Equivalent Mass

Q.

What is the equivalent weight of ${\mathrm{KMnO}}_4$ in acidic, basic, and neutral medium?

Q.

What is effective atomic number? Calculate effective atomic number of copper $(\mathrm{Z}=29)$ in ${\left[\mathrm{Cu}({\mathrm{NH}}_3{)}_4\right]}^{2+}$.

Q.

Calculate the mass of CaCO3 required to react completely with 25ml of 0.75M HCl

Q.

The equivalent weight of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ is?

Q.

What is the equivalent weight of ${\mathrm{H}}_3{\mathrm{PO}}_4$ in the reaction: $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2+{\mathrm{H}}_3{\mathrm{PO}}_4\to {\mathrm{CaHPO}}_4+2{\mathrm{H}}_2\mathrm{O}$

Q.

What is equivalent weight of crystalline oxalic acid?

Q. The normality of solution obtained by mixing $100\text{mL}$ of $0.2M$ $H_{2}S{O}_4$ with $100\text{mL}$ of $0.2M$ $NaOH$ is:

1. $0.1\text{N}$
2. $0.2\text{N}$
3. $0.5\text{N}$
4. $0.3\text{N}$

Q. A metal oxide contains 60 % of metal by mass. The equivalent weight of the metal is:

1. $12\text{g}$
2. $40\text{g}$
3. $40\text{g}$
4. $24\text{g}$

Q.

What is the number of moles of ${\mathrm{KMnO}}_4$ that will be needed to react with one mole of sulphite ions in acidic solution?

Q.

What mass of CaCO₃ is required to react completely with 25ml of 0.75M of HCL.

Q. Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as indicator. The number of moles of Mohr's salt required per mole of dichromate is:
(The formula for Mohr's salt is $FeS{O}_4.(N{H}_4{)}_{2}S{O}_4.6H_{2}O$)

1. 6
2. 5
3. 4
4. 3

Q. Find the number of moles of $KMn{O}_4$ needed to oxidise one mole $C{u}_{2}S$ in acidic medium. The reaction is $KMn{O}_4+C{u}_{2}S\to M{n}^{2+}+C{u}^{2+}+S{O}_2$

1. 0.4
2. 1.6
3. 0.5
4. 1.2

Q.

Determine the equivalent weight of sodium chloride ($\mathrm{NaCl}$).

Q. The equivalent weight of Mohr’s salt, $FeS{O}_4.(N{H}_4{)}_{2}S{O}_4.6H_{2}O$ is equal to:

1. Molar weight of Mohr’s salt
2. One-fourth of the molar weight
3. Half of its molar weight
4. One-third of the molar weight

Q. One mole of acidfied potassium dichromate on reaction with excess $KI$ will liberate ………….. mole(s) of $I_2$.

1. 3
2. 1
3. 7
4. 2

Q.

Given the chemical equation,

${\mathrm{K}}_3{\mathrm{PO}}_4+\mathrm{Al}{\left({\mathrm{NO}}_3\right)}_3\to 3{\mathrm{KNO}}_3+{\mathrm{AlPO}}_4$

How many moles of potassium nitrate are produced when two moles of potassium phosphate react with two moles of aluminum nitrate?

Q. 0.9 g Al reacts with dil. HCl to give H2. The volume of H2 evolved at STP is [Atomic weight of Al=27]

Q.

The oxide of a metal has 32% oxygen. Its equivalent weight would be

1. 32
2. 17
3. 34
4. 8

Q.

Normality of 1% (wt/vol) H2SO4 is

Q. 1.25 g of a solid dibasic acid is completely neutralised by 25 ml of 0.25 molar $Ba(OH{)}_2$ solution. Molecular mass of the acid is

1. 150
2. 120
3. 200
4. 100

Q. Q. The equivalent mass of H3PO4 (Molecular weight = 98 g/mol) and Na2HPO4 (Molecular weight = 142 g/mol) in the reaction are respectively :- H3PO4 + 2NaOH → Na2HPO4 + 2H2O (1) 49, 142 (2) 49, 71 (3) 98, 71 (4) 98, 142

Q. $4\text{g}$ of copper was dissolved in concentrated nitric acid. The copper nitrate on strong heating gave $5\text{g}$ of its oxide. The equivalent weight of copper is _______.

1. $12\text{g}$
2. $16\text{g}$
3. $32\text{g}$
4. $34\text{g}$

Q. Equivalent mass of H3PO4 for the given reaction, H3PO4 + Ca[OH]2 -- CaHPO4 + 2 H2O

Q. Find the equivalent weight of thiosulphate ion from the following reaction:
$\underset{\left(Reducingagent\right)}{2S_2{O}_3^{2-}}\to S_4{O}_6^{2-}+2e^{-}$

1. M
2. 2M
3. $\frac{M}{2}$
4. 3M

Q.

Solubility of $\mathrm{Cu}{\left(\mathrm{OH}\right)}_2$ in $0.1\mathrm{M}$ aqueous $\mathrm{NaOH}$ solution is ($\mathrm{Ksp}$ of $\mathrm{Cu}{\left(\mathrm{OH}\right)}_2=2.2\times {10}^{-20}$)

Q. 0.52 g of a dibasic acid required 100 mL of 0.2 N NaOH for complete neutralization.
The equivalent weight of acid is:

1. 26
2. 52
3. 104
4. 156

Q.

Human blood has pH value_______.

1. 6

2. 7.4

3. 6.5

4. 7

Q. The number of Faradays(F) required to produce $4.5\text{g}$ of aluminium from molten $AlC{l}_3$ is:
(Atomic mass of $Al=27u$)

1. $2$
2. $3$
3. $1$
4. $0.5$

Q. 0.64 g of a metal hydride contains 0.24 g of hydrogen. The equivalent mass of the metal will be:

1. 1.366 g
2. 2.666 g
3. 13.33 g
4. 1.66 g

Q. $AgN{O}_3$ sample is $73\%$ by mass. To prepare $125mL$ of $0.04MAgN{O}_3$ solution, $AgN{O}_3$ sample required is

1. $1.250g$
2. $1.471g$
3. $1.164g$
4. $1.063g$