CBSE Questions for Class 11 Medical Chemistry Equilibrium Quiz 7 - MCQExams.com

What is rate?
  • Change / Time
  • Time / Concentration
  • Time / Change
  • Rate / Time
  • Concentration / Time
Assertion: $$NaCl(aq)$$ is an electrolyte.
Reason: It forms ions in solution.
  • Both Assertion and Reason are true and Reason is the correct explanation of Assertion
  • Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
  • Assertion is true but Reason is false
  • Assertion is false but Reason is true
  • Both Assertion and Reason are false
Statement I: Water makes a good buffer.
Statement II: A good buffer will resist changes in pH.
  • Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
  • Both the Statement 1 and Statement 2 are correct and Statement 2 is NOT the correct explanation of Statement 1
  • Statement 1 is correct but Statement 2 is not correct
  • Statement 1 is not correct but Statement 2 is correct
  • Both the Statement 1 and Statement 2 are not correct.
The Haber process is used for producing ammonia from nitrogen and hydrogen. This reaction could be forced to produce more ammonia by :
  • Increasing the reaction pressure
  • Decreasing the reaction pressure
  • Adding a catalyst
  • Both b and c
  • None of the above
The hydrogen sulfate or bisulfate ion, $$H{SO}_{4}^{-}$$, can act as either an acid or a base in water solution. In which of the following equations does $$H{SO}_{4}^{-}$$ act as an acid?
  • $$H{SO}_{4}^{-}+{H}_{2}O\rightarrow {H}_{2}{SO}_{4}+{OH}^{-}$$
  • $$H{SO}_{4}^{-}+{H}_{3}{O}^{+}\rightarrow {SO}_{3}+2{H}_{2}O$$
  • $$H{SO}_{4}^{-}+{OH}^{-}\rightarrow {H}_{2}{SO}_{4}+{O}^{2-}$$
  • $$H{SO}_{4}^{-}+{H}_{2}O\rightarrow {SO}_{4}^{2-}+{H}_{3}{O}^{+}$$
  • None of these
What does a buffer do?
  • It keeps the $$pH$$ of a solution from changing very much.
  • It maintains the equilibrium of a reaction.
  • It maintains the amount of acid in a solution
  • It maintains the amount of base in a solution
  • It keeps the $$pH$$ of a solution from changing at all.
It accepts a proton. It is called as:
  • a Bronsted acid
  • a Bronsted base
  • a strong acid
  • a weak base
The type of bonding present in a substance can be determined from experimental data.
Based on the information in the table below, which of the following substances is MOST likely to represent the identity of the solid?
Melting PointDensityConductivityConductivity in Aqueous Solution
$$801^{\circ}C$$$$2.17\ g/cc$$NoneExcellent
  • Platinum, $$Pt$$
  • Sodium chloride, $$NaCl$$
  • Glucose, $$C_{6}H_{12}O_{6}$$
  • Quartz, $$SiO_{2}$$
$$Ca{SO}_{4}$$ is somewhat soluble in water.
$$I$$. When $${H}_{2}{SO}_{4}$$ is added to a solution of $$Ca{SO}_{4}$$, the solubility of the $$Ca{SO}_{4}$$ will be increased.
$$II$$. The addition of $${H}_{2}{SO}_{4}$$ will lower the $$pH$$ of the solution.
  • Statement $$I$$ is true, Statement $$II$$ is true
  • Statement $$I$$ is true, Statement $$II$$ is false
  • Statement $$I$$ is false, Statement $$II$$ is true
  • Statement $$I$$ is false, Statement $$II$$ is false
The colour of bleaching powder is :
  • green
  • pale yellow
  • blue
  • white
Addition of water to this solution will not change $$[H_3 O^+]$$.
  • Chemical pH indicator
  • Acid/base buffer
  • Anhydrous solution
  • Hypotonic solution
Which of the following items are not bleached by bleaching powder?
  • Straw
  • Silk
  • Ivory
  • None of the above
For each pair of chemicals below, the amounts shown are dissolved, together, in water to make 1.0 L of solution. Which mixture will form a buffer solution?
  • 0.2 mol of $$\displaystyle HCl$$ and 0.1 mol of $$\displaystyle { K }_{ 2 }{ SO }_{ 3 }$$
  • 0.2 mol of $$\displaystyle NaOH$$ and 0.4 mol of $$\displaystyle HF$$
  • 0.1 mol of $$\displaystyle HBr$$ and 0.1 mol of $$\displaystyle Ba{ \left( OH \right) }_{ 2 }$$
  • 0.4 mol of $$\displaystyle HCl$$ and 0.2 mol of $$\displaystyle { NH }_{ 3 }$$
  • 0.2 mol of $$\displaystyle NaOH$$ and 0.4 mol of $$\displaystyle HCl$$
Bleaching powder loses ___________ by the action of dilute acids in excess.
  • oxygen
  • calcium
  • chlorine
  • water
On long standing, bleaching powder undergoes auto-oxidation into:
  • $$Ca(ClO_3)_2, CaCl_2$$
  • $$CaO, CaCl_2$$
  • $$CaClO, CaClO_3$$
  • $$CaClO_2, CaCl_2$$
Bleaching powder loses oxygen in the presence of:
  • calcium chloride
  • cobalt chloride
  • sodium chloride
  • none of the above

State whether the given statement is true or false.
Ideal solutions doesn't obey Roult's law.
  • True
  • False
Which of the following solutions show positive deviation from Raoult's law?
  • Acetone + Ethanol
  • Acetone + Benzene
  • Water + Methanol
  • All of the above
Which of the following compounds will be dissociated into its constituent ions?
  • Aqueous $$KCl$$
  • Solid $$KCl$$
  • Aqueous $$MgCl_2$$
  • Solid $$MgCl_2$$
An example for a neutral buffer is :
  • ammonium hydroxide and ammonium chloride
  • acetic acid and sodium acetate
  • acetic acid and ammonium hydroxide
  • citric acid and sodium citrate
Which of the following is false of a binary solution showing false deviation from Roult's law?
  • $$P_A < X_AP_A^o$$
  • $$\Delta H_{mix} < 0$$
  • $$\Delta V_{mix} < 0$$
  • None of the above
Dissociation events in $$H_2O \rightarrow H^+ +OH^-$$ is termed as ionization because :
  • the electron is initially shared between both atoms, thus the dissociation event into ions involves the transfer of an electron from one atom to the other
  • it does not involve any electron transfer
  • charged species formed
  • no charge species formed
When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because __________.
  • HCl is highly ionised in solution
  • HCl is highly soluble in water
  • The solubility product of NaCl is lowered by HCl
  • The ionic product of $$[Na^+] [Cl^-]$$ exceeds the solubility product of NaCl
Name of the organic acid present in tomato is :
  • tartaric acid
  • malic acid
  • lactic acid
  • oxalic acid
Sulfuric acid in air causes:
  • hair loss
  • acid precipitation
  • skin problems
  • respiratory problems
Which of the following statement is correct?
  • Sodium hydroxide turns blue litmus red
  • Nitric acid turns red litmus blue
  • Sodium hydroxide turns red litmus blue
  • Nitric acid does not change blue litmus to red
Which two sets of reactants best represents the amphoteric character of $$Zn{ \left( OH \right)  }_{ 2 }$$?
Set I   $$Zn{ \left( OH \right)  }_{ 2 }\left( s \right)$$ and $$ OH\left( aq \right)$$
Set II  $$Zn{ \left( OH \right)  }_{ 2 }\left( s \right)$$ and $$ { H }_{ 2 }O\left( I \right)$$
Set III $$Zn{ \left( OH \right)  }_{ 2 }\left( s \right)$$ and $$ { H }^{ + }\left( aq \right)$$
Set IV $$Zn{ \left( OH \right)  }_{ 2 }\left( s \right)$$ and $$ N{ H }_{ 3 }\left( aq \right) $$
  • III and II
  • I and III
  • IV and I
  • II and IV
A chemical which turns red litmus to blue is:
  • acidic in nature
  • basic in nature
  • neutral in nature
  • can be acidic or basic in nature
How many grams of ammonium chloride should be dissolved in 500 mL of water to have a solution of pH 4.5? 

[$$\displaystyle K_b$$ for ammonium hydroxide is $$ \displaystyle1.8 \times 10^{-5}$$]
  • 25.22
  • 48.15
  • 53.5
  • 90
The process in which metal surface is made inactive is called:
  • passivation
  • galvanizing
  • corrosion
  • pickling
Ammonia is basic in nature. Hence it turns:
  • red litmus to blue
  • blue litmus to red
  • white litmus to red
  • white litmus to blue
Degree of ionisation does not depend on:
  • nature of the solvent
  • nature of the electrolyte
  • dilution
  • molecular mass of the electrolyte
Curd taste sour because this is a/an :
  • base
  • salt
  • acid
  • liquid
When a blue litmus paper is dipped in a solution, it remains blue. What can be concluded about this solution?
  • Th solution is neutral.
  • The solution is basic or neutral.
  • The solution is acidic or neutral.
  • None of the above.
The number of ions given by one molecule of $$K_{4}Fe(CN)_{6}$$ after complete dissociation is____________.
  • $$5$$
  • $$11$$
  • $$2$$
  • $$10$$
Which of the following will not function as a buffer solution?

$$(i)$$ $$NaCl$$ and $$NaOH$$
$$(ii)$$ $$NaOH$$ and $${NH}_{4}OH$$
$$(iii)$$ $${CH}_{3}COO{NH}_{4}$$ and $$HCl$$
$$(iv)$$ Borax and boric acid
  • $$(i),(ii),(iii)$$
  • $$(ii),(iii),(iv)$$
  • $$(i),(iii),(iv)$$
  • $$(i),(ii),(iii),(iv)$$
The state of equilibrium refers to:
  • State of rest
  • Dynamic state
  • Stationary state
  • State of inertness
Acid turns blue litmus to:
  • White
  • Yellow
  • Red
  • Green
A monoprotic acid in $$1.00M$$ solution is $$0.001$$% ionised. The dissociation constant of acid is:
  • $$1\times { 10 }^{ -3 }$$
  • $$1\times { 10 }^{ -6 }$$
  • $$1\times { 10 }^{ -8 }$$
  • $$1\times { 10 }^{ -10 }$$
Which pair will show common ion effect?
  • $$Ba{ Cl }_{ 2 }+Ba{ \left( { NO }_{ 3 } \right) }_{ 2 }$$
  • $$NaCl+HCl$$
  • $${ NH }_{ 4 }OH+{ NH }_{ 4 }Cl$$
  • $$AgCN+KCN$$
When $${ NH }_{ 4 }Cl$$ is added to $${ NH }_{ 4 }OH$$ solution, the dissociation of ammonium hydroxide is reduced. It is due to:
  • common ion effect
  • hydrolysis
  • oxidation
  • reduction
A monoprotic acid in $$1.00M$$ solution is $$30$$% ionised. The dissociation constant of acid is related degree dissociation as:
  • $${ \alpha }^{ 2 }C+\alpha K-K=0$$
  • $${ \alpha }^{ 2 }C-\alpha K-K=0$$
  • $${ \alpha }^{ 2 }C-\alpha K+K=0$$
  • $${ \alpha }^{ 2 }C+\alpha K+K=0$$
The ionisation constant of acetic acid is $$1.8\times { 10 }^{ -5 }$$. The concentration at which it will be dissociated to $$2$$% is:
  • $$1M$$
  • $$0.045M$$
  • $$0.018M$$
  • $$0.45M$$
One litre of water contains $${ 10 }^{ -7 }$$ mole of $${H}^{+}$$ ions. Degree of ionisation of water is:
  • $$5 . 4\times { 10 }^{ -7 }$$
  • $$1.8\times { 10 }^{ -7 }$$
  • $$0.8\times { 10 }^{ -9 }$$
  • $$5. 4\times { 10 }^{ -9 }$$
Which one does not give a buffer solution?
  • Ammonia and sodium hydroxide in water
  • Sodium acetate and acetic acid in water
  • Ammonia and ammonium chloride in water
  • Sodium acetate and hydrochloric acid in water
A certain weak acid has dissociation constant of $$1.0\times { 10 }^{ -4 }$$. The equilibrium constant for its reaction with a strong base is:
  • $$1.0\times { 10 }^{ -4 }$$
  • $$1.0\times { 10 }^{ -10 }$$
  • $$1.0\times { 10 }^{ 10 }$$
  • $$1.0\times { 10 }^{ -14 }$$
The pH of a neutral water is $$6.5$$. Then the temperature of water:
  • Is $${ 25 }^{ o }C$$
  • Is more than $${ 25 }^{ o }C$$
  • Is less than $${ 25 }^{ o }C$$
  • Can be more or less than $${ 25 }^{ o }C$$
  • Cannot be predicted
The dissociation constants of two acids $$ H{ A }_{ 1 }$$ and $$H{ A }_{ 2 }$$ are $$3.0\times { 10 }^{ -4 }$$ and $$1.8\times { 10 }^{ -5 }$$ respectively. The relative strengths of the acids will be:
  • $$1:4$$
  • $$4:1$$
  • $$1:16$$
  • $$16:1$$
The $$pH$$ of an aqueous solution of a $$0.1M$$ solution of a weak monoprotic acid which is $$1$$% ionised is:
  • $$1$$
  • $$2$$
  • $$3$$
  • $$11$$
Which of the following statements is correct?
  • $$p{ K }_{ w } $$ increases with increase of temperature
  • $$p{ K }_{ w }$$ decreases with increase of temperature
  • $$p{ K }_{ w }=14$$ at all temperatures
  • $$p{ K }_{ w }=pH $$ at all temperatures
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