Which image represents the buffer after the addition of strong acid? Which image represents the buffer after the addition of strong base? Place the image into the appropriate category. (Note: Not all of the images will be used.) Items (4 images) (Drag and drop into the appropriate area below)

Which image represents the buffer after the addition of strong acid? Which image represents the buffer after the addition of strong base? Place the image into the appropriate category. (Note: Not all of the images will be used.) Items (4 images) (Drag and drop into the appropriate area below)

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.116E: a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium...

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Which image represents the buffer after the addition of strong acid? Which image represents the buffer after the addition of strong
base? Place the image into the appropriate category. (Note: Not all of the images will be used.)
Items (4 images) (Drag and drop into the appropriate area below)

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Similar questions

a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium lactate, C2H4(OH)COONa. b.What is the pH of a buffer that is 1M in lactic acid and 1M in sodium lactate? c.What is the difference between the buffers described in parts a and b?
All boxes. answer choices: Volume at the equivalence point, the volume at the 1/2 equivalence point, the initial pH, pH at the equivalence point, or pH at the 1/2 equivalence point.
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.
Part C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.
Part A Review Constants | Periodic Table Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH, COO). Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base: H++ CH3COO→CH3COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid: OH +…
What is a buffer?
Using the image attached please please answer question 3 & 4 Please please answer as soon as possible please
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Don't reject Please answer A and B according to this data. Data Buffer pH without adding HCL = 3.56 pH of buffer with 1 ml HCL = 2.14 pH of buffer with 2 ml HCL = 1.19 pH of buffer with 3 ml HCL = 1.41 Buffer pH without adding NaOH =2.70 pH of buffer for 1 ml NaOH = 3.87 pH of buffer for 2 ml NaOH = 4.90 pH of buffer for 3 ml NaOH = 12.50 Additional data: The buffer consists of 0.731 g of sodium acetate, 10 mL of acetic acid, and has a target pH of 4.70. A. What is the expected buffer capacity for HCL? B. What is the expected buffer capacity for NaOH?
Part C - Acid-base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO, to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system. Results Test tube…
How titration techniques can be used to determine the concentration of acetic acid in the vinegar sample? (3 sentences)
??2????3 + ??2??(??) ⇌ ??3??+ + ??????3− Explain why both acid (H2CO3) and conjugate base (HCO3-) are necessary in buffer system.