Sample QuestionsPART - 1 CH - 6 Equilibrium questions
One sample from each question group in this chapter. Select any group above to see the full set with answer keys.
How many molecules of $H _2 O$ are present in one litre water?
Answer: A.
View full solution →What will be the effect on pH when 1 liter water is added to 2 liter solution of mixture of $CH _3 COOH$ and $CH _3 COONa$ :
Answer: C.
View full solution →The solubility of a less soluble salt having formula $M _2 Y$ will be :
( $K _{\text {sp }}=$ solubility product constant)
- A
$\sqrt{ K _{ sp }}$
- ✓
$\left(\frac{ K _{ sp }}{4}\right)^{\frac{1}{3}}$
- C
$\left( K _{ sp }\right)^{\frac{1}{3}}$
- D
$\left(\frac{ K _{ sp }}{2}\right)^{\frac{1}{2}}$
Answer: B.
View full solution →If concentration of reactants and products are doubled then value of equilibrium constant KC is equal to which of the following:
- A
$2 K_{ c }$
- B
$\frac{K_c}{2}$
- C
$K _{ c }^2$
- ✓
Answer: D.
View full solution →The equilibrium constant for reaction $H _2+ I _2 \rightleftharpoons$ 2 HI will change :
Answer: C.
View full solution →KCl is a salt formed by strong acid and__________.
Perchloric acid is a__________.
Equilibrium is always__________.
The value of ionic product of water is__________.
On adding common ion in ionic salts, its solubility__________.
Reaction quotient $\left(Q_c\right)$ is always equal to equilibrium constant $( K )$.
View full solution →At equilibrium the value of free energy change $(\Delta G)$ is zero.
View full solution →When value of equilibrium constant is very less than reaction gets almost completed.
For reaction $PCl _5(g) \rightleftharpoons PCl _3(g)+ Cl _2(g), K _{ p }>$ $K _{ c }$.
View full solution →Molar concentration is also known as active mass.
Predict if solutions of following salts are neutral, acidic or basic :
$NaCl , KBr , NaCN , NH _4 NO _3, NaNO _2$ and KF .
View full solution →For the following equilibrium, $K_c=6.3 \times$ $10^{14}$ at 1000 K
$NO ( g )+ O _3(g) \rightleftharpoons NO _2(g)+ O _2(g)$
Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is $K_c$, for the reverse reaction?
View full solution →The pH of a sample of vinegar is 3.76 . Calculate the concentration of hydrogen ion in it.
The concentration of hydrogen ion in a sample of soft drink is $3.8 \times 10^{-3} M$. What is its pH ?
View full solution →Write conjugate acids for following bronsted bases : $NH _2^{-}, NH _3$ and $HCOO ^{-}$.
View full solution →Nitric oxide reacts with $Br _2$ and gives nitrosyl bromide as per reaction given below :
$2 NO ( g )+ Br _2(g) \rightleftharpoons 2 NOBr ( g )$
When 0.087 mol of NO and 0.0437 mol of $Br _2$ are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and $Br _2$.
View full solution →What is the minimum volume of water required to dissolve 1 gm of calcium sulphate at 298 $K ?\left(\right.$ For calcium sulphate, $\left.K_{\text {sp }}=9.1 \times 10^{-6}\right)$
View full solution →Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression?
The solubility product constant of $Ag _2 CrO _4$ and AgBr are $1.1 \times 10^{-12}$ and $5.0 \times 10^{-13}$ respectively. Calculate the ratio of the molarities of their saturated solutions.
View full solution →Calculate the pH of the resultant mixture :
10 mL of $0.01 M H _2 SO _4+10 mL$ of 0.01 M $Ca ( OH )_2$
View full solution →What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, $\left.K_{s p}=6.3 \times 10^{-18}\right)$
View full solution →Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate $K_{s p}=7.4 \times 10^{-8}$ )
View full solution →Calculate the pH of the resultant mixture :
10 mL of $0.1 M H _2 SO _4+10 mL$ of 0.1 M KOH
View full solution →The pH of 0.1 M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
The solubility of $Sr ( OH )_2$ at 298 K is $19.23 g / L$ of solution. Calculate the concentration of strontium and hydroxyl ions and the pH of the solution.
View full solution →| Column A | Column B |
| (1) Amphoprotic solvent | (a) $CO _3^{2-}$ |
| (2) Conjugate base of $HCO _3^{-}$ | (b) $BF _3$ |
| (3) $CH _3 COOH$ | (c) $NH _3$ |
| (4) Lewis acid | (d) A weak base |
| Column A | Column B |
| (1) Solution of $CuSO _4$ | (a) 14 |
| (2) $SnS _2$ | (b) $pH <7$ |
| (3) Relationship of $K _{ p }$ and $K _{ c }$ | (c) $K_{s p}=4 s^3$ |
| (4) $pK _{ a }+ pK _{ b }$ | (d) $K _{ p }= K _{ c }( RT )^{\Delta n}$ |
| Column A | Column B |
| (1) $CH _3 COOK$ | (a) $h=\sqrt{ Kh }$ |
| (2) $CH _3 COONH _4$ | (b) $K _{s p}=s^2$ |
| (3) pH range of acidic buffer | (c) $Kh =\frac{ K _{ w }}{ K _{ a }}$ |
| (4) For $BaSO _4$ | (d) $pK _{ a } \pm 1$ |
| Column A | Column B |
| (1) Solution of $CH _3 COONH _4$ | (a) Salt formed by weak acid and weak base |
| (2) $NH _4 Cl$ | (b) $pH =7$ |
| (3) $NH _4 OH + NH _4 Cl$ | (c) $Kh =\frac{ K _{ w }}{ K _{ b }}$ |
| (4) $\left( NH _4\right)_2 CO _3$ | (d) Basic buffer |
| Column A | Column B |
| (1) $Ba ( OH )_2$ | (a) $\alpha \propto \sqrt{V}$ |
| (2) For weak acid | (b) Acidity = 2 |
| (3) Ostwald dilution law | (c) $\left[ H ^{+}\right]=\sqrt{ C . K _{ a }}$ |
| (4) For dibasic acid | (d) $K _{ a _2}< K _{ a _1}$ |
Reaction between $N _2$ and $O _2$ takes place as follows :
$2 N _2(g)+ O _2(g) \rightleftharpoons 2 N _2 O ( g )$
If a mixture of $0.482 mol N _2$ and 0.933 mol of $O _2$ is placed in a 10 L reaction vessel and allowed to form $N _2 O$ at a temperature for which $K _{ c }=2.0 \times 10^{-37}$, determine the composition of equilibrium mixture.
View full solution →The concentration of sulphide ion in 0.1 M HCl solution saturated with hydrogen sulphide is $1.0 \times 10^{-19} M$. If 10 mL of this is added to 5 mL of 0.04 M solution of the following : $FeSO _4, MnCl _2$, $Z n C l _{ 2 }$ and $C d C l _{ 2 }$. In which of these solutions precipitation will take place?
View full solution →The ionization constant of benzoic acid is $6.46 \times 10^{-5}$ and $K_{s p}$ for silver benzoate is $2.5 \times$ $10^{-13}$. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?
View full solution →Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298 K from their solubility product constants given in Table 6.9. Determine also the molarities of individual ions.
Calculate the pH of the resultant mixture :
10 mL of $0.2 M Ca ( OH )_2+25 mL$ of 0.1 M HCI
View full solution →