229709 A student needs to prepare a buffer solution of propanoic acid and its sodium salt with $\mathrm{pH} 4$.
The ratio of $\frac{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COO}^{-}\right]}{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\right]}$ required to make buffer is
Given : $\left.\overline{\mathrm{K}_{\mathrm{a}}\left(\mathrm{CH}_3\right.} \mathrm{CH}_2 \mathrm{COOH}\right)=1.3 \times 10^{-5}$

229715 Study the following table
${c} { Buffer solution } |
| { (in } { ) }$ | ${c} { Volume (in } |
|---|---|
| { mL) of } |
| { weak acid }$ | ${c} { Volume (in } { ) } |
| { of } { M sodium } |
| { salt of weak } |
| { acid }$ |
|I | 4.0 | 4.0 |
|II | 4.0 | 40.0 |
|III | 40.0 | 4.0 |
|IV | 0.1 | 10.0 |
|
Which of the two sets of buffer solutions have least $\mathrm{pH}$ ?

229717 A buffer solution is prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M}$ acetic acid and $20 \mathrm{~mL}$ of $0.5 \mathrm{M}$ sodium acetate and then diluted to $100 \mathrm{~mL}$ with distilled water. If the $\mathrm{pK}_{\mathrm{a}}$ of acetic acid is 4.76 , what is the $\mathrm{pH}$ of the buffer solution prepared?

229718 Which one of the following will not function as buffer solution?

229722 Which of the following equations give ionic product of water?
(i) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
(ii) $\mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{NH}_3$ (aq)
(iii) $\mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \square \quad \mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}$
(iv) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \square \quad \mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}$

229709 A student needs to prepare a buffer solution of propanoic acid and its sodium salt with $\mathrm{pH} 4$.
The ratio of $\frac{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COO}^{-}\right]}{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\right]}$ required to make buffer is
Given : $\left.\overline{\mathrm{K}_{\mathrm{a}}\left(\mathrm{CH}_3\right.} \mathrm{CH}_2 \mathrm{COOH}\right)=1.3 \times 10^{-5}$

229715 Study the following table
${c} { Buffer solution } |
| { (in } { ) }$ | ${c} { Volume (in } |
|---|---|
| { mL) of } |
| { weak acid }$ | ${c} { Volume (in } { ) } |
| { of } { M sodium } |
| { salt of weak } |
| { acid }$ |
|I | 4.0 | 4.0 |
|II | 4.0 | 40.0 |
|III | 40.0 | 4.0 |
|IV | 0.1 | 10.0 |
|
Which of the two sets of buffer solutions have least $\mathrm{pH}$ ?

229717 A buffer solution is prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M}$ acetic acid and $20 \mathrm{~mL}$ of $0.5 \mathrm{M}$ sodium acetate and then diluted to $100 \mathrm{~mL}$ with distilled water. If the $\mathrm{pK}_{\mathrm{a}}$ of acetic acid is 4.76 , what is the $\mathrm{pH}$ of the buffer solution prepared?

229718 Which one of the following will not function as buffer solution?

229722 Which of the following equations give ionic product of water?
(i) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
(ii) $\mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{NH}_3$ (aq)
(iii) $\mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \square \quad \mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}$
(iv) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \square \quad \mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}$

229709 A student needs to prepare a buffer solution of propanoic acid and its sodium salt with $\mathrm{pH} 4$.
The ratio of $\frac{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COO}^{-}\right]}{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\right]}$ required to make buffer is
Given : $\left.\overline{\mathrm{K}_{\mathrm{a}}\left(\mathrm{CH}_3\right.} \mathrm{CH}_2 \mathrm{COOH}\right)=1.3 \times 10^{-5}$

229715 Study the following table
${c} { Buffer solution } |
| { (in } { ) }$ | ${c} { Volume (in } |
|---|---|
| { mL) of } |
| { weak acid }$ | ${c} { Volume (in } { ) } |
| { of } { M sodium } |
| { salt of weak } |
| { acid }$ |
|I | 4.0 | 4.0 |
|II | 4.0 | 40.0 |
|III | 40.0 | 4.0 |
|IV | 0.1 | 10.0 |
|
Which of the two sets of buffer solutions have least $\mathrm{pH}$ ?

229717 A buffer solution is prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M}$ acetic acid and $20 \mathrm{~mL}$ of $0.5 \mathrm{M}$ sodium acetate and then diluted to $100 \mathrm{~mL}$ with distilled water. If the $\mathrm{pK}_{\mathrm{a}}$ of acetic acid is 4.76 , what is the $\mathrm{pH}$ of the buffer solution prepared?

229718 Which one of the following will not function as buffer solution?

229722 Which of the following equations give ionic product of water?
(i) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
(ii) $\mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{NH}_3$ (aq)
(iii) $\mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \square \quad \mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}$
(iv) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \square \quad \mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}$

229709 A student needs to prepare a buffer solution of propanoic acid and its sodium salt with $\mathrm{pH} 4$.
The ratio of $\frac{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COO}^{-}\right]}{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\right]}$ required to make buffer is
Given : $\left.\overline{\mathrm{K}_{\mathrm{a}}\left(\mathrm{CH}_3\right.} \mathrm{CH}_2 \mathrm{COOH}\right)=1.3 \times 10^{-5}$

229715 Study the following table
${c} { Buffer solution } |
| { (in } { ) }$ | ${c} { Volume (in } |
|---|---|
| { mL) of } |
| { weak acid }$ | ${c} { Volume (in } { ) } |
| { of } { M sodium } |
| { salt of weak } |
| { acid }$ |
|I | 4.0 | 4.0 |
|II | 4.0 | 40.0 |
|III | 40.0 | 4.0 |
|IV | 0.1 | 10.0 |
|
Which of the two sets of buffer solutions have least $\mathrm{pH}$ ?

229717 A buffer solution is prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M}$ acetic acid and $20 \mathrm{~mL}$ of $0.5 \mathrm{M}$ sodium acetate and then diluted to $100 \mathrm{~mL}$ with distilled water. If the $\mathrm{pK}_{\mathrm{a}}$ of acetic acid is 4.76 , what is the $\mathrm{pH}$ of the buffer solution prepared?

229718 Which one of the following will not function as buffer solution?

229722 Which of the following equations give ionic product of water?
(i) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
(ii) $\mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{NH}_3$ (aq)
(iii) $\mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \square \quad \mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}$
(iv) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \square \quad \mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}$

229709 A student needs to prepare a buffer solution of propanoic acid and its sodium salt with $\mathrm{pH} 4$.
The ratio of $\frac{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COO}^{-}\right]}{\left[\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\right]}$ required to make buffer is
Given : $\left.\overline{\mathrm{K}_{\mathrm{a}}\left(\mathrm{CH}_3\right.} \mathrm{CH}_2 \mathrm{COOH}\right)=1.3 \times 10^{-5}$

229715 Study the following table
${c} { Buffer solution } |
| { (in } { ) }$ | ${c} { Volume (in } |
|---|---|
| { mL) of } |
| { weak acid }$ | ${c} { Volume (in } { ) } |
| { of } { M sodium } |
| { salt of weak } |
| { acid }$ |
|I | 4.0 | 4.0 |
|II | 4.0 | 40.0 |
|III | 40.0 | 4.0 |
|IV | 0.1 | 10.0 |
|
Which of the two sets of buffer solutions have least $\mathrm{pH}$ ?

229717 A buffer solution is prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M}$ acetic acid and $20 \mathrm{~mL}$ of $0.5 \mathrm{M}$ sodium acetate and then diluted to $100 \mathrm{~mL}$ with distilled water. If the $\mathrm{pK}_{\mathrm{a}}$ of acetic acid is 4.76 , what is the $\mathrm{pH}$ of the buffer solution prepared?

229718 Which one of the following will not function as buffer solution?

229722 Which of the following equations give ionic product of water?
(i) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
(ii) $\mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \quad \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{NH}_3$ (aq)
(iii) $\mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \square \quad \mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}$
(iv) $\mathrm{NH}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \square \quad \mathrm{NH}_2^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}$