Question

What happens when small amounts of acid or base are added to a buffer solution? What...

What happens when small amounts of acid or base are added to a buffer solution? What would happen if these solutions were not buffered? What conclusions can you draw about buffer solutions?  

Homework Answers

Answer #1

Ans- A buffer solution is such a solution which has a tendency to resist change in pH when small amounts of acid or base are added to it.

So as per the definition itself, an adding amount of acid and base, the pH of buffer solution generally remains same or changes very little.

If the solution were not buffer, on adding acid it's pH would have decreased and on adding base it's pH would have increased.

So we draw rhe conclusion that buffer solution actually helps in resisting change in pH and has a vast number applications in our day to day life. Example- blood is a buffer.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A buffer contains significant amounts of a weak acid and its conjugate base. The acid consumes...
A buffer contains significant amounts of a weak acid and its conjugate base. The acid consumes any added base, and the base consumes any added acid. In this way, a buffer resists pH change. Part A Which set of compounds would form a buffer in aqueous solution? NaF and NaOH NaF and KF HCN and NaCN HF and KF HCl and HClO HBr and NaBr HF and KCN NaCl and KCl Please say if they are a buffer or not...
A buffer contains significant amounts of a weak acid and a salt containing its conjugate base....
A buffer contains significant amounts of a weak acid and a salt containing its conjugate base. The acid consumes any added base, and the base consumes any added acid. In this way, a buffer resists pH change. Strong acids, strong bases, two bases, or two acids cannot form a buffer on their own. Part A Which set of compounds would form a buffer in aqueous solution? HF and KCN HCl and KCl NaCl and KCl NaBr and KBr HCOOH and...
When the Sorensen’s buffer was prepared, equal amounts of the acid and base forms of the...
When the Sorensen’s buffer was prepared, equal amounts of the acid and base forms of the buffer system should have been present. However, you likely found that the pH was not equal to the pKa of the buffer. What likely caused this discrepancy?
When a solution contains a weak acid and its conjugate base or a weak base and...
When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base is...
When a solution contains a weak acid and its conjugate base or a weak base and...
When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base is...
Prepare a buffer by acid–base reactions. Consider how to prepare a buffer solution with pH =...
Prepare a buffer by acid–base reactions. Consider how to prepare a buffer solution with pH = 9.31 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.316-M solution of weak acid with 0.351 M potassium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the potassium hydroxide solution would have to be added...
A buffer is a mixed solution of a weak acid or base, combined with its conjugate....
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift...
Prepare a buffer by acid–base reactions. Close Problem Consider how to prepare a buffer solution with...
Prepare a buffer by acid–base reactions. Close Problem Consider how to prepare a buffer solution with pH = 9.31 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.316-M solution of weak acid with 0.351 M potassium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the potassium hydroxide solution would have to...
explain the buffer mechanism in terms of the common-ion effect when strong acid HCl and base...
explain the buffer mechanism in terms of the common-ion effect when strong acid HCl and base NaOH are added to the acetic/ sodium acetate buffer solution
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base...
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the addedH+, forming more...