buffer solution practice problems with answers

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| By Catherine Halcomb
Catherine Halcomb
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| Attempts: 1,204 | Questions: 15
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1. Which of the following is TRUE?

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About This Quiz
Buffer Solution Practice Problems With Answers - Quiz

How good are you at solving buffer solution practice problems? Here, we have a few questions with answers based on the buffer solution in the quiz below. Give... see moreit a try and check how good your problem-solving skills are. A buffer solution is an aqueous solution consisting of a weak acid and its conjugate base. The quiz below will ask you to calculate the pH of chemical compounds using the Henderson–Hasselbalch equation. Can you do so? Play the quiz and assess yourself.
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2. In a water molecule, hydrogens are partially ___, oxygens are partially  ____

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3. Which of these non-covalent bonds in biological systems is usually the weakest? 

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4. Which of the following would be the strongest acid?

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5. Calculate the pH of the following aqueous solutions: 1*10^-3M HCl

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6. Calculate the pH of the aqueous solutions 1*10^-4M NaOH

Explanation

The correct answer is pH=10. A 1*10^-4M NaOH solution is a weak base. When NaOH dissolves in water, it dissociates into Na+ and OH- ions. The OH- ions combine with water molecules to form hydroxide ions (OH-) and the concentration of OH- ions increases. Since OH- ions are responsible for the basicity of a solution, an increase in their concentration results in a higher pH value. A pH of 10 indicates that the solution is slightly basic.

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7. An aqueous solution containing a concentration of 2.5*10^-8 M NaOH will have a PH; which of the following?

Explanation

The pH of the solution, containing a concentration of 2.5×10−8 M2.5×10−8M NaOH, is around 6.40. This pH level indicates a slightly acidic nature, as it is lower than the neutral pH of 7.0. The calculation involves assessing the concentration of hydroxide ions in the solution.

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8. Using the Henderson - Hasselbalch Equation, Convince yourself that the proper ratio of A / HA for pH 7.00 PKA =7.20 calculate [HPO4^-2]/[h2po4-]

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9. Using the henderson-hasselbalch equation calculate PH when 0.7 mol of NaOH is added pka=4.76 , 0.7 mol of acetic acid react  

Explanation

The Henderson-Hasselbalch equation is used to calculate the pH of a solution when a weak acid and its conjugate base are present. In this case, acetic acid (a weak acid) reacts with sodium hydroxide (a strong base) to form sodium acetate and water. The pKa value of acetic acid is given as 4.76. By using the Henderson-Hasselbalch equation, the pH can be calculated using the equation pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base (sodium acetate) and [HA] is the concentration of the weak acid (acetic acid). The equation can be rearranged to calculate the concentration of the conjugate base, [A-]. Since 0.7 mol of acetic acid reacts, the concentration of the conjugate base is also 0.7 mol. Plugging these values into the equation, the pH is calculated to be 5.13.

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10. Using the Henderson-Hasselbalch equation, calculate PH when 0.5 mol of NaOH is added pka=4.76 , 0.5 mol of acetic acid react  

Explanation

The Henderson-Hasselbalch equation is used to calculate the pH of a solution containing a weak acid and its conjugate base. In this case, acetic acid (CH3COOH) is a weak acid and its conjugate base is acetate (CH3COO-). When NaOH is added, it reacts with acetic acid to form water and sodium acetate. Since NaOH is a strong base, it completely reacts with acetic acid, resulting in the conversion of 0.5 mol of acetic acid to 0.5 mol of acetate. The pKa value given (4.76) is the logarithmic acid dissociation constant of acetic acid. By using the Henderson-Hasselbalch equation, the pH can be calculated as the pKa value, which is 4.76.

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11. All of the above examples on buffer in vitro except? 

Explanation

The given options are examples of buffers used in vitro. TRIS, Zwitterions, and phosphate buffer system are all commonly used in laboratory settings to maintain a stable pH. However, carbonic acid is not typically used as a buffer in vitro. It is a weak acid that exists in equilibrium with bicarbonate ions in the body, playing a role in maintaining blood pH. Therefore, the correct answer is carbonic acid.

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12. Which of the following statements is FALSE?

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13. Using the Henderson-Hasselbalch equation calculate PH when 0.3 mol of NaOH is added pka=4.76 , 0.3 mol of acetic acid react  

Explanation

The Henderson-Hasselbalch equation is used to calculate the pH of a solution containing a weak acid and its conjugate base. In this case, acetic acid (CH3COOH) is the weak acid and its conjugate base is acetate (CH3COO-). When NaOH is added, it reacts with acetic acid to form water and sodium acetate. The equation to calculate pH using the Henderson-Hasselbalch equation is pH = pKa + log([A-]/[HA]), where pKa is the acid dissociation constant, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. Given that 0.3 mol of acetic acid reacts, the concentration of acetic acid is reduced by 0.3 mol, while the concentration of acetate is increased by 0.3 mol. Plugging these values into the equation, we get pH = 4.76 + log(0.3/0.3) = 4.76 + log(1) = 4.76. Therefore, the correct answer is 4.76.

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14. Which of the following identifies a good buffer?

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15. Using the Henderson-Hasselbalch equation calculate PH when 0.1 mol of NaOH is added pka=4.76 , 0.1 mol of acetic acid react  

Explanation

The Henderson-Hasselbalch equation is used to calculate the pH of a solution containing a weak acid and its conjugate base. In this case, acetic acid (CH3COOH) is a weak acid and NaOH is a strong base. When NaOH is added, it reacts with acetic acid to form water and sodium acetate (CH3COONa). The reaction consumes the acetic acid, causing a decrease in the concentration of the weak acid. As a result, the pH of the solution decreases. The pKa value of 4.76 indicates that the solution is slightly acidic. Among the given options, the closest pH value to an acidic solution is 3.81, which is the correct answer.

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Which of the following is TRUE?
In a water molecule, hydrogens are partially ___, oxygens are...
Which of these non-covalent bonds in biological systems is usually the...
Which of the following would be the strongest acid?
Calculate the pH of the following aqueous solutions: 1*10^-3M HCl
Calculate the pH of the aqueous solutions 1*10^-4M NaOH
An aqueous solution containing a concentration of 2.5*10^-8 M NaOH...
Using the Henderson - Hasselbalch Equation, Convince yourself that the...
Using the henderson-hasselbalch equation calculate PH when 0.7 mol of...
Using the Henderson-Hasselbalch equation, calculate PH when 0.5 mol of...
All of the above examples on buffer in vitro except? 
Which of the following statements is FALSE?
Using the Henderson-Hasselbalch equation calculate PH when 0.3 mol of...
Which of the following identifies a good buffer?
Using the Henderson-Hasselbalch equation calculate PH when 0.1 mol of...
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