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PART - 1 CH - 6 Equilibrium Chemistry - PART - 1 CH - 6 Equilibrium

Gujarat Board (GSEB) - STD 11 Science - Chemistry (GSEB - English Medium). 140 questions in this chapter.

Question types

PART - 1 CH - 6 Equilibrium question types

140 questions across 7 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

140
Questions
7
Question groups
5
Question types
Sample Questions

PART - 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.

Q 2M.C.Q (1 Marks)1 Mark
The equilibrium constant for reaction $H _2+ I _2 \rightleftharpoons$ 2 HI will change :
  • A
    on increasing concentration of $H _2$ and $I _2$
  • B
    on increasing pressure
  • ✓
    on increasing temperature
  • D
    on adding catalyst

Answer: C.

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Q 3M.C.Q (1 Marks)1 Mark
The solubility product of $SnS _2$ is represented as :
  • A
    $\left[ Sn ^{+2}\right]\left[ S ^{-2}\right]^2$
  • ✓
    $\left[ Sn ^{+4}\right]\left[ S ^{-2}\right]^2$
  • C
    $\left[ Sn ^{+4}\right]\left[2 S^{-2}\right]$
  • D
    $\left[ Sn ^{+2}\right]\left[ S ^{-2}\right]$

Answer: B.

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Q 4M.C.Q (1 Marks)1 Mark
How many molecules of $H _2 O$ are present in one litre water?
  • ✓
    $55.5 \times 6.022 \times 10^{23}$
  • B
    $55.5 \times 6.022 \times 10^{16}$
  • C
    $55.5 \times 10^{-1}$
  • D
    $55.5 \times 10^{-4}$

Answer: A.

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Q 122 Marks Questions2 Marks
If in 500 ml of buffer solution 0.004 mole HCl are added then its pH is decreased by 0.04 , then what will be the buffer capacity of buffer solution?
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Q 132 Marks Questions2 Marks
The dissociation constant of HCOOH and $CH _3 COOH$ is $2 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively then calculate the isohydric concentration of HCOOH with $0.03 N CH _3 COOH$.
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Q 152 Marks Questions2 Marks
The $K_{\text {sp }}$ of PbS is $4 \times 10^{-28}$. If $\left[ Pb ^{+2}\right]=4 \times$ $10^{-27}$ then what will be the minimum concentration of $S ^{-2}$ to precipitation PbS ?
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Q 31Match the following.4 Marks
Column AColumn 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) $K _{ p }= K _{ c }( RT )^{\Delta n}$
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Q 32Match the following.4 Marks
Column AColumn B
(1) Condition of precipitation(a) Do not hydrolysed
(2) II group of basic radicals$\begin{array}{c}\text { (b) } pH = pKa + \\ \log \frac{[\text { salt }]}{[\text { acid }]}\end{array}$
(3) Henderson equation(c) $K _{ sp }< Q _{ sp }$
(4) NaCl(d) Acidic medium
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Q 33Match the following.4 Marks
Column AColumn 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) $pK _{ a } \pm 1$
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Q 34Match the following.4 Marks
Column AColumn 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
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Q 35Match the following.4 Marks
Column AColumn B
(1) Basicity of boric acid(a) $\Delta H$ is positive
(2) Proton acceptor(b) pH < 7
(3) Endothermic reaction(c) Bronsted-Lowry base
(4) Aqueous solution of NH4 CI(d) 1
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