Balancing Redox Reaction

Q. The mass of $70\%H_{2}S{O}_4$ required for neutralisation of 1 mole of $NaOH$ is:

1. 49 g
2. 98 g
3. 70 g
4. 34.3 g

Q. What is the mass of precipitate formed when $50\text{mL}$ of $17\%\left(w/V\right)$ solution of $AgN{O}_3$ is mixed with $50\text{mL}$ of $5.85\%\left(w/V\right)$ $NaCl$ solution?
$(Ag=108,N=14,O=16,Na=23,Cl=35.5)$

1. $3.5\text{g}$
2. $7\text{g}$
3. $14\text{g}$
4. $28\text{g}$

Q. How many gram equivalents of $H_{2}S{O}_4$ are present in 200 ml of $\frac{N}{10}$ $H_{2}S{O}_4$ solution ?

1. 0.01
2. 0.03
3. 0.02
4. 0.04

Q. Balance the following and choose the quantity which is the sum of the coefficients of reactants and products:
$PtC{l}_4+Xe{F}_2\to Pt{F}_6+ClF+Xe$

1. 16
2. 13
3. 18
4. 12

Q. In a balanced equation $H_{2}S{O}_4+xHI\to H_{2}S+y{I}_2+z{H}_{2}O,$ the values of x, y, z are

1. $x=5,y=3,z=4$
2. $x=4,y=8,z=5$
3. $x=3,y=5,z=2$
4. $x=8,y=4,z=4$

Q. 10 g of $BaC{l}_2$ is dissolved in 90 g of water. The density of the solution is 1.09 g/mL. Calculate the % (w/v) concentration of the solution.

1. 10.90%
2. 9.17%
3. 1.09%
4. 0.91%

Q.

A mixture of gases contains $H_2$ and $O_2$ gases in the ratio of 1 : 4 (w/w). What is the molar ratio of the two gases in the mixture ?

1. 2 : 1

2. 1 : 4

3. 4 : 1

4. 16 : 1

Q. A sea water sample contains $8\times {10}^{-3}$ g of dissolved oxygen per kilogram. What is the concentration of oxygen in parts per billion?

1. $8ppb$
2. $8\times {10}^{-3}ppb$
3. $8000ppb$
4. $800ppb$

Q. Concentrated aqueous sulphuric acid is 98% $H_{2}S{O}_4$ by mass and has a density of 1.80 g $m{L}^{-1}$. Volume of acid required to make one litre of 0.1 M $H_{2}S{O}_4$ is:

1. 5.55 mL
2. 11.10 mL
3. 16.65 mL
4. 22.20 mL

Q. In a reaction
$A+B_2\to A{B}_2$

Identify the limiting reagent, if any, in the following reaction mixtures

$A$: $300$ atoms of $A$ +$200$ molecules of $B$

$B$: $2$ mol $A$+$3$ mol $B$

$C$: $100$ atoms of $A$ +$100$ molecules of $B$

$D$: $5$ mol $A$ +$2.5$ mol $B$

$E$: $2.5$ mol$A$+$5$ mol $B$

Q. Match the items in column I with relevant items in column II.

\(\begin{array}{|c|c|c|c|}
\hline
\text{} & \text{Column I} & \text{} & \text{Column II}\\\hline
\text{A} & \text{Ions having positive charge} & \text{(i)} & \text{+7}\\\hline
\text{B} & \text{The sum of oxidation number of all atoms in a neutral molecule} & \text{(ii)} & \text{-1}\\\hline
\text{C} & \text{Oxidation number of hydrogen
ion \((H^+)\)} & \text{(iii)} & \text{+1}\\\hline
\text{D} & \text{Oxidation number of fluorine in NaF} & \text{(iv)} & \text{+0}\\\hline
\text{E} & \text{Ions having negative charge} & \text{(v)} & \text{Cation}\\\hline
\text{} & \text{} & \text{(vi)} & \text{Anion}\\\hline
\end{array}\)

Q. Match the items in column I with relevant items in column II.

$\begin{array}{cccc}& \text{Column I}& & \text{Column II}\\ \text{A}& \text{Ions having positive charge}& \text{(i)}& \text{+7}\\ \text{B}& \text{The sum of oxidation number of all atoms in a neutral molecule}& \text{(ii)}& \text{-1}\\ \text{C}& \text{Oxidation number of hydrogen ion}\left(H^{+}\right)& \text{(iii)}& \text{+1}\\ \text{D}& \text{Oxidation number of fluorine in NaF}& \text{(iv)}& \text{+0}\\ \text{E}& \text{Ions having negative charge}& \text{(v)}& \text{Cation}\\ & & \text{(vi)}& \text{Anion}\end{array}$

Q. What is the mass of $KI$ in 14.86 mL of a $32.44g/100mL$ aqueous $KI$ solution?

1. 6.85 g
2. 3.85 g
3. 5.82 g
4. 4.82 g

Q. A sample of drinking water was found to be severely contaminated with $CC{l}_4$. The level of contamination was 15 ppm (by mass). Calculate the mass percentage of $CC{l}_4$.

1. $1.5\times {10}^{-3}\%$
2. $1.5\times {10}^{-4}\%$
3. $0.005\%$
4. $0.001\%$

Q. For the equation in acidic medium: $S_2{O}_3^{2-}\left(aq\right)+C{r}_2{O}_7^{2-}\left(aq\right)\to S_4{O}_6^{2-}\left(aq\right)+C{r}^{3+}\left(aq\right)$
The coefficient of $H^{+}$ in the balanced reaction by oxidation number method will be

Q. Find out the volume of $98\%$ (w/w) $H_{2}S{O}_4$ (density $=1.8$ g/ml) that must be diluted to prepare $12.0$ litres of $2.4M$ sulphuric acid solution.

1. $1.6$ L
2. $2.3$ L
3. $1.8$ L
4. $2.8$ L

Q. Which of the following acts as a self - indicator?

1. Oxalic acid
2. $K_{2}C{r}_2{O}_7$
3. $KMn{O}_4$
4. Iodine

Q. $21.2\text{g}$ sample of impure $N{a}_{2}C{O}_3$ is dissolved and reacted with a solution of $CaC{l}_2$, the weight of $CaC{O}_3$ formed was $10.0\text{g}$. Which of the following statements is/are correct?

1. The percentage purity of $N{a}_{2}C{O}_3$ is $50\%$
2. The percentage purity of $N{a}_{2}C{O}_3$ is $60\%$
3. The number of moles of $N{a}_{2}C{O}_3=CaC{O}_3=0.1\text{mol}$
4. The number of moles of $NaCl$ formed is $0.1\text{mol}$

Q. The brown ring complex compound is formulated as $\left[Fe\right(H_{2}O{)}_5\left(NO\right)]S{O}_4$]. The oxidation state of iron in this complex is:

1. $+1$
2. $0$
3. $+2$
4. $+3$

Q. $S_8+bO{H}^{-}\to c{S}^{2-}+s{S}_2{O}_3^{2-}+H_{2}O$. Find the value of c.

Q. Which of the following concentration factor is affected by change in temperature?

1. Molarity
2. Molality
3. Mole fraction
4. Weight fraction

Q. $C{\underset{–}{S}}_2$

Q. 10 g of $BaC{l}_2$ is dissolved in 90 g of water. The density of the solution is 1.09 g/mL. Calculate the % (w/v) concentration of the solution.

1. 10.90%
2. 9.17%
3. 1.09%
4. 0.91%

Q. The oxidation number of $Pt$ in $\left[Pt\right(C_2{H}_4)C{l}_3{]}^{-}$ is :

Q. Which is the correct expression of van't Hoff factor for association of electrolyte?
Here,
n is the number of molecules associate to form n-mer
$\beta$ is the degree of dissociation

1. $i=1+\left[\frac{1}{n}-1\right]\beta$
2. $i=2+\left[\frac{1}{n}-1\right]\beta$
3. $i=1+[n-1]\beta$
4. $i=1+\left[\frac{1}{n}+1\right]\beta$

Q. Write balanced half reactions for the following redox reaction:
$C{r}_2{O}_7^{2-}+F{e}^{2+}\to C{r}^{3+}+F{e}^{3+}$

1. Reduction: $6e^{-}+14H^{+}+C{r}_2{O}_7^{2-}\to C{r}^{3+}+7H_{2}O$
   Oxidation: $F{e}^{2+}\to F{e}^{3+}+e^{-}$
2. Oxidation: $6e^{-}+14H^{+}+C{r}_2{O}_7^{2-}\to C{r}^{3+}+7H_{2}O$
   Reduction: $F{e}^{2+}\to F{e}^{3+}+e^{-}$
3. Oxidation: $6e^{-}+14H^{+}+C{r}_2{O}_7^{2-}\to C{r}^{3+}+6H_{2}O$
   Reduction: $F{e}^{2+}\to F{e}^{3+}+e^{-}$
4. Reduction: $4e^{-}+14H^{+}+C{r}_2{O}_7^{2-}\to C{r}^{3+}+7H_{2}O$
   Oxidation: $F{e}^{2+}\to F{e}^{3+}+e^{-}$

Q. 56.75 g of $HCl$ is dissolved in 2 L of water. Calculate the mass of $CaC{O}_3$ required to react completely with 25 mL of this $HCl$ solution.
$CaC{O}_3+2HCl\to CaC{l}_2+C{O}_2+H_{2}O$

1. 10.54 g
2. 9.275 g
3. 0.9715 g
4. 0.09727 g

Q. Statement – 1: Specific gravity is dimensionless.
Statement – 2: Specific gravity is density of a substance measured with respect to density of water at $4^{\circ }\text{C}$.

1. Both the statements are true and statement - 2 is the correct explanation of statement - 1
2. Both the statements are true and statement - 2 is not the correct explanation of statement - 1
3. Statement - 1 is true and statement - 2 is false.
4. Statement - 1 is false and statement - 2 is true.

Q. The molality of a sulphuric acid solution is $0.2$. Calculate the total weight of the solution having $1000$ gm of solvent.

1. $19.6$ g
2. $1000$ g
3. $1019.6$ g
4. $980.4$ g

Q. $0.45\text{g}$ of an acid (molar mass: $90\text{g/mol}$) was neutralized by $20\text{mL}$ of a $0.5\text{N}$ caustic potash. The basicity of the acid is:

1. 1
2. 3
3. 2
4. 4