Common Ion Ef...

Common Ion Effect

Trending Questions

Q. The dissociation constants for acetic acid and

H C N

25 ° C

are

1.5 \times 10^{- 5}

and

4.5 \times 10^{- 10}

respectively. The equilibrium constant for the equilibrium,

C N^{-} + C H_{3} C O O H ⇌ H C N + C H_{3} C O O^{-}

would be:

$3.33 \times 10^{- 5}$
$3.33 \times 10^{- 4}$
$3.33 \times 10^{4}$
$3.33 \times 10^{- 5}$

View Solution

What is ionization?

View Solution

Q. A solution containing 8.6 g urea in 1 L was found to be isotonic with a 5%(weight/volume) solution of an organic non-volatile solute. The molecular weight of latter is

3489
861.2
348.9
34.89

View Solution

Why is it necessary to use acetic acid and not sulphuric acid for acidification of sodium extract for testing sulphur by lead acetate test?

View Solution

The ionization constant of propanoic acid is $1.32 \times 10^{- 5}$ . Calculate the degree of ionization of the acid in its 0.05M solution and also its pH. What will be its degree of ionization if the solution is 0.01M in HCl also?

View Solution

Q. The amount (in g) of H2SO4 present in 250 ml of 1M solution is Solve using law of equivalence .

View Solution

Q. White precipitate of

A g C l

dissolves in aqueous ammonia solution due to formation of:

View Solution

The ionization constant of phenol is $1.0 \times 10^{- 10}$ . What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01M in sodium phenolate?

View Solution

Q. Concentration of H2SO4 is 98% H2SO4 by mass and has density of 1.8 g/L. Volume of acid needed to make one litre of 0.1 M H2SO4

View Solution

Q. What is the decreasing order of strength of the bases

O H^{-}, N H_{2}^{-}, H C \equiv C^{⊝}

and

C H_{3} - C H_{2}^{⊝}

$C H_{3} - C H_{2}^{⊝} > N H_{2}^{⊝} > H - C \equiv C^{⊝} > O H^{⊝}$
$H - C \equiv C^{⊝} > C H_{3} - C H_{2}^{⊝} > N H_{2}^{⊝} O H^{⊝}$
$O H^{⊝} > N H_{2}^{⊝} > H - C \equiv C^{⊝} > C H_{3} - C H_{2}^{⊝}$
$N H_{2}^{⊝} > H - c \equiv C^{⊝} > O H^{⊝} > C H_{3} - C H_{2}^{⊝}$

View Solution

When the pH of the solution decreases, its hydrogen ion concentration

increases
decreases
nothing can be said
remains same

View Solution

Q. A solution contains 0.1 M

H_{2} S

and 0.3 M HCl. Calculate the conc. of

S^{2 -}

and

H S^{-}

ions in solution, Given

K_{a_{1}}

and

K_{a_{2}}

for

H_{2} S

are

10^{- 7}

and

1.3 \times 10^{- 13}

respectively.

$1.43 \times 10^{- 20} M, 3.3 \times 10^{- 8} M$
$1.43 \times 10^{- 10} M, 3.3 \times 10^{- 4} M$
$2.83 \times 10^{- 19} M, 3.3 \times 10^{- 8} M$
$1.43 \times 10^{- 19} M, 1.65 \times 10^{- 8} M$

View Solution

Which is more soluble Mg(oh)2 or. Ba(oh)2

While comparing solubility do we compare Ksp(solubility product values) or solubility (s) value

View Solution

Q. Sucrose solution which is 40% by mass is heated till it becomes 50% by mass. Water lost from 100 g of the solution is (a) 10g (b) 15g (c) 20g (d) 25

View Solution

Q. Among the following oxoacids, the correct decreasing order of acid strength is

$H O C l > H C I O_{2} > H C l O_{3} > H C l O_{4}$
$H C l O_{2} > H C l O_{4} > H C l O_{3} > H O C l$
$H C l O_{4} > H O C l > H C l O_{2} > H C l O_{3}$
$H C l O_{4} > H C l O_{3} > H C l O_{2} > H O C l$

View Solution

Q. Calculate the pH of a solution made by adding

0.001 mol of N a O H to 100 {cm}^{3}

of solution which is

0.50 M

C H_{3} C O O H and 0.5 M in C H_{3} C O O N a

$6.50$
$7.80$
$3.56$
$4.76$

View Solution

Q. Which among the following compound is a white coloured precipitate? ___

P b C l_{2}, H g_{2} C l_{2}, A l (O H)_{3}, Z n S, H g S, S n S_{2}, C d S, S r C O_{3}, B a C O_{3}

View Solution

Q. An industrial waste water is found to contain

8.2 % N a_{3} P O_{4}

, and

12 % M g S O_{4}

by weight in solution. If

%

ionization of

N a_{3} P O_{4}

and

M g S O_{4}

are

50

and

60

respectively then it’s normal boiling point (in

^{o} C

) is:

[k_{b} (H_{2} O) = 0.50 {K kg mol}^{- 1}

View Solution

Which is more basic $LiOH or CsOH$ ?

View Solution

Q. calculate the vant hoff factor for a binary solute undergoing 100% dissociation

View Solution

2 mol of $S O_{2}$ and I mol of $O_{2}$ are heated in a closed vessel to reach the equilibrium:
$2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$ . The equilibrium mixture exerted a pressure of 5 atm and required $\frac{1}{3}$ mol of $K_{2} C r_{2} O_{7}$ in acidic medium. $K_{P}$ for the reaction is

1.0
none of these
2.0
0.5

View Solution

Diamine silver chloride is a __________ complex. [soluble/insoluble]

View Solution

Q. The instantanous rate of Dissaperance MnO4- ion in the following reaction is 4.56 x 10^-3 ms 2 MnO^-4 + 10 I^- + 16H^+ gives 2Mn^+2 + 5 I2 + 8H2O The rate of apperance of I2 is (a) 1.14 x 10^-3 (b) 5.7×10^-3 (c) 4.56x10^-4 (d) 1. 14x10^-2

View Solution

Q. 10 cc H2O2 solution when reacted with KI (solution) produced 0.5 g iodine. What is percentage purity of H2O2 ?

View Solution

Q. Why is the white ppt. , Al(OH)3 not soluble in (NH)4OH?
i mean ammoium ion should displace silver from its salt right??

View Solution

Q. Solubility of Ba F2 in a solution of Ba(NO3)2 will be represented by 1. [Ba+2] 2. [F-] 3. 1/2 [F-] 4. 2[NO3-]

View Solution

19.5 g

C H_{2} F C O O H

is dissolved in

500 g

of water. The depression in the freezing point of water observed is

{1.00}^{0} C

. Calculate the van't Hoff factor and dissociation constant of fluoroacetic acid.

View Solution

Q. Determine the solubility of Ag₂SO₄. Calculate molarities of individual ions and also the solubilities of salts in gL^-1.
(K_Sp = 1.4 x 10^-5)
BOOK SOLUTION
K_sp= [Ag⁺]²[SO₄^2-]
= (2S)²(S) = 2² x 1 x S³ M³ = 4S³M³
(I) S = 1.52 x 10^-2mol L^-1
MY PROBLEM
In my book in theory portion it is given a headline as ' RELATION BETWEEN K_SPAND MOLAR SOLUBILITY OF A SPARINGLY SOLUBLE SALT'
Type of Salt : M_xX_y
Relation : K_sp= x^xy^y.(S)^x+y
If we apply this rule to above problem then we will get 2²x 4⁴(S)²⁺⁴
K_sp = 1024(S)⁶See, this 'book rule' is working on every problem except this case.
NOTE: I am understanding book Solution but I want to know that when I am using the rule why it is not making correct sense.

View Solution

Q. Suppose it is required to make a buffer solution of pH = 4, using acetic acid and sodium acetate.
How many grams of sodium acetate is to be added to one litre of

\frac{N}{10}

acetic acid?

K_{a} = 1.8 \times 10^{- 5}

2.567
3.257
1.476
4.235

View Solution

Q. In which of the following, dissociation of

N H_{4} O H

will be minimised

$N a C l$
$H_{2} O$
$N a O H$
$N H_{4} C l$

View Solution