Q: Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution?

A mixture of ammonium hydroxide and \$HCl\$ react to form ammonium chloride. This also contains unreacted ammonium hydroxide.\$NH_4OH+HCl \rightarrow NH_4Cl + H_2O\$Thus, the resulting mixture of \$(NH_4OH+NH_4Cl)\$ is a basic buffer solution. It contains a mixture of weak base ammonium hydroxide and its salt (ammonium chloride) with strong acid \$(HCl)\$.It is used in a qualitative analysis of group \$III\$ radicals.A mixture of \$HNO_3\$ and \$NaOH\$ is a mixture of strong acid and strong base similarly a mixture of \$H_2SO_4\$ and \$KOH\$ is also a mixture of strong acid and strong base, thus they do not form buffer solution. Similarly, in option D mixture will form a strong base and salt of strong base weak acid hence it will not form a buffer solution.Hence, option C is correct.

Q: Match List-1 with List-2. List -1 List-2 A) Aq. Solution of NaCl 1)Acidic buffer B) Aq. Solution of \$CH_3COONa\$ 2)Acidic solution C) Aq. Solution of \$NH_{4}Cl\$ 3) Basic solution D) Aq. Solution of \$CH_{3}COOH\$ along with \$CH_{3}COONa\$ 4)Neutral solution

\$NaCl\$ is a salt of strong acid \$HCl\$ and strong base \$NaOH\$. It does not undergo hydrolysis in water. Hence its aqueous solution is neutral.Sodium acetate is a salt of strong base sodium hydroxide and weak acid acetic acid. Its solution is basic in nature.Ammonium chloride is the salt of strong acid \$HCl\$ and weak base ammonium hydroxide. Its solution is acidic in nature.A mixture of acetic acid and sodium acetate is an acidic buffer. Its aqueous solution is acidic in nature.Thus, A-4 ; B-3; C-2; D-1Hence, the correct option is \$\text{B}\$

Q: The ionic product of water changes when:

Hint:\$\text { Ionization of } \mathrm{H}_{2} \mathrm{O} \text { increases as the temperature increases. }\$Correct Answer: \$D\$Explanation:Water is a weak electrolyte and ionizes only to a small extent. water is dissociated in the following manner:\$\Rightarrow \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}^{+}+\mathrm{OH}^{-}\$.According to Le-Chatelier’s principle, as the temperature increases, the position of equilibrium shifts to the right of the equation to minimize the effect of increased temperature.This means with the increase in temperature the concentration of \$\left[\mathrm{H}^{+}\right]\$and \$\left[\mathrm{OH}^{-}\right]\$ions will increase which will result in increased value ofK \$_{w}\$ as forward reaction is favoured.Conclusion:This means that the ionic product depends only on temperature and is unaffected by any other changes.

Q: A mixture of 0.01 M \$CH_{3}COO Na\$ and \$CH_{3}COO H \$ is a acidic buffer solution.

\$CH_{3}COOH\$ is a weak acid.Read the above assertion and reason and choose the correct option regarding it.

Q: What will happen when \$CH_{3}COO Na\$ is added to an aqueous solution of \$CH_{3}COO H\$?

\$CH_{3}COOH \leftrightharpoons CH_{3} COO^{-}+H^{+}\$If \$CH_{3}COONa\$ is added, equilibrium will shift backward due to the common ion effect. \$H^{+}\$ will decrease.\$\therefore\$ pH will increase.

Question 1

Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution?

Accepted Answer

A mixture of ammonium hydroxide and $HCl$ react to form ammonium chloride. This also contains unreacted ammonium hydroxide.$NH_4OH+HCl \rightarrow NH_4Cl + H_2O$Thus, the resulting mixture of $(NH_4OH+NH_4Cl)$ is a basic buffer solution. It contains a mixture of weak base ammonium hydroxide and its salt (ammonium chloride) with strong acid $(HCl)$.It is used in a qualitative analysis of group $III$ radicals.A mixture of $HNO_3$ and $NaOH$ is a mixture of strong acid and strong base similarly a mixture of $H_2SO_4$  and $KOH$ is also a mixture of strong acid and strong base, thus they do not form buffer solution. Similarly, in option D mixture will form a strong base and salt of strong base weak acid hence it will not form a buffer solution.Hence, option C is correct.

Question 2

Blood is an example of basic buffer.

Accepted Answer

$p{H}$ of blood is 7.4

Question 3

$H_{2}O$ is a:

Accepted Answer

Hint: According to Bronsted-Lowry's theory, the compounds that have tendency to donate$ \left(\mathrm{H}^{+}\right) $ ion are acids and the compounds that have tendency to accept $\left(\mathrm{H}^{+}\right)$  ion are bases.  Explanation: A compound such as water $&#10;\left(\mathrm{H}_{2} \mathrm{O}\right)&#10;$ has many interesting properties. Water molecules can accept a proton to act as Bronsted-Lowry bases in certain circumstances. The following is an example of $&#10;\mathrm{HCl}&#10;$ dissolving in water:$\mathrm{HCl}+\mathrm{H}_{2} \mathrm{O}_{(\ell)} \rightarrow \mathrm{H}_{3} \mathrm{O}_{\text {(aq) }}^{+}+\mathrm{Cl}_{(\mathrm{aq})}^{-}$The another possibility is water can act like a Bronsted-Lowry acid by donating a proton. Water donates a proton to a proton-accepting amide ion in the presence of ammonia, resulting in the following product:$\mathrm{H}_{2} \mathrm{O}_{(\ell)}+\mathrm{NH}_{2(a q)}^{-} \rightarrow \mathrm{OH}_{(a q)}^{-}+N H_{3(a q)}$ &#10;Therefore, depending on the circumstances, $&#10;\left(\mathrm{H}_{2} \mathrm{O}\right)&#10;$ can either act as a Bronsted-Lowry acid or a Bronsted-Lowry base. There are other substances that can react either as acids or bases in certain circumstances, but water is the most common example. It is called an amphiprotic compound when it either donates or accepts a proton, depending on the situation.Final Answer: Option (C)

Question 4

In aqueous solution, the following mixture acts as buffer :

Accepted Answer

For buffer solutionWeak acid + Its salt of strong baseor Weak base + Its salt of strong acid.In Option C,$NH_{4}OH \to$ weak base$NH_{4}Cl \to$ weak base and strong acid saltThus option C is right. While no other option follow definition of buffer solution.

Question 5

Match List-1 with List-2.

List -1    List-2
A) Aq. Solution of NaCl 1)Acidic buffer
B) Aq. Solution of $C H_{3} C O O N a$    2)Acidic solution
C) Aq. Solution of $N H_{4} C l$ 3) Basic solution
D) Aq. Solution of $C H_{3} C O O H$ along with $C H_{3} C O O N a$ 4)Neutral solution

Accepted Answer

$NaCl$ is a salt of strong acid $HCl$ and strong base $NaOH$. It does not undergo hydrolysis in water. Hence its aqueous solution is neutral.Sodium acetate is a salt of strong base sodium hydroxide and weak acid acetic acid. Its solution is basic in nature.Ammonium chloride is the salt of strong acid $HCl$ and weak base ammonium hydroxide. Its solution is acidic in nature.A mixture of acetic acid and sodium acetate is an acidic buffer. Its aqueous solution is acidic in nature.Thus, A-4 ; B-3; C-2; D-1Hence, the correct option is $\text{B}$

Question 6

Which of the following solution cannot act as a buffer?

Accepted Answer

A mixture of weak acid and a salt of strong base, or a mixture of weak base and a salt of strong acid acts as a buffer.$NaH_2PO_4+H_3PO_4$ ,$CH_3COOH+CH_3COONa$ and $H_3PO_4+Na_2HPO_4$ have an acid/salt-base pair.Therefore they act as a buffer.A mixture of strong acid and its salt of strong acid don't make an effective buffer. Therefore, $HCl+NH_4Cl$ cannot act as a buffer.Hence the correct option is C.

Question 7

The ionic product of water changes when:

Accepted Answer

Hint:$\text { Ionization of } \mathrm{H}_{2} \mathrm{O} \text { increases as the temperature increases. }$Correct Answer: $D$Explanation:Water is a weak electrolyte and ionizes only to a small extent. water is dissociated in the following manner:$\Rightarrow \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}^{+}+\mathrm{OH}^{-}$.According to Le-Chatelier&#8217;s principle, as the temperature increases, the position of equilibrium shifts to the right of the equation to minimize the effect of increased temperature.This means with the increase in temperature the concentration of $\left[\mathrm{H}^{+}\right]$and $\left[\mathrm{OH}^{-}\right]$ions will increase which will result in increased value ofK $_{w}$ as forward reaction is favoured.Conclusion:This means that the ionic product depends only on temperature and is unaffected by any other changes.

Question 8

A mixture of 0.01 M $CH_{3}COO Na$ and $CH_{3}COO H $ is a acidic buffer solution.

Accepted Answer

$CH_{3}COOH$ is a weak acid.Read the above assertion and reason and choose the correct option regarding it.

Question 9

Which can act as buffer?

Accepted Answer

Buffer solution is a mixture of weak acid and its salt of weak acid.In Option C $NaCN\rightarrow$ salt of strong base and weak acid $HCN \rightarrow$ weak acid$\therefore$ They can act as buffer.While no other options follow definition of buffer solution.Option C is correct.

Question 10

What will happen when $CH_{3}COO Na$ is added to an aqueous solution of $CH_{3}COO H$?

Accepted Answer

$CH_{3}COOH \leftrightharpoons  CH_{3} COO^{-}+H^{+}$If $CH_{3}COONa$ is added, equilibrium will shift backward due to the common ion effect. $H^{+}$ will decrease.$\therefore$ pH will increase.

Equilibrium

Chemistry
8331 Views

Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution?

Blood is an example of basic buffer.

$p H$ of blood is 7.4

$H_{2} O$ is a:

In aqueous solution, the following mixture acts as buffer :

Match List-1 with List-2.

List -1    List-2
A) Aq. Solution of NaCl 1)Acidic buffer
B) Aq. Solution of $C H_{3} C O O N a$    2)Acidic solution
C) Aq. Solution of $N H_{4} C l$ 3) Basic solution
D) Aq. Solution of $C H_{3} C O O H$ along with $C H_{3} C O O N a$ 4)Neutral solution

Which of the following solution cannot act as a buffer?

The ionic product of water changes when:

A mixture of 0.01 M $C H_{3} C O O N a$ and $C H_{3} C O O H$ is a acidic buffer solution.

$C H_{3} C O O H$ is a weak acid.

Read the above assertion and reason and choose the correct option regarding it.

Which can act as buffer?

What will happen when $C H_{3} C O O N a$ is added to an aqueous solution of $C H_{3} C O O H$ ?

List -1	List-2
A) Aq. Solution of NaCl	1)Acidic buffer
B) Aq. Solution of $C H_{3} C O O N a$	2)Acidic solution
C) Aq. Solution of $N H_{4} C l$	3) Basic solution
D) Aq. Solution of $C H_{3} C O O H$ along with $C H_{3} C O O N a$	4)Neutral solution

Equilibrium

Chemistry 8331 Views

Which of the following mixtures in aqueous solution of equimolar concentration acts as a buffer solution?

Blood is an example of basic buffer.

pH of blood is 7.4

H2​O is a:

In aqueous solution, the following mixture acts as buffer :

Match List-1 with List-2. List -1 List-2 A) Aq. Solution of NaCl 1)Acidic buffer B) Aq. Solution of CH3​COONa 2)Acidic solution C) Aq. Solution of NH4​Cl 3) Basic solution D) Aq. Solution of CH3​COOH along with CH3​COONa 4)Neutral solution

Which of the following solution cannot act as a buffer?

The ionic product of water changes when:

A mixture of 0.01 M CH3​COONa and CH3​COOH is a acidic buffer solution.

CH3​COOH is a weak acid. Read the above assertion and reason and choose the correct option regarding it.

Which can act as buffer?

What will happen when CH3​COONa is added to an aqueous solution of CH3​COOH?

Chemistry
8331 Views

$p H$ of blood is 7.4

$H_{2} O$ is a:

Match List-1 with List-2.

List -1 List-2
A) Aq. Solution of NaCl 1)Acidic buffer
B) Aq. Solution of $C H_{3} C O O N a$ 2)Acidic solution
C) Aq. Solution of $N H_{4} C l$ 3) Basic solution
D) Aq. Solution of $C H_{3} C O O H$ along with $C H_{3} C O O N a$ 4)Neutral solution

A mixture of 0.01 M $C H_{3} C O O N a$ and $C H_{3} C O O H$ is a acidic buffer solution.

$C H_{3} C O O H$ is a weak acid.

Read the above assertion and reason and choose the correct option regarding it.

What will happen when $C H_{3} C O O N a$ is added to an aqueous solution of $C H_{3} C O O H$ ?