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12th Chemistry weekly Test - 3 ( Ionic Equilibrium )

St. Britto Hr. Sec. School - Madurai

12th Chemistry weekly Test - 3 ( Ionic Equilibrium )-Aug 2020

Time : 1.30 Hours

Part - A

Multiple Choice Question - Answer All Question

Pick the strongest conjugate base among the following

Cl^-
\({ NO }_{ 2 }^{ - }\)
\({ SO }_{ 4 }^{ 2- }\)
CH₃COO^-

The conjugate base of \({ NH }_{ 2 }^{ - }\) is

NH^-
NH₃
\({ NH }_{ \ 3 }^{ \ + }\)
NH^2-

An example of basic buffer is

NH₄OH and NH₄Cl
NH₄OH and NaOH
NaOH and NH₄Cl
NaOH and KOH

Using Gibb's free energy change,∆G° = 57.34 kj mol^-1, for the reaction, X₂ Y_(s) \(\rightleftharpoons \) 2X⁺ + Y^2-_(aq) calculate the solubility product of X₂Y in water at 300 K

(R = 8.3JK^-1 Mol^-1)

10^-10
10^-12
10^-14
can not be calculated from the given data

Analyses the equilibrium

HClO₄ + H₂O \(\rightleftharpoons \) H₃O⁺ + \({ ClO }_{ 4 }^{ - }\)

and choose the correct statement.

H₃O⁺ is the conjugate base of H₂O
\({ ClO }_{ 4 }^{ - }\)is the conjugate base of HClO₄
H₂O is the conjugate acid of H₃O⁺
HClO₄ is the conjugate acid of H₃O⁺

When sodium acetate is added to acetic acid, the degree of ionisation of acetic acid

increases
decreases
dose not change
becomes zero

The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salt is given by

\(\left[ { H }^{ + } \right] ={ K }_{ a }\frac { \left[ Acid \right] }{ \left[ Salt \right] } \)
\(\left[ { H }^{ + } \right] ={ K }_{ a }\left[ Salt \right] \)
\(\left[ { H }^{ + } \right] ={ K }_{ a }\left[ Acid \right] \)
\(\left[ { H }^{ + } \right] ={ K }_{ a }\frac { \left[ Salt \right] }{ \left[ Acid \right] } \)

Henderson equation for a weak acid and its salt is

pH= pK_b +log (Salt) / (Acid)
pH = pK_a +log (Salt) / (Acid)
pH = pK_a +log (Salt) / (Base)
pH = pK_a + log (Acid) / (Salt)

Ostwald's dilution law is applicable in· the case of the solution of

CH₃COOH
NaCI
NaOH
H₂SO₄

Which of the following is not a Lewis acid?

SiCl₄
AlCl₃
SO₃
CO

Addition of sodium chloride to a saturated solution of silver chloride

dissociation of AgCl increases
concentration of Cl^- decreases
dissociation of AgCl^- decreases
concentration of Ag⁺ increases

The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively

acidic, acidic, basic
basic, acidic, basic
basic, neutral, basic
none of these

The ionic product of water at 25°C is_______

1 X 10^-7
1 X 10⁷
1 X 10^-14
1 X 10¹⁴

Which one among the following in the strongest Bronsted base

\(Cl{ O }_{ 4 }^{ - }\)
\(Cl{ O }_{ 3 }^{ - }\)
\(Cl{ O }_{2 }^{ - }\)
\(Cl{ O }^{ - }\)

___ can acts as both bronsted acid and Bronsted base.

\({ NH }_{ 4 }^{ + }\)
Cl^-
\({ HCO }_{ 3 }^{ - }\)
H₃O⁺

Dissociation constant ofNH40H is 1.8 x 10^-5 the hydrolysis constant of NH₄Cl would be

1.8 x 10^-19
5.55 x 10^-10
5.55 x 10^-5
1.80 x 10^-5

Electrophiles are______

Lewis acid
Lewis base
Bronsted acid
Bronsted base

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅NH) in a 0.10M aqueous pyridine solution (K_b for C₅H₅N =1.7 x l0^-9) is

0.006%
0.013%
0.77%
1.6%

If the solubility product of lead iodide is 3.2 x I0^-8, its solubility will be

2 x 10- ³M
4 x 10^-4M
1.6 x 10^-5 M
1.8 x 10^-5 M

\({ X }_{ m }{ Y }_{ n(s) }\overset { { H }_{ 2 }O }{ \rightleftharpoons } { mX }_{ (aq) }^{ n+ }+{ nY }_{ (aq) }^{ m- }\) solubility prouct K_sp is

\({ \left[ { X }^{ n+ } \right] }^{ m }{ \left[ { Y }^{ m- } \right] }^{ n }\)
\({ \left[ { X }^{ n+ } \right] }{ \left[ { Y }^{ m- } \right] }\)
\({ \left[ { X }^{ n+ } \right] }^{ m }/{ \left[ { Y }^{ m- } \right] }^{ n }\)
\({ \left[ { X }^{ n+ } \right] / }{ \left[ { Y }^{ m- } \right] }\)

According to ___ concept, BF₃ acts as a acid.

Bronsted.
Arrhenius
Lewis
None of the above

An acid is a substance that dissociates to give hydrogen ions in water. The above concept of acids was proposed by______

Lewis
Arrhenius
Bronsted
Lowry

Which of the following fluoro - compounds is most likely to behave as a Lewis base?

BF₃
PF₃
CF₄
SiF₄

pH of0.05 M H₂SO₄ is

1
2.6990
1.3010
1.6990

Degree if dissociation is nearly equal to 1 for

Strong acids and strong bases
Strong acids and weak bases
Weak acids and strong bases
Weak acids and weak bases

Part - B

Generic 2 - Answer All Question

Derive an expression for Ostwald’s dilution law.

Define solubility product.

Define Buffer solution.

A particular saturated solution of silver chromate Ag₂CrO₄ has [Ag⁺] = 5 x 10^-5 and [CrO_4]^2- = 4.4 x 10^-4 M. What is the value of K_sPfor Ag₂CrO4?

Why is aqueous solution of FeCl₃ acidic?

Give the Limitations of Arrhenius concept theory of acids and bases.

The K_a value for HCN is 10^-9. What is the pH of 0.4 M HCN solution?

Calculate the pH of 0.04 M HNO₃ Solution.

Write the expression for the solubility product of Ca₃ (PO₄)₂

Give a condition for , a compound to be precipitated.

Define neutralisation reaction.

A lab assistant prepared a solution by adding a calculated quantity of HC1 gas 25°C to get a solution with [H₃O⁺] = 4 x 10^-5 M. Is the solution neutral (or) acidic (or) basic.

Indentify the conjugate acid base pair for the following reaction in aqueous solution.
i) \({ HS }^ -_{ aq }\) + HF\(\rightleftharpoons \) \({ F }^ -_{ aq }\) + H₂S(aq)
ii) HP\({ O }_{ 3 }^{ 2- }\)- + \({ SO }_{ 3 }^{ 2- }\)\(\rightleftharpoons \) \({ PO }_{ 4 }^{ 3- }\) + \({ HSO }_{ 3 }^{ - }\)
iii) \({ NH }_{ 4 }^{ + }\) +\({ CO }_{ 3 }^{ 2- }\) \(\rightleftharpoons \) NH₃ + \({ HCO }_{ 3 }^{ - }\)

When temperature is increased, will ionic product of water increase or decrease? Give reason to justify your answer.

Calculate the pH of 1.5 x 10^-3 M solution of Ba(OH)₂.

Part - C

Generic 3 - Answer All Question

What is Henderson equation?

For an aqueous solution of NH₄Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)

How will you calculate solubility product from molar solubility?

What do you mean by buffer action?

Define buffer Index.

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