An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

Question

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

A. 16 x $10^{- 8}$

B. 3.2 x 10 $10^{- 11}$

C. 3.2 x $10^{- 6}$

D. 0.156 x $10^{- 2}$

Share this question with your friends

Show all ionic Equilibrium MCQ

Comment

pH of a solution is 8.5. solution is

A. amphoteric

B. neutral

C. acids

D. basic

Discuss this answer

pH of a solution is 10. Hydroxide ion concentration in the solution is

A. $10^{- 10}$ gm eq.

B. $10^{- 4}$ mole $l i t e r^{- 1}$

C. $10^{- 4}$ gm $l i t e r^{- 1}$

D. $10^{- 3}$ gm eq.

Discuss this answer

On dissolving sodium chloride in water pH of the solution

A. decreases

B. increases

C. remains unchanged

D. increase or decreases

Discuss this answer

If $N H_{3}$ is dissolved in water, pH of the solution

A. decreases

B. increases

C. remains unchanged

D. may increase or decrease

Discuss this answer

Conjugate base of $H C O_{3}^{-}$ is

A. $H C O_{3}^{2 -}$

B. $H C O_{3}^{+}$

C. $H_{2} C O_{3}^{-}$

D. $C O_{3}^{2 -}$

Discuss this answer

On dissolving copper sulphate in water pH of the solution

A. decreases

B. increases

C. remains unchanged

D. may increase or decrease

Discuss this answer

Which of the following is not hydrolysed in water ?

A. $H C O O N a$

B. KCN

C. $K_{2} C O_{3}$

D. KC1

Discuss this answer

During salt analysis $N H_{4} O H$ is added before adding NH4OH for third gp., cation analysis so as to

A. increase the concentration of $O H^{-}$ ions

B. increase the concentration of ammonia

C. increase the concentration of chloride ions

D. prevent the precipitation of hydroxides of subsequent groups

Discuss this answer

Solubility of calcium carbonate is 0.0305 gm/litre. $K_{s p}$ for $C a C O_{3}$ is

A. 0.000305

B. 193 x $10^{- 8}$

C. 9.3 x $10^{- 8}$

D. 93.05 x $1^{- 5}$

Discuss this answer

Strength of an acid depends on

A. hydrolysis

B. concentration of $O H^{-}$ ions

C. concentration of $H^{+}$ ions

D. no. of moles of base used for neutralisation

Discuss this answer

pH of 0.1 M monoprotic acid is 4. Then dissociation constant of the acid is :

A. 9

B. $10^{- 7}$

C. $10^{- 5}$

D. $1^{- 3}$

Discuss this answer

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

A. 16 x $10^{- 8}$

B. 3.2 x 10 $10^{- 11}$

C. 3.2 x $10^{- 6}$

D. 0.156 x $10^{- 2}$

Discuss this answer

Which of the following is not hydrolysed in water ?

A. $H C O O N a$

B. KCN

C. $K_{2} C O_{3}$

D. KC1

Discuss this answer

Ionisation constant of formic acid is 1.8 x $1.8 \times 10^{- 4}$ at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

A. 0.18

B. 42.4

C. 4.24

D. 2.89

Discuss this answer

Ostwald dilution law is applicable for :

A. weak electrolytes

B. strong electorate

C. basic

D. acids

Discuss this answer

Conjugate acid differs from its conjugate base by

A. proton

B. meson

C. electron pair

D. positron

Discuss this answer

Acetic acid is weak acid because it is

A. organic acid

B. immiscible with water

C. slightly ionised

D. viscous

Discuss this answer

Sum of pH and pOH of an acidic solution at $25 ° C$ is

A. 0

B. 14

C. depends on pH of base

D. depends on pH of acid

Discuss this answer

pH of 0.1 M monobasic acid is 4 then molar concentration of $H^{+}$ per litre will be

A. $10^{- 8}$

B. $20 \times 10^{5}$

C. $10^{- 3}$

D. $10^{- 4}$

Discuss this answer

Molar concentration of $A g^{+}$ in an aqueous solution of $A g_{2} C r O_{4}$ at 298K is 1.5 x $10^{- 4}$ $K_{s p}$ , for $A g_{2} C r O_{4}$ is

A. 1.125 x $10^{- 8}$

B. 2.5 x $10^{- 4}$

C. 2.25 x $10^{- 8}$

D. 1.6875 x $10^{- 12}$

Discuss this answer

According to Bronsted Lowry an acid is

A. that gives cation in solution

B. one that gives $H^{+}$ ions in solution

C. electron acceptor

D. proton donor

Discuss this answer

2 gm of NaOH is dissolved in one litre water. pH of the solution will be

A. 12.7

B. 11.7

C. 1.3

D. 17.7

Discuss this answer

$C H_{3} C O O H + H_{2} ⇋ H_{3} O^{+} + C H_{3} C O O^{-}$
In the above reaction acid is

A. $H_{3} O^{+}$

B. $H_{2} O$

C. $C H_{3} C O O H$

D. $C H_{3} C O O H a n d H_{3} O^{+}$

Discuss this answer

In III gp of salt analysis for cations $N H_{4} C L$ and $N H_{4} O H$ are added as group reagents. Which of the following can be used instead of $N H_{4} C L$ ?

A. $N H_{4} N O_{3}$

B. NaCL

C. ${(N H_{4})}_{2} S O_{4}$

D. ${(N H_{4})}_{2} C_{2} O_{4}$

Discuss this answer

Dissociation constant of 0.01 M HCN is 4 x $10^{- 10}$ . The $H^{-}$ concentration in the solution is

A. $3 \times 10^{- 6} m o l e l i t^{- 1}$

B. $2 \times 10^{- 6} m o l e l i t^{- 1}$

C. $5 \times 10^{- 10} m o l e l i t^{- 1}$

D. $5 \times 10^{- 8} m o l e l i t^{- 1}$

Discuss this answer

In an aquous solution of silver bromide concentration of $A g^{+} i s 1 \times 10^{- 6} m o l l i t^{- 1}$ . If $K_{s p}$ for AgBr is
4 x $10^{- 13}$ then concentration of Br in the solution is

A. 4 x $10^{- 8}$ mole $l i t e r^{- 1}$

B. 2 x $10^{- 19}$ mole $l i t e r^{- 1}$

C. 4 x $10^{- 7}$ mole $l i t e r^{- 1}$

D. 2 x $10^{- 5}$ mole $l i t e r^{- 1}$

Discuss this answer

At a given temperature $P b I_{2}$ will be more soluble in

A. water

B. 0.02 M Nal

C. O.4 M Pb ${(N O_{3})}_{2}$

D. 0.02 MKI

Discuss this answer

A solution is said to be saturated w.r.t the electrolyte it contains if

A. ionic product < $K_{s p}$

B. ionic product > $K_{s p}$

C. $[i o n i c p r o d u c t]^{2}$ = $K_{s p}$

D. ionic product = $K_{s p}$

Discuss this answer

$B a S O_{4}$ (Mol. wt 233) has solubility 0.009 gm $l i t^{- 1}$ at 298 K. Its solubility product is

A. 1.521 x $10^{- 5}$

B. 152.1 x $10^{- 19}$ 10"19

C. 1.9 x $10^{- 5}$

D. 15.21 x $10^{- 9}$

Discuss this answer

Decinormal solution of acetic acid ionised to an extent of 1.3%. pH of this solution will be (log 1.3 = 0.11)

A. 3.89

B. 2.89

C. 4

D. 1.0

Discuss this answer

Accepted Answer

B. 3.2 x 10

10^{- 11}

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

Correct Answer :

Show all ionic Equilibrium MCQ

Related Questions

pH of a solution is 8.5. solution is

pH of a solution is 10. Hydroxide ion concentration in the solution is

On dissolving sodium chloride in water pH of the solution

If $N H_{3}$ is dissolved in water, pH of the solution

Conjugate base of $H C O_{3}^{-}$ is

On dissolving copper sulphate in water pH of the solution

Which of the following is not hydrolysed in water ?

During salt analysis $N H_{4} O H$ is added before adding NH4OH for third gp., cation analysis so as to

Solubility of calcium carbonate is 0.0305 gm/litre. $K_{s p}$ for $C a C O_{3}$ is

Strength of an acid depends on

pH of 0.1 M monoprotic acid is 4. Then dissociation constant of the acid is :

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

Which of the following is not hydrolysed in water ?

Ionisation constant of formic acid is 1.8 x $1.8 \times 10^{- 4}$ at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

Ostwald dilution law is applicable for :

Conjugate acid differs from its conjugate base by

Acetic acid is weak acid because it is

Sum of pH and pOH of an acidic solution at $25 ° C$ is

pH of 0.1 M monobasic acid is 4 then molar concentration of $H^{+}$ per litre will be

Molar concentration of $A g^{+}$ in an aqueous solution of $A g_{2} C r O_{4}$ at 298K is 1.5 x $10^{- 4}$ $K_{s p}$ , for $A g_{2} C r O_{4}$ is

According to Bronsted Lowry an acid is

2 gm of NaOH is dissolved in one litre water. pH of the solution will be

$C H_{3} C O O H + H_{2} ⇋ H_{3} O^{+} + C H_{3} C O O^{-}$
In the above reaction acid is

In III gp of salt analysis for cations $N H_{4} C L$ and $N H_{4} O H$ are added as group reagents. Which of the following can be used instead of $N H_{4} C L$ ?

Dissociation constant of 0.01 M HCN is 4 x $10^{- 10}$ . The $H^{-}$ concentration in the solution is

In an aquous solution of silver bromide concentration of $A g^{+} i s 1 \times 10^{- 6} m o l l i t^{- 1}$ . If $K_{s p}$ for AgBr is
4 x $10^{- 13}$ then concentration of Br in the solution is

At a given temperature $P b I_{2}$ will be more soluble in

A solution is said to be saturated w.r.t the electrolyte it contains if

$B a S O_{4}$ (Mol. wt 233) has solubility 0.009 gm $l i t^{- 1}$ at 298 K. Its solubility product is

Decinormal solution of acetic acid ionised to an extent of 1.3%. pH of this solution will be (log 1.3 = 0.11)

Also checkout

An aqueous solution CaF2 contains 2 x 10-4mole lit-1 of CaF2. Ksp for CaF2 is

Correct Answer :

Show all ionic Equilibrium MCQ

Related Questions

pH of a solution is 8.5. solution is

pH of a solution is 10. Hydroxide ion concentration in the solution is

On dissolving sodium chloride in water pH of the solution

If NH3 is dissolved in water, pH of the solution

Conjugate base of HCO3-is

On dissolving copper sulphate in water pH of the solution

Which of the following is not hydrolysed in water ?

During salt analysis NH4OH is added before adding NH4OH for third gp., cation analysis so as to

Solubility of calcium carbonate is 0.0305 gm/litre.Kspfor CaCO3 is

Strength of an acid depends on

pH of 0.1 M monoprotic acid is 4. Then dissociation constant of the acid is :

An aqueous solution CaF2 contains 2 x 10-4mole lit-1 of CaF2. Ksp for CaF2 is

Which of the following is not hydrolysed in water ?

Ionisation constant of formic acid is 1.8 x 1.8×10-4 at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

Ostwald dilution law is applicable for :

Conjugate acid differs from its conjugate base by

Acetic acid is weak acid because it is

Sum of pH and pOH of an acidic solution at 25°C is

pH of 0.1 M monobasic acid is 4 then molar concentration of H+ per litre will be

Molar concentration of Ag+ in an aqueous solution of Ag2CrO4 at 298K is 1.5 x 10-4 Ksp, for Ag2CrO4 is

According to Bronsted Lowry an acid is

2 gm of NaOH is dissolved in one litre water. pH of the solution will be

CH3COOH+H2⇋H3O++CH3COO-In the above reaction acid is

In III gp of salt analysis for cations NH4CL and NH4OH are added as group reagents. Which of the following can be used instead of NH4CL ?

Dissociation constant of 0.01 M HCN is 4 x10-10. The H- concentration in the solution is

In an aquous solution of silver bromide concentration of Ag+ is 1×10-6 mol lit-1. If Ksp for AgBr is 4 x 10-13 then concentration of Br in the solution is

At a given temperature PbI2 will be more soluble in

A solution is said to be saturated w.r.t the electrolyte it contains if

BaSO4(Mol. wt 233) has solubility 0.009 gmlit-1 at 298 K. Its solubility product is

Decinormal solution of acetic acid ionised to an extent of 1.3%. pH of this solution will be (log 1.3 = 0.11)

Also checkout

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

If $N H_{3}$ is dissolved in water, pH of the solution

Conjugate base of $H C O_{3}^{-}$ is

During salt analysis $N H_{4} O H$ is added before adding NH4OH for third gp., cation analysis so as to

Solubility of calcium carbonate is 0.0305 gm/litre. $K_{s p}$ for $C a C O_{3}$ is

An aqueous solution $C a F_{2}$ contains 2 x $10^{- 4}$ mole $l i t^{- 1}$ of $C a F_{2}$ . $K_{s p} f o r C a F_{2 i s}$

Ionisation constant of formic acid is 1.8 x $1.8 \times 10^{- 4}$ at 298 K. In 0.1 NHCOOH the percentage ionisation of HCOOH acid is

Sum of pH and pOH of an acidic solution at $25 ° C$ is

pH of 0.1 M monobasic acid is 4 then molar concentration of $H^{+}$ per litre will be

Molar concentration of $A g^{+}$ in an aqueous solution of $A g_{2} C r O_{4}$ at 298K is 1.5 x $10^{- 4}$ $K_{s p}$ , for $A g_{2} C r O_{4}$ is

$C H_{3} C O O H + H_{2} ⇋ H_{3} O^{+} + C H_{3} C O O^{-}$
In the above reaction acid is

In III gp of salt analysis for cations $N H_{4} C L$ and $N H_{4} O H$ are added as group reagents. Which of the following can be used instead of $N H_{4} C L$ ?

Dissociation constant of 0.01 M HCN is 4 x $10^{- 10}$ . The $H^{-}$ concentration in the solution is

In an aquous solution of silver bromide concentration of $A g^{+} i s 1 \times 10^{- 6} m o l l i t^{- 1}$ . If $K_{s p}$ for AgBr is
4 x $10^{- 13}$ then concentration of Br in the solution is

At a given temperature $P b I_{2}$ will be more soluble in

$B a S O_{4}$ (Mol. wt 233) has solubility 0.009 gm $l i t^{- 1}$ at 298 K. Its solubility product is