Question

Which of the following represents a buffer system? Explain.

a. $\mathrm{NaOH}$and$\mathrm{NaCl}$

b. ${\mathrm{H}}_2{\mathrm{CO}}_3$and${\mathrm{NaHCO}}_3$

c. $\mathrm{HF}$and$KF$

d. $\mathrm{KCl}$and$\mathrm{NaCl}$

Short answer

(Part a) The mixture $NaOH$and $NaCI$$\&$$KCI$and $NaCI$are not a buffer systems.

(Part b) The mixture ${\mathrm{H}}_2{\mathrm{CO}}_3$and ${\mathrm{NaHCO}}_3$$\&$$HF$and $KF$are a buffer systems.

Step-by-step solution

Step 1- Introduction (Part a)

A buffer system is a solution that withstands changes in $pH$ when an acid or base is added. The acidic solution contains a high concentration of hydrogen ions $(H+)$and has a $pH$ value of less than $7$. The basic solution contains a high concentration of hydroxide ions $\left(OH\right)$ and has a pH value above $7.$

Step 2- Explanation (part a)

a.

The solution of strong base and its salt is completely ionized. Therefore, the $NaOH$ and $NaCl$ solutions are not buffer systems.

Step 3- Explanation (part b)

b.

The mixture contains weak acid $H_2{CO}_3$ and its salt ${\mathrm{NaHCO}}_3$. Therefore, the solution of $H_2{CO}_3$and ${\mathrm{NaHCO}}_3$ is a buffer system.

Step 4- Explanation (part c)

c.

The mixture contains the weak acid $HF$ and its salt $KF.$ Therefore, the mixture of $HF$ and $KF$ is a buffer system.

Step 5- Explanation (part d)

d.

Both substances are salts. The mixture does not contain weak acids. Therefore, a mixture of $KCl$ and $NaCl$ is not a buffer.