Which of the following statements is TRUE? At pH = 9, [CH3COOH] would be a lot...
Which of the following statements is TRUE?
| At pH = 9, [CH3COOH] would be a lot lower than [CH3COO-] |
| At pH = 2, [CH3COO-] would be dominant, compared to [CH3COOH] |
| The ratio of concentration of acetate to acetic acid in a solution would go up as pH goes down. |
| At pH = 4.76, [CH3COO-] = 2 * [CH3COOH] |
Homework Answers
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Which of the following statements is TRUE?
At pH = 9, [CH3COOH] would be a lot...
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For the following dissociation of acetic acid, Ka = 1.760 x 10-5: CH3COOH + H2O ? CH3COO- + H3O+ Sodium acetate completely dissociates in solution according to the following reaction: NaCH3COO ? Na+ + CH3COO- A solution was prepared which contains CH3COOH at a pre-equilibrium concentration of 0.05782 M and NaCH3COO at a pre-equilibrium concentration of 0.04991 M. I know all answers, just do not know how to find them. What is the equilibrium concentration of H3O+? (Answer: 0.00002037) What...
What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10...
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What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...
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1. Calculate the pH of IL solution to which 5.OmL of 1.0 Macetic acid and 5.OmL of 0.5M sodium acetate have been added. The pKa of acetic acid is 4.76. 2. You need to carry out an enzymatic reaction at pH-3.5. A friend suggests phosphate buffer with pka of 7.21 as the basis of a buffer. Will this be a good choice to make the suitable buffer? Why or why not? 3. Calculate the concentration of acetate in a 100mM...
what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M...
what concentration of acetic acid (pka=4.76) and acetate would be
required to prepare a .15 M buffer solution at pH 5.0?
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What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water) A. The concentration of CH3COOH will decrease. True False B. The concentration of CH3COO" will remain the same C. The equilibrium concentration of H30* will increase D. The pH will increase E. The ratio of [CH3COOH]/ [CH3coo]...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.92 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [ A HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate...
Which of the statements below is/are true of your solution at equivalence? Select all true statements below. The concentration of acetate ions (CH2C00) at equivalence is the same as the original concentration of acetic acid (CH2COOH) at the start of the titration (i.e. 1.0 M). The number of moles of acetate ions (CH3COO") at equivalence is the same as the number of moles of of acetic acid (CH2COOH) at the start of the titration (i.e. 0.10 mol). At the equivalence...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...
1. Calculate the pH of IL solution to which 5.OmL of 1.0 Macetic acid and 5.OmL of 0.5M sodium acetate have been added. The pKa of acetic acid is 4.76. 2. You need to carry out an enzymatic reaction at pH-3.5. A friend suggests phosphate buffer with pka of 7.21 as the basis of a buffer. Will this be a good choice to make the suitable buffer? Why or why not? 3. Calculate the concentration of acetate in a 100mM...
what concentration of acetic acid (pka=4.76) and acetate would be
required to prepare a .15 M buffer solution at pH 5.0?
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
A 1.00 liter solution contains 0.35M acetic acid and 0.26 M potassium acetate. If 35.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water) A. The concentration of CH3COOH will decrease. True False B. The concentration of CH3COO" will remain the same C. The equilibrium concentration of H30* will increase D. The pH will increase E. The ratio of [CH3COOH]/ [CH3coo]...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.92 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [ A HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate...
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