JEE Questions for Chemistry Equilibrium Quiz 11 - MCQExams.com

Which of the following solution acts as a buffer?
  • HCl + NaCl
  • NaOH + NaCl
  • CH3COOH + CH3COONa
  • HCOOH + HCOONH4
Which buffer solution comprising of the following has its pH value greater than 7:
  • CH3COOH + CH3COONa
  • HCOOH + HCOOK
  • CH3COONH4
  • NH4OH + NH4Cl
Which of the following salt undergoes hydrolysis?
  • KCl
  • K2SO4
  • NaNo3
  • K2C2O4
On dissolving a salt in water (pH=7), the pH of the solution was found to be greater than 7. It must be salt of
  • strong acid, weak base
  • weak acid, strong base
  • strong acid, strong base
  • weak acid, weak base
For the salt of weak acid and strong base, the hydrolysis constant is given by the expression

  • Chemistry-Equilibrium-3917.png
  • 2)
    Chemistry-Equilibrium-3918.png

  • Chemistry-Equilibrium-3919.png

  • Chemistry-Equilibrium-3920.png
Which of the following relations is correct for degree of hydrolysis of CH3COONH4 ?

  • Chemistry-Equilibrium-3921.png
  • 2)
    Chemistry-Equilibrium-3922.png

  • Chemistry-Equilibrium-3923.png

  • Chemistry-Equilibrium-3924.png
Which one of the following statements is incorrect?
  • In Group II of analysis, the solution is acidified before passing H2S to decreases S2- ion conc.
  • In Group IV, the solution is made ammoniacal before passing H2S to increase S2- ion concentration
  • Solubility products to sulphides of Group II radicals are higher than those of Group IV radicals
  • Solubility product can be calculated from the concentrations of the ions only if the solution is saturated
The units of lonic product of water (kw) are :
  • mol-1 L-1
  • mol-2 L-2
  • mol-2 L-1
  • mol2 L-2
During the precipitation of third group of qualitative analysis, ammonium chloride is added before adding ammonium hydroxide. The function of NH4Cl is to
  • increase the ionisation of NH4OH
  • supress the ionisation of NH4OH
  • convert the ions of group third into their respective chlorides
  • stabilise the hydroxides of Group III cations
At 900 C, pure water has [H3O+] = 10–6 mol L–1. What is the value of Kw at 900 C ?
  • 10–6
  • 10–12
  • 10–14
  • 10–8
Which of the following salts undergoes anionic hydrolysis?
  • CuSO4
  • NH4Cl
  • FeCl3
  • Na2CO3
Which of the following is most soluble?

  • Chemistry-Equilibrium-3927.png
  • 2)
    Chemistry-Equilibrium-3928.png

  • Chemistry-Equilibrium-3929.png

  • Chemistry-Equilibrium-3930.png
The best indicator for the detection of end point in titration of a weak acid and a strong base is
  • Methyl orange (3 to 4)
  • Methyl red (5 to 6)
  • Bromothymol blue (6 t0 7.
  • Phenolphthalein (8 to 9.6)
The compound whose 0.1 M solution is basic is
  • Ammonium acetate
  • Ammonium chloride
  • Ammonium sulphate
  • Sodium acetate
The term pH comes from
  • pure hydrogen content
  • “potenz de hydrogen” which implies potential of hydrogen
  • purity of hydrogen ions in solution
  • name of the scientist associated
When equal volumes of the following solutions are mixed, precipitation of AgCl(Ksp = 1.8 × 10–10) will occur only with
  • 10–4 MAg+ and 10–4 Cl–
  • 10–5 MAg+ and 10–5 Cl–
  • 10–6 MAg+ and 10–6 Cl–
  • 10–10 MAg+ and 10–10 Cl–
The pKa of acetyl salicyclic acid (aspirin) is 3.5. The pH of gastric juice in human stomach is about 2-3 and pH in the small intestine is about 8. Aspirin will be
  • unionised in the small intestine and in the stomach
  • completely ionised in the small intestine and in the stomach
  • ionised in the stomach and almost unionised in the small intestine
  • ionised in the small intestine and almost unionised in the stomach
The compound whose water solution has the highest pH is
  • NaCl
  • NaHCo3
  • Na2CO3
  • NH4Cl
The acidic buffer solution can be prepared by mixing solutions of
  • Sodium acetate and acetic acid
  • Ammonium chloride and ammonium hydroxide
  • Sulphuric acid and sodium sulphate
  • Sodium chloride and sodium hydroxide
Amongst the following hydroxides, the one which has the lowest value of Ksp at ordinary temperature (about 25o C) is
  • Mg(OH)2
  • Ca(OH)2
  • Ba(OH)2
  • Be(OH)2
Out of Ca2+, Al3+, Bi3+, Mg2+ and Zn2+ the reagents NH4Cl and aqueous NH3 will precipitate
  • Ca2+, Al3+
  • Al3+, Bi3+
  • Bi3+, Mg2+
  • Mg2+, Zn2+
The pH of the neutralisation point of 0.1 N ammonium hydroxide with 0.1 N HCl is
  • 1
  • 6
  • 7
  • 9
Aqueous solution of acetic acid contains
  • CH3COO– and H+
  • CH3COO–, H3O+ and CH3COOH
  • CH3COO-, H3O+ and H+
  • CH3COOH, CH3COO– and H+
The following equilibrium is established when hydrogen chloride is dissolved is acetic acid
Chemistry-Equilibrium-3932.png

  • Chemistry-Equilibrium-3933.png
  • 2)
    Chemistry-Equilibrium-3934.png

  • Chemistry-Equilibrium-3935.png

  • Chemistry-Equilibrium-3936.png
The precipitate of CaF2 (Ksp = 1.7 × 10–) is obtained when equal volumes of the following are mixed
  • 10–4 M Ca3+ + 10–4 MF–
  • 10–2 M Ca2+ + 10–3 MF–
  • 10–5 M Ca2+ + 10–3 MF–
  • 10–3 M Ca2+ + 10–5 MF–
0.1 M solution of which one of these substances will react basic?
  • Sodium borate
  • Ammonium chloride
  • Calcium nitrate
  • Sodium sulphate
What is the decreasing order of strength of the bases
Chemistry-Equilibrium-3938.png

  • Chemistry-Equilibrium-3939.png
  • 2)
    Chemistry-Equilibrium-3940.png

  • Chemistry-Equilibrium-3941.png

  • Chemistry-Equilibrium-3942.png
In which of the following, the solubility of AgCl will be maximum?
  • 0.1 M NaNO3
  • water
  • 0.1 M NaCl
  • 0.1 M NaBr
The correct order of increasing [H3O+] in the aqueous solution is
  • 0.01 M H2S < 0.01 M H2SO4 < 0.01 M NaCl < 0.01 M NaNO2
  • 0.01 M NaCl < 0.01 M NaNO2 < 0.01 M H2S < 0.01 M H2SO4
  • 0.01 M NaNO2 < 0.01 M NaCl < 0.01 M H2S < 0.01 M H2SO4
  • 0.01 M H2S < 0.01 M NaNO2 < 0.01 M NaCl < 0.01M H2SO4
The solubility of AgBrO3 in an aqueous solution of NaBrO3 (as compared to that in water) is
  • the same
  • more
  • less
  • Unpredicatable due to a new chemical reaction
Choose the solution with lowest pH value
  • CaCO3
  • CH3COONa
  • Ca(OH)2
  • CaCl2
When NaCl is added to the reaction mixture of an oil and caustic soda, the soap is thrown out because
  • NaCl is an ionic compound
  • Soap is insoluble in the presence of chloride ions
  • The solubility product of NaCl decreases in the presence of soap
  • The solubility of the soap is exceeded due to the increased concentration of Na+ ions.
Which equilibrium can be described as an acid-base reaction using the Lewis acid- base definition, but not using Bronsted –Lowry definition?

  • Chemistry-Equilibrium-3945.png
  • 2)
    Chemistry-Equilibrium-3946.png

  • Chemistry-Equilibrium-3947.png

  • Chemistry-Equilibrium-3948.png
Sodium carbonate cannot be used in place of ammonium carbonate for the identification of the fifth group radicals. This is because the
  • sodium ions will interfere in the detection of the fifth group radicals
  • concentration of carbonate ions is very low
  • sodium will react with acidic radicals
  • magnesium will be precipitated
The pH of blood does not appreciably change by a small addition of acid or a base because blood
  • contains serum protein which acts as buffer
  • contains iron as a part of the molecule
  • can be easily coagulated
  • is body fluid
The solubility of calcium phosphate in water is x mol L–1 at 25o C. Its solubility product is equal to
  • 108x2
  • 36x3
  • 36x5
  • 108x5
The Ksp of CuS, Ag2S and HgS are 10–31,10–44 and 10–54 respectively The solubility of these sulphides are in the order
  • Ag,sub>2S > CuS > HgS
  • AgS > HgS > CuS
  • HgS >Ag,sub>2S > CuS
  • CuS >Ag2S >HgS
A physician wishes to prepare a buffer solution at pH = 3.58 that efficiently resists a change in pH yet contain only small conc. of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use?
  • m - Chloro benzoic acid (pKa = 3.98)
  • p - Chlorocinnamic acid (pKa = 4.41)
  • 2,5-dihydroxy benzoic acid (pKa = 2.97)
  • Acetoacetic acid (pKa =3.58)

Chemistry-Equilibrium-3952.png
  • I2
  • I–

  • Chemistry-Equilibrium-3953.png
  • None
Which of the following on reaction with H2S does not produce metallic sulphide?
  • CdCl2
  • ZnCl2
  • COCl2
  • CuCl2
What is the value of Ksp for PbCl2 ?

  • Chemistry-Equilibrium-3954.png
  • 2)
    Chemistry-Equilibrium-3955.png

  • Chemistry-Equilibrium-3956.png

  • Chemistry-Equilibrium-3957.png
1 M NaCl and 1 MHCl are present in an aqueous solution. The solution is
  • not a buffer solution with pH < 7
  • not a buffer solution with pH > 7
  • a buffer solution with pH < 7
  • a buffer solution with pH > 7
Species acting both as Bronsted acid and base is
  • (HSO4)–1
  • Na2CO3
  • NH3
  • OH–1
How do we differentiate between Fe3+ and Cr3+ in group III ?
  • by taking excess of NH4OH
  • 2)
    Chemistry-Equilibrium-3960.png
  • by decreasing OH− ion concentration
  • both (b) and (c)
In which of the following acid-base titration,pH is greater than 8 at the equivalence point?
  • Acetic acid versus ammonia
  • Acetic acid versus sodium hydroxide
  • Hydrochloric acid versus ammonia
  • Hydrocholric acid versus sodium hydroxide
Which one of the following statements is not true?
  • pH + pOH = 14 for all aqueous solutions
  • The pH of 10-8 M HCl is 8
  • 96,500 coulombs of electricity when passed through a CuSO4 solution deposites 1 gram equivalent of copper at the cathode

  • Chemistry-Equilibrium-3961.png
When rain is accompanied by a thunderstorm, the collected rain water will have pH value
  • slightly higher than that when the thunderstorm is not there
  • uninfluenced by occurrence of thunderstorm
  • which depends on the amount of dust in air
  • slightly lower than that of rain water without thunderstorm
A solution which is 10-3 M each in Mn2+,Fe2+,Zn2+ and Hg2+ is treated with 10-16 M sulphide ion. If Ksp of MnS, FeS, ZnS and HgS are 10-15, 10-23, 10-20, and 10-54 respectively, which one will precipitate first ?
  • FeS
  • MgS
  • HgS
  • ZnS
The hydrogen ion concentration of 0.2 N CH3COOH which is 40% dissociated is
  • 0.08N
  • 0.12N
  • 0.80N
  • 1.2N
The gastric juice in our stomach contains enough HCl to make the hydrogen ion concentration about 0.01 mole/litre.The pH of gastric juice is
  • 0.01
  • 1
  • 2
  • 14
0:0:1


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