 100 mL 0.050 mM NaH2PO4 and 25 mL 0.075 mM Na2HPO4? (pKa1=2.2; pKa2= 7.21; pKa3=12.7)
How would the results of an experiment change if a basic buffer was utilized instead of an acidic one? in this experiment a strong base and strong acid are titrated agaisnt water and an acidic buffer. however, how were the reuslts differ with a basic buffer? please explain
Reorder the following steps to the correct order of preparing a buffer. 1.Weigh out the calculated dry reagents into a beaker and dissolve them with deionized water only up to 70% capacity of the total volume. 2.Use an acid or a base to adjust the pH of the solution to the required pH level. 3.Calculate the mass required to prepare all the dry reagents, specific for concentration and volume. 4.Adjust the volume of the solution to the total volume required for the buffer with deionized water.
When a buffer is used in an experiemnt does the buffer action last over the entire pH range? Why or why not? Please explain. What requires more acetate buffer to be used to reach the equivalence point a strong base or a strong acid? Please explain.

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12. A buffer solution may be a mixture of a. a weak acid and its salt b. a weak base and its salt C. an excess of a weak acid with a strong base d. all of the above Answer and brief explanation: 13. The ammonium ion would be classified as a Bronsted a. acid b. base