Ionic Equilibrium Test

Result

Ionic Equilibrium Test - 9

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Weekly Quiz Competition

Question 1
1 / -0

The equilibrium constant for the given reaction is approximately 10^–3

HPO₄^2– (aq) + HCO₃^– (aq) ⇌ H₂PO₄^– (aq) + CO₃^2– (aq)

Which is strongest conjugate base in the given reaction?

A
HPO₄^2– (aq)

B
HCO₃^– (aq)

C
H₂PO₄^– (aq)

D
CO₃^2–(aq)

Solution

CO₃^2– + H₂PO₄– ⇌ HPO₄^2– + HCO₃^2–

K_c = 10³

Therefore CO₃²⁻ is the stronger conjugate base than HPO₄²⁻
Question 2
1 / -0

Which of the following constitutes a set amphoteric species.?

A

B

C

D

Solution

H₃O⁺ cannot take up proton; H₂PO₂^– cannot give up proton, SO₄²⁻ cannot give proton
Question 3
1 / -0

Which of the following order of acid strengths are correct?

A
HOI < HOBr < HOCl

B
HCl < HBr < HI

C
HIO₄< HBrO₄ < HClO₄

D
All of the above are correct order

Solution

In HOX with increase in electronegativity acid strength increases

In H – X acid strength increases with decrease in bond energies.

In HXO₄ acid strength increases with decrease in size of X.
Question 4
1 / -0

The pH of Ba(OH)₂ solution is 13. The number millimoles of Ba(OH)₂present in 10 ml of solution would be

A
1.00

B
0.50

C
10.00

D
15.00

Solution

[OH^–] = 0.1

And conc. of Ba(OH)₂ = 0.1/2

∴ The no. of millimoles of Ba(OH)₂ present in 10 ml solution

= 0.1/2 × 10 × 10^-3 × 10³ = 0.5
Question 5
1 / -0

For 10^–2(M) H₃PO₃ solution which of the following relations is correct?

A

B

C

D

Solution
Question 6
1 / -0

The pH of 0.01 (M) KOH is 12; if the temperature of the given KOH solution is increased which of the following would occur ?

A
Both pH and pOH would remain constant

B
pH would be decreased but pOH remain constant

C
pH would be increased while pOH remain constant

D
pH would be increased while pOH would be decreased

Solution

Since, KOH is a strong electrolyte its dissociation remain unaffected, hence, [OH^– ] = 10^–2

or pOH = 2 but on increasing temperature pK_w < 14

or pH + pOH < 14

or pH < 12

Therefore, pH would be decreased.
Question 7
1 / -0

4 ml of HCl solution of pH = 2 is mixed with 6 ml of NaOH solution of pH = 12. What would be the final pH of solution? log 2 = 0.3

A
10.3

B
11.3

C
11

D
4.3

Solution
Question 8
1 / -0

The pH of 0.1(M) H₂SO₄ in water is

A
is equal to one

B
is more than one

C
is less than one

D
may be equal to or greater than or smaller than one depending upon temperature

Solution

H₂SO₄ → H⁺ + HSO₄^–

In solution [H⁺] > 0.1(M), hence pH < 1
Question 9
1 / -0

A solution of NaCl is

A
acidic in nature

B
alkaline in nature

C
neutral in nature

D
amphoteric in nature

Solution

A solution of NaCl is neutral as both Na⁺ and Cl^– ions are weak conjugate acid and base respectively.
Question 10
1 / -0

A solution of ammonium cyanide is

A
acidic in nature

B
alkaline in nature

C
neutral in nature

D
amphoteric in nature

Solution

A solution of NH₄CN is alkaline because CN^– is more strong conjugate base than NH₄⁺ , conjugate acid. The hydrolysis of CN^– proceeds more that of NH₄⁺ .