Basic Buffer Action

Q. $N{H}_{4}OH$ is titrated with $HCl$ solution. Find the value of $\log \left(\frac{\left[N{H}_4^{+}\right]}{\left[N{H}_{4}OH\right]}\right)$ when the volume of $HCl$ added is half of that of equivalence point.

1. 0
2. 1
3. 0.5
4. 0.75

Q. Calculate the weight (in $mg$) of $HCl$ that should be added to $100ml$ of $0.1MBOH$ to make a buffer solution of $pOH=6$.
$K_b\left(BOH\right)=1\times {10}^{-8}$ (assume there is no change in volume on addition of $HCl$)

1. 4.6
2. 3.6
3. 5.6
4. 6.6

Q. Calculate the weight in mg of HCl added to 100 ml of 0.1 N BOH to have its pH = 6.6 and $K_b=6.25\times {10}^{-8};$ Antilog $(-7.4)=3.98\times {10}^{-8}.$ (Assume there is no change in volume on addition of $HCl$)

1. 300
2. 425
3. 100
4. 223

Q. Which will make basic buffer ?

1. $50mLof0.1MNaOH+25mLof0.1MC{H}_{3}COOH$
2. $100mLof0.1MC{H}_{3}COOH+100mLof0.1MNaOH$
3. $100mLof0.1MHCl+200mLof0.1MN{H}_{4}OH$
4. $100mLof0.1MHCl+100mLof0.1MNaOH$

Q. Calculate the weight (in $mg$) of $HCl$ that should be added to $100ml$ of $0.1MBOH$ to make a buffer solution of $pOH=6$.
$K_b\left(BOH\right)=1\times {10}^{-8}$ (assume there is no change in volume on addition of $HCl$)

1. 3.6
2. 4.6
3. 5.6
4. 6.6

Q. Which will make basic buffer ?

1. $50mLof0.1MNaOH+25mLof0.1MC{H}_{3}COOH$
2. $100mLof0.1MC{H}_{3}COOH+100mLof0.1MNaOH$
3. $100mLof0.1MHCl+200mLof0.1MN{H}_{4}OH$
4. $100mLof0.1MHCl+100mLof0.1MNaOH$

Q. Which will make a basic buffer?

1. $50mL$ of $0.1M$ $NaOH$ + $25mL$ of $0.1M$ $C{H}_{3}COOH$
2. $100mL$ of $0.1M$ $C{H}_{3}COOH$ + $100mL$ of $0.1M$ $NaOH$
3. $100mL$ of $0.1M$ $HCl$ + $200mL$ of $0.1M$ $N{H}_{4}OH$
4. $100mL$ of $0.1M$ $HCl$ + $100mL$ of $0.1M$ $NaOH$

Q. Conductometric titration curve of an equimolar mixture of $HCl$ and $HCN$ with $NaOH\left(aq\right)$ can be given as

Q. $C{H}_{3}N{H}_2$ (0.1 mole $K_b$ = 5 $\times {10}^{-4})$ is added to 0.08 mole of HCl and the solution is diluted to one litre, resulting hydrogen ion concentration is

1. $1.6\times {10}^{-11}$
2. $8\times {10}^{-11}$
3. $5\times {10}^{-5}$
4. $8\times {10}^{-2}$

Q. $N{H}_{4}OH$ is titrated with $HCl$ solution. Find the value of $\log \left(\frac{\left[N{H}_4^{+}\right]}{\left[N{H}_{4}OH\right]}\right)$ when the volume of $HCl$ added is half of that of equivalence point.

1. \N
2. 0.5
3. 0.75
4. 1

Q. Calculate the weight in mg of HCl added to 100 ml of 0.1 N BOH to have its pH = 6.6 and $K_b=6.25\times {10}^{-8};$ Antilog $(-7.4)=3.98\times {10}^{-8}.$ (Assume there is no change in volume on addition of $HCl$)

1. 300
2. 100
3. 425
4. 223

Q. Calculate the ratio of $C{H}_{3}N{H}_2$ to $C{H}_{3}N{H}_3^{+}C{l}^{-}$ required to create a buffer with pH = 10.14
$K_{b}ofC{H}_{3}N{H}_2=4.4\times {10}^{-4}$
take $log2.27=0.356,log0.313=-0.504$

1. 0.5
2. 1.05
3. 0.31
4. None of the above