04. Hydrogen Ion Concentration - pH Scale
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Ionic Equilibrium

229784 $75 \mathrm{ml}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $25 \mathrm{ml}$ of $1 \mathrm{M}$ $\mathrm{HCl}$. To this solution, $300 \mathrm{ml}$ of distilled water is added. What is the $\mathrm{pH}$ of the resultant solution?

1 1
2 2
3 4
4 0.2
AP-EAMCET-2002
Ionic Equilibrium

229786 Assertion (A) : The $\mathrm{pH}$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8\left(\mathrm{pK}_{\mathrm{a}}\right.$ of acetic acid is 4.8$)$ ).
Reason (R) : The ionic product of water at $\mathbf{2 5}^{\circ} \mathrm{C}$ is $10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$.
The correct answer is

1 Both (A) and (R) are true and (R) is the correct explanation of $(A)$
2 Both (A) and (R) are true and (R) is not correct explanation of $(A)$
3 (A) is true but (R) is not true
4 (A) is not true but (R) is true
AP-EAMCET-2005
Ionic Equilibrium

229788 $50 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ is added to $50 \mathrm{~mL}$ of $1 \times 10^{-3} \mathrm{M}$ barium hydroxide solution. What is the $\mathrm{pH}$ of the resulting solution?

1 3.0
2 3.3
3 11.0
4 11.7
AP-EAMCET-2008
Ionic Equilibrium

229791 A 0.20 molar solution of a weak monoprotic acid, HA, has a $\mathrm{pH}$ of 3.0. The ionization constant of the acid is

1 $5.0 \times 10^{-7}$
2 $2.0 \times 10^{-7}$
3 $5.0 \times 10^{-6}$
4 $5.0 \times 10^{-3}$
SCRA-2014
Ionic Equilibrium

229793 Which of the following gas the highest $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ ?

1 Distilled $\mathrm{H}_2 \mathrm{O}$
2 $1 \mathrm{Maq} \mathrm{NH}_3$
3 $1 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{HCl}$
Shift-I]
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Ionic Equilibrium

229784 $75 \mathrm{ml}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $25 \mathrm{ml}$ of $1 \mathrm{M}$ $\mathrm{HCl}$. To this solution, $300 \mathrm{ml}$ of distilled water is added. What is the $\mathrm{pH}$ of the resultant solution?

1 1
2 2
3 4
4 0.2
AP-EAMCET-2002
Ionic Equilibrium

229786 Assertion (A) : The $\mathrm{pH}$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8\left(\mathrm{pK}_{\mathrm{a}}\right.$ of acetic acid is 4.8$)$ ).
Reason (R) : The ionic product of water at $\mathbf{2 5}^{\circ} \mathrm{C}$ is $10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$.
The correct answer is

1 Both (A) and (R) are true and (R) is the correct explanation of $(A)$
2 Both (A) and (R) are true and (R) is not correct explanation of $(A)$
3 (A) is true but (R) is not true
4 (A) is not true but (R) is true
AP-EAMCET-2005
Ionic Equilibrium

229788 $50 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ is added to $50 \mathrm{~mL}$ of $1 \times 10^{-3} \mathrm{M}$ barium hydroxide solution. What is the $\mathrm{pH}$ of the resulting solution?

1 3.0
2 3.3
3 11.0
4 11.7
AP-EAMCET-2008
Ionic Equilibrium

229791 A 0.20 molar solution of a weak monoprotic acid, HA, has a $\mathrm{pH}$ of 3.0. The ionization constant of the acid is

1 $5.0 \times 10^{-7}$
2 $2.0 \times 10^{-7}$
3 $5.0 \times 10^{-6}$
4 $5.0 \times 10^{-3}$
SCRA-2014
Ionic Equilibrium

229793 Which of the following gas the highest $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ ?

1 Distilled $\mathrm{H}_2 \mathrm{O}$
2 $1 \mathrm{Maq} \mathrm{NH}_3$
3 $1 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{HCl}$
Shift-I]
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Ionic Equilibrium

229784 $75 \mathrm{ml}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $25 \mathrm{ml}$ of $1 \mathrm{M}$ $\mathrm{HCl}$. To this solution, $300 \mathrm{ml}$ of distilled water is added. What is the $\mathrm{pH}$ of the resultant solution?

1 1
2 2
3 4
4 0.2
AP-EAMCET-2002
Ionic Equilibrium

229786 Assertion (A) : The $\mathrm{pH}$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8\left(\mathrm{pK}_{\mathrm{a}}\right.$ of acetic acid is 4.8$)$ ).
Reason (R) : The ionic product of water at $\mathbf{2 5}^{\circ} \mathrm{C}$ is $10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$.
The correct answer is

1 Both (A) and (R) are true and (R) is the correct explanation of $(A)$
2 Both (A) and (R) are true and (R) is not correct explanation of $(A)$
3 (A) is true but (R) is not true
4 (A) is not true but (R) is true
AP-EAMCET-2005
Ionic Equilibrium

229788 $50 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ is added to $50 \mathrm{~mL}$ of $1 \times 10^{-3} \mathrm{M}$ barium hydroxide solution. What is the $\mathrm{pH}$ of the resulting solution?

1 3.0
2 3.3
3 11.0
4 11.7
AP-EAMCET-2008
Ionic Equilibrium

229791 A 0.20 molar solution of a weak monoprotic acid, HA, has a $\mathrm{pH}$ of 3.0. The ionization constant of the acid is

1 $5.0 \times 10^{-7}$
2 $2.0 \times 10^{-7}$
3 $5.0 \times 10^{-6}$
4 $5.0 \times 10^{-3}$
SCRA-2014
Ionic Equilibrium

229793 Which of the following gas the highest $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ ?

1 Distilled $\mathrm{H}_2 \mathrm{O}$
2 $1 \mathrm{Maq} \mathrm{NH}_3$
3 $1 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{HCl}$
Shift-I]
NEET DIGITAL LIBRARY
Ionic Equilibrium

229784 $75 \mathrm{ml}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $25 \mathrm{ml}$ of $1 \mathrm{M}$ $\mathrm{HCl}$. To this solution, $300 \mathrm{ml}$ of distilled water is added. What is the $\mathrm{pH}$ of the resultant solution?

1 1
2 2
3 4
4 0.2
AP-EAMCET-2002
Ionic Equilibrium

229786 Assertion (A) : The $\mathrm{pH}$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8\left(\mathrm{pK}_{\mathrm{a}}\right.$ of acetic acid is 4.8$)$ ).
Reason (R) : The ionic product of water at $\mathbf{2 5}^{\circ} \mathrm{C}$ is $10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$.
The correct answer is

1 Both (A) and (R) are true and (R) is the correct explanation of $(A)$
2 Both (A) and (R) are true and (R) is not correct explanation of $(A)$
3 (A) is true but (R) is not true
4 (A) is not true but (R) is true
AP-EAMCET-2005
Ionic Equilibrium

229788 $50 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ is added to $50 \mathrm{~mL}$ of $1 \times 10^{-3} \mathrm{M}$ barium hydroxide solution. What is the $\mathrm{pH}$ of the resulting solution?

1 3.0
2 3.3
3 11.0
4 11.7
AP-EAMCET-2008
Ionic Equilibrium

229791 A 0.20 molar solution of a weak monoprotic acid, HA, has a $\mathrm{pH}$ of 3.0. The ionization constant of the acid is

1 $5.0 \times 10^{-7}$
2 $2.0 \times 10^{-7}$
3 $5.0 \times 10^{-6}$
4 $5.0 \times 10^{-3}$
SCRA-2014
Ionic Equilibrium

229793 Which of the following gas the highest $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ ?

1 Distilled $\mathrm{H}_2 \mathrm{O}$
2 $1 \mathrm{Maq} \mathrm{NH}_3$
3 $1 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{HCl}$
Shift-I]
Join With Us for More Updates
Ionic Equilibrium

229784 $75 \mathrm{ml}$ of $0.2 \mathrm{M} \mathrm{HCl}$ is mixed with $25 \mathrm{ml}$ of $1 \mathrm{M}$ $\mathrm{HCl}$. To this solution, $300 \mathrm{ml}$ of distilled water is added. What is the $\mathrm{pH}$ of the resultant solution?

1 1
2 2
3 4
4 0.2
AP-EAMCET-2002
Ionic Equilibrium

229786 Assertion (A) : The $\mathrm{pH}$ of a buffer solution containing equal moles of acetic acid and sodium acetate is $4.8\left(\mathrm{pK}_{\mathrm{a}}\right.$ of acetic acid is 4.8$)$ ).
Reason (R) : The ionic product of water at $\mathbf{2 5}^{\circ} \mathrm{C}$ is $10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$.
The correct answer is

1 Both (A) and (R) are true and (R) is the correct explanation of $(A)$
2 Both (A) and (R) are true and (R) is not correct explanation of $(A)$
3 (A) is true but (R) is not true
4 (A) is not true but (R) is true
AP-EAMCET-2005
Ionic Equilibrium

229788 $50 \mathrm{~mL}$ of $\mathrm{H}_2 \mathrm{O}$ is added to $50 \mathrm{~mL}$ of $1 \times 10^{-3} \mathrm{M}$ barium hydroxide solution. What is the $\mathrm{pH}$ of the resulting solution?

1 3.0
2 3.3
3 11.0
4 11.7
AP-EAMCET-2008
Ionic Equilibrium

229791 A 0.20 molar solution of a weak monoprotic acid, HA, has a $\mathrm{pH}$ of 3.0. The ionization constant of the acid is

1 $5.0 \times 10^{-7}$
2 $2.0 \times 10^{-7}$
3 $5.0 \times 10^{-6}$
4 $5.0 \times 10^{-3}$
SCRA-2014
Ionic Equilibrium

229793 Which of the following gas the highest $\mathrm{pH}$ at $25^{\circ} \mathrm{C}$ ?

1 Distilled $\mathrm{H}_2 \mathrm{O}$
2 $1 \mathrm{Maq} \mathrm{NH}_3$
3 $1 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{HCl}$
Shift-I]