Question 1: Palette 1/64

NEET 2026 MCQ

In a qualitative analysis, $\mathrm{Bi}^{3+}$ is detected by appearance of precipitate of $\mathrm{BiO}(\mathrm{OH})(\mathrm{s})$. Calculate pH when the following equilibrium exists at 298 K .

$ \mathrm{BiO}(\mathrm{OH})(\mathrm{s}) \rightleftharpoons \mathrm{BiO}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}), \mathrm{K}=4 \times 10^{-10} $

(Given : $\log 2=0.3010$ )

A

8.714

B

4.699

C

5.286

D

9.301

Question 2: Palette 2/64

NEET 2026 MCQ

At 298 K , a certain buffer solution contains equal concentrations of $\mathrm{X}^{-}$and $\mathrm{HX}, \mathrm{K}_{\mathrm{b}}$ for $\mathrm{X}^{-}$is $10^{-10}$. What is the pH of this buffer solution?

A

2

B

4

C

6

D

10

Question 3: Palette 3/64

NEET 2026 MCQ

Phenolphthalein is used as an indicator for the titration of sodium hydroxide solution against a standard solution of oxalic acid. The colour change that is observed at an alkaline pH close to the equivalence point during this titration is:

A

pinkish red to yellow

B

yellow to pinkish red

C

pink to colourless

D

colourless to pink

Question 4: Palette 4/64

NEET 2026 MCQ

$ \text { The correct order of solubility of the given salts in water at } 298 \mathrm{~K} \text { is } $

$ \begin{array}{|l|l|} \hline \text { Salt } & \mathbf{K}_{\text {sp }} \text { at } \mathbf{2 9 8} \text { K } \\ \hline \mathrm{AgBr} & 5.0 \times 10^{-13} \\ \hline \mathrm{Zn}(\mathrm{OH})_2 & 1.0 \times 10^{-15} \\ \hline \mathrm{Hg}_2 \mathrm{Cl}_2 & 1.3 \times 10^{-18} \\ \hline \end{array} $

A

$\mathrm{Zn}(\mathrm{OH})_2>\mathrm{AgBr}>\mathrm{Hg}_2 \mathrm{Cl}_2$

B

$\mathrm{Hg}_2 \mathrm{Cl}_2>\mathrm{Zn}(\mathrm{OH})_2>\mathrm{AgBr}$

C

$\mathrm{AgBr}>\mathrm{Zn}(\mathrm{OH})_2>\mathrm{Hg}_2 \mathrm{Cl}_2$

D

$\mathrm{Hg}_2 \mathrm{Cl}_2>\mathrm{AgBr}>\mathrm{Zn}(\mathrm{OH})_2$

Question 5: Palette 5/64

NEET 2025 MCQ

If the molar conductivity $\left(\Lambda_{\mathrm{m}}\right)$ of a $0.050 \mathrm{~mol} \mathrm{~L}^{-1}$ solution of a monobasic weak acid is $90 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, its extent (degree) of dissociation will be

[Assume $\Lambda_{+}^{\circ}=349.6 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and $\Lambda_{-}^{\circ}=50.4 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$.]

A

0.225

B

0.215

C

0.115

D

0.125

Question 6: Palette 6/64

NEET 2025 MCQ

Phosphoric acid ionizes in three steps with their ionization constant values $K_{a_1}, K_{a_2}$ and $K_{a_3}$, respectively, while $K$ is the overall ionization constant. Which of the following statements are true?

A. $\quad \log \mathrm{K}=\log \mathrm{K}_{\mathrm{a}_1}+\log \mathrm{K}_{\mathrm{a}_2}+\log \mathrm{K}_{\mathrm{a}_3}$

B. $\mathrm{H}_3 \mathrm{PO}_4$ is a stronger acid than $\mathrm{H}_2 \mathrm{PO}_4^{-}$and $\mathrm{HPO}_4^{2-}$

C. $K_{a_1}>K_{a_2}>K_{a_3}$

D. $K_{a_1}=\frac{K_{a_3}+K_{a_2}}{2}$

Choose the correct answer from the options given below :

A

B, C and D only

B

A, B and C only

C

A and B only

D

A and C only

Question 7: Palette 7/64

NEET 2024 MCQ

Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?

A

Phenolphthalein, pink to yellow

B

Alkaline KMnO$_4$, colourless to pink

C

Phenolphthalein, colourless to pink

D

Methyl orange, yellow to pinkish red colour

Question 8: Palette 8/64

NEET 2024 MCQ

The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is:

(Given : Solubility product of AgCl = 10$^{–10}$)

A

10$^{-4}$

B

10$^{-6}$

C

10$^{-9}$

D

10$^{-5}$

Question 9: Palette 9/64

NEET 2023 MCQ

An acidic buffer is prepared by mixing :

A

weak acid and it's salt with strong base

B

equal volumes of equimolar solutions of weak acid and weak base

C

strong acid and it's salt with strong base

D

strong acid and it's salt with weak base (The pK$_a$ of acid = pK$_b$ of the base)

Question 10: Palette 10/64

NEET 2022 MCQ

0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :

A

1

B

3

C

2

D

4

Question 11: Palette 11/64

NEET 2022 MCQ

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pK_a of CH₃COOH = 4.57]

A

5.57

B

3.57

C

4.57

D

2.57

Question 12: Palette 12/64

NEET 2021 MCQ

The pK_b of dimethyl amine and pK_a of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethyl ammonium acetate solution is :

A

6.25

B

8.50

C

5.50

D

7.75

Question 13: Palette 13/64

NEET 2020 MCQ

Find out the solubility of Ni(OH)₂ in 0.1M NaOH. Given that the ionic product of Ni(OH)₂ is 2 $ \times $ 10^-15.

A

2 $ \times $ 10^-8 M

B

1 $ \times $ 10^-13 M

C

1 $ \times $ 10⁸ M

D

2 $ \times $ 10^-13 M

Question 14: Palette 14/64

NEET 2019 MCQ

Conjugate base for Bronsted acids H₂O and HF are :

A

OH^– and F^– , respectively

B

H₃O⁺ and H₂F⁺ , respectively

C

OH^– and H₂F⁺ , respectively

D

H₃O⁺ and F^– , respectively

Question 15: Palette 15/64

NEET 2019 MCQ

pH of a saturated solution of Ca(OH)₂ is 9. The solubility product (K_sp) of Ca(OH)₂ is :

A

0.125 × 10^–15

B

0.5 × 10^–10

C

0.5 × 10^–15

D

0.25 × 10^–10

Question 16: Palette 16/64

NEET 2019 MCQ

Which will make basic buffer?

A

100 mL of 0.1 M HCl + 200 mL of 0.1 M NH₄OH

B

100 mL of 0.1 M HCl + 100 mL of 0.1 M NHOH

C

50 mL of 0.1 M NaOH + 25 mL of 0.1 M CH₃COOH

D

100 mL of 0.1 M CH₃COOH + 100 mL of 0.1 M NaOH

Question 17: Palette 17/64

NEET 2018 MCQ

The solubility of BaSO₄ in water is 2.42 × 10^–3 g L^–1 at 298 K. The value of its solubility product (K_sp) will be (Given molar mass of BaSO₄ = 233 g mol^–1)

A

1.08 × 10^–10 mol² L^–2

B

1.08 × 10^–12 mol² L^–2

C

1.08 × 10^–14 mol² L^–2

D

1.08 × 10^–8 mol² L^–2

Question 18: Palette 18/64

NEET 2018 MCQ

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :

A. 60 mL ${M \over {10}}$ HCl + 40 mL ${M \over {10}}$ NaOH

B. 55 mL ${M \over {10}}$ HCl + 45 mL ${M \over {10}}$ NaOH

C. 75 mL ${M \over {5}}$ HCl + 25 mL ${M \over {5}}$ NaOH

D. 100 mL ${M \over {10}}$ HCl + 100 mL ${M \over {10}}$ NaOH

pH of which one of them will be equal to 1?

A

B

B

A

C

D

D

C

Question 19: Palette 19/64

NEET 2017 MCQ

Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 $ \times $ 10^$-$4 mol L^$-$1. Solubility product of Ag₂C₂O₄ is

A

2.66 $ \times $ 10^$-$12

B

4.5 $ \times $ 10^$-$11

C

5.3 $ \times $ 10^$-$12

D

2.42 $ \times $ 10^$-$8

Question 20: Palette 20/64

NEET 2016 MCQ

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

A

BF₃

B

PF₃

C

CF₄

D

SiF₄

Question 21: Palette 21/64

NEET 2016 MCQ

The solubility of AgCl_(s) with solubility product 1.6 $ \times $ 10^$-$10 in 0.1 M NaCl solution would be

A

1.26 $ \times $ 10^$-$5 M

B

1.6 $ \times $ 10^$-$9 M

C

1.6 $ \times $ 10^$-$11 M

D

zero

Question 22: Palette 22/64

NEET 2016 MCQ

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N⁺H) ina 0.10 M aqueous pyridine solution (K_b for C₅H₅N = 1.7 $ \times $ 10^$-$9) is

A

0.0060%

B

0.013%

C

0.77%

D

1.6%

Question 23: Palette 23/64

NEET 2016 MCQ

MY and NY₃, two nearly insoluble salts, have the same K_sp values of 6.2 $ \times $ 10^$-$13 at room temperature. Which statement would be true in regard to MY and NY₃?

A

The salts MY and NY₃ are more soluble in 0.5 M KY than in pure water.

B

The addition of the salt of KY to solution of MY and NY₃ will have no effect on their solubilities.

C

The molar solubilities of MY and NY₃ in water are identical.

D

The molar solubility of MY in water is less than that of NY₃.

Question 24: Palette 24/64

NEET 2015 MCQ

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

A

2.0

B

7.0

C

1.04

D

12.65

Question 25: Palette 25/64

NEET 2015 MCQ

Which one of the following pairs of solution is not an acidic buffer ?

A

CH₃COOH and CH₃COONa

B

H₂CO₃ and Na₂CO₃

C

H₃PO₄ and Na₃PO₄

D

HClO₄ and NaClO₄

Question 26: Palette 26/64

NEET 2015 MCQ

The K_sp of Ag₂CrO₄,  AgCl,  AgBr  and Agl  are respectively, 1.1 $ \times $ 10^$-$12, 1.8 $ \times $ 10^$-$10, 5.0 $ \times $ 10^$-$13, 8.3 $ \times $ 10^$-$17. Which one of the following salts will precipitate last if AgNO₃ solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na₂CrO₄?

A

AgBr

B

Ag₂CrO₄

C

Agl

D

AgCl

Question 27: Palette 27/64

NEET 2014 MCQ

Which of the following salts will give highest pH in water?

A

KCl

B

NaCl

C

Na₂CO₃

D

CuSO₄

Question 28: Palette 28/64

NEET 2013 MCQ

The dissociation constant of weak acid is 1 $ \times $ 10^$-$4. In order to prepare a buffer solution with a pH = 5, the [Salt]/[Acid] ratio should be

A

4 : 5

B

10 : 1

C

5 : 4

D

1 : 10

Question 29: Palette 29/64

NEET 2013 MCQ

At 100^oC the K_w of water is 55 times its value at 25^oC. What will be the pH of neutral solution? (log 55 = 1.74)

A

7.00

B

7.87

C

5.13

D

6.13

Question 30: Palette 30/64

NEET 2013 MCQ

The values of K_sp of CaCO₃ and CaC₂O₄ are 4.7 $ \times $ 10^$-$9 and 1.3 $ \times $ $-$9 respectively at 25^oC. If the mixture of these two is washed with water, what is the concentration of Ca²⁺ ions in water ?

A

5.831 $ \times $ 10^$-$5 M

B

6.856 $ \times $ 10^$-$5 M

C

3.606 $ \times $ 10^$-$5 M

D

7.746 $ \times $ 10^$-$5 M

Question 31: Palette 31/64

NEET 2013 MCQ

Accumulation of lactic acid (HC₃H₅O₃), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociates. The value of dissociation constant, K_a, for this acid will be

A

1.4 $ \times $ 10^$-$5

B

1.4 $ \times $ 10^$-$4

C

3.7 $ \times $ 10^$-$4

D

2.8 $ \times $ 10^$-$4

Question 32: Palette 32/64

NEET 2013 MCQ

KMnO₄ can be prepared from K₂MnO₄ as per the reaction,

3MnO₄^2$-$ + 2H₂O $\rightleftharpoons$ 2MnO₄^$-$ + MnO² + 4OH^$-$

The reaction can go to completion by removing OH^$-$ ions by adding

A

CO₂

B

SO₂

C

HCl

D

KOH

Question 33: Palette 33/64

NEET 2013 MCQ

Which of these is least likely to act as a lewis base ?

A

BF₃

B

PF₃

C

CO

D

F^$-$

Question 34: Palette 34/64

NEET 2012 MCQ

Buffer solutions have constant acidity and alkalinity because

A

these give unionised acid or base on reaction with added acid or alkali

B

acids and alkalies in these solutions are shielded from attack by other ions

C

they have large excess of H⁺ or OH^$-$ ions

D

they have fixed value of pH

Question 35: Palette 35/64

NEET 2012 MCQ

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value ?

A

BaCl₂

B

AlCl₃

C

LiCl

D

BeCl₂

Question 36: Palette 36/64

NEET 2012 MCQ

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product (K_sp) of Ba(OH)₂ is

A

3.3 $ \times $ 10^$-$7

B

5.0 $ \times $ 10^$-$7

C

4.0 $ \times $ 10^$-$6

D

5.0$ \times $ 10^$-$6

Question 37: Palette 37/64

NEET 2011 MCQ

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag⁺ and pb²⁺ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl^$-$ concentration is 0.10 M. What will the concentrations of Ag⁺ and Pb²⁺ be at equilibrium ?

(K_sp for AgCl = 1.8 $ \times $ 10^$-$10, K_sp for PbCl₂ = 1.7 $ \times $ 10^$-$5)

A

[Ag⁺] = 1.8 $ \times $ 10^$-$7 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$6 M

B

[Ag⁺] = 1.8 $ \times $ 10^$-$11 M, [Pb²⁺] = 8.5 $ \times $ 10^$-$5 M

C

[Ag⁺] = 1.8 $ \times $ 10^$-$9 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$3 M

D

[Ag⁺] = 1.8 $ \times $ 10^$-$11 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$4 M

Question 38: Palette 38/64

NEET 2011 MCQ

Which of the following is least likely to behave as Lewis base?

A

H₂O

B

NH₃

C

BF₃

D

OH^$-$

Question 39: Palette 39/64

NEET 2011 MCQ

A buffer solution is prepared in which the concentration of NH₃ is 0.30 M and the concentration of NH⁺₄ is 0.20 M. If the equilibrium constant, K_b for NH₃ equals 1.8 $ \times $ 10^$-$5, what is the pH of this solution? (log 2.7 = 0.43)

A

9.08

B

9.43

C

11.72

D

8.73

Question 40: Palette 40/64

NEET 2010 MCQ

What is [H⁺] in mol/L of a solution that is 0.20 M in CH₃COONa and 0.10 M in CH₃COOH? K_a for CH₃COOH = 1.8 $ \times $ 10^$-$5

A

3.5 $ \times $ 10^$-$4

B

1.1 $ \times $ 10^$-$5

C

1.8 $ \times $ 10^$-$5

D

9.0 $ \times $ 10^$-$6

Question 41: Palette 41/64

NEET 2010 MCQ

If pH of a saturated solution of Ba(OH)₂ is 12, the value of its K_sp is

A

4.00 $ \times $ 10^$-$6 M³

B

4.00 $ \times $ 10^$-$7 M³

C

5.00 $ \times $ 10^$-$6 M³

D

5.00$ \times $ 10^$-$7 M³

Question 42: Palette 42/64

NEET 2010 MCQ

In a buffer solution containing equal concentration of B^$-$ and HB, the K_b for B^$-$ is 10^$-$10. The pH of buffer solution is

A

10

B

7

C

6

D

4

Question 43: Palette 43/64

NEET 2009 MCQ

Which of the following molecules acts as a Lewis acid?

A

(CH₃)₂O

B

(CH₃)₃P

C

(CH₃)₃N

D

(CH₃)₃B

Question 44: Palette 44/64

NEET 2009 MCQ

The ionization constant of ammonium hydroxide is 1.77 $ \times $ 10^$-$5 at 298 K. Hydrolysis constant of ammonium chloride is

A

6.50 $ \times $ 10^$-$12

B

5.65 $ \times $ 10^$-$13

C

5.65 $ \times $ 10^$-$12

D

5.65 $ \times $ 10^$-$10

Question 45: Palette 45/64

NEET 2009 MCQ

What is the [OH^$-$] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)₂?

A

0.40 M

B

0.0050 M

C

0.12 M

D

0.10 M

Question 46: Palette 46/64

NEET 2008 MCQ

Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture?

A

3.7 $ \times $ 10^$-$3 M

B

1.11 $ \times $ 10^$-$3 M

C

1.11 $ \times $ 10^$-$4 M

D

3.7 $ \times $ 10^$-$4 M

Question 47: Palette 47/64

NEET 2007 MCQ

A weak acid, HA, has a K_a of 1.00 $ \times $ 10^$-$5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to

A

1.00%

B

99.9%

C

0.100%

D

99.0%

Question 48: Palette 48/64

NEET 2007 MCQ

Calculate the pOH of a solution at 25^oC that contains 1 $ \times $ 10^$-$10 M of hydronium ions, i.e. H₃O⁺.

A

4.000

B

9.000

C

1.000

D

7.000

Question 49: Palette 49/64

NEET 2006 MCQ

The hydrogen ion concentration of a 10^$-$8 M, HCl aqueous solution at 298 K (K_w = 10^$-$14) is

A

1.0 $ \times $ 10^$-$8 M

B

1.0 $ \times $ 10^$-$6 M

C

1.0525 $ \times $ 10^$-$7 M

D

9.525 $ \times $ 10^$-$8 M

Question 50: Palette 50/64

NEET 2006 MCQ

Which of the following pairs constitutes a buffer?

A

HCl and KCl

B

HNO₂ and NaNO₂

C

NaOH and NaCl

D

HNO₃ and NH₄NO₃

Question 51: Palette 51/64

NEET 2005 MCQ

H₂S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because

A

presence of HCl decreases the sulphide ion concentration

B

solubility product of group II sulphides is more than that of group IV sulphates

C

presence of HCl increases the sulphide ion concentration

D

sulphides of group IV cations are unstable in HCl.

Question 52: Palette 52/64

NEET 2005 MCQ

At 25^oC, the dissociation constant of a base, BOH, is 1.0 $ \times $ 10^$-$12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

A

1.0 $ \times $ 10^$-$5 mol L^$-$1

B

1.0 $ \times $ 10^$-$6 mol L^$-$1

C

2.0 $ \times $ 10^$-$6 mol L^$-$1

D

1.0 $ \times $ 10^$-$7 mol L^$-$1

Question 53: Palette 53/64

NEET 2004 MCQ

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In^$-$) forms of the indicator by the expression

A

$\log {{\left[ {I{n^ - }} \right]} \over {\left[ {HIn} \right]}} = p{K_{In}} - pH$

B

$\log {{\left[ {HIn} \right]} \over {\left[ {I{n^ - }} \right]}} = p{K_{In}} - pH$

C

$\log {{\left[ {HIn} \right]} \over {\left[ {I{n^ - }} \right]}} = pH - p{K_{In}}$

D

$\log {{\left[ {I{n^ - }} \right]} \over {\left[ {HIn} \right]}} = pH - p{K_{In}}$

Question 54: Palette 54/64

NEET 2004 MCQ

The solubility product of a sparingly soluble salt AX₂ is 3.2 $ \times $ 10^$-$11. Its solubility (in moles/L) is

A

5.6 $ \times $ 10^$-$6

B

3.1 $ \times $ 10^$-$4

C

2 $ \times $ 10^$-$4

D

4 $ \times $ 10^$-$4

Question 55: Palette 55/64

NEET 2003 MCQ

The solubility product of AgI at 25^oC is 1.0 $ \times $ 10^$-$16 mol² L^$-$2. The solubility of AgI in 10^$-$4 N solution of KI at 25^oC is approximately (in mol L^$-$1

A

1.0 $ \times $ 10^$-$16

B

1.0 $ \times $ 10^$-$12

C

1.0 $ \times $ 10^$-$10

D

1.0 $ \times $ 10^$-$8

Question 56: Palette 56/64

NEET 2002 MCQ

Solution of 0.1 N NH₄OH and 0.1 N NH₄Cl has pH 9.25. Then find out pK_b of NH₄OH

A

9.25

B

4.75

C

3.75

D

8.25

Question 57: Palette 57/64

NEET 2002 MCQ

Solubility of MX₂ type electrolytes is 0.5 $ \times $ 10^$-$4 mole/lit., then find out K_sp of electrolytes.

A

5 $ \times $ 10^$-$12

B

25 $ \times $ 10^$-$10

C

1 $ \times $ 10^$-$13

D

5 $ \times $ 10^$-$13

Question 58: Palette 58/64

NEET 2002 MCQ

Which has highest pH?

A

CH₃COOK

B

Na₂CO₃

C

NH₄Cl

D

NaNO₃

Question 59: Palette 59/64

NEET 2001 MCQ

Solubility of M₂S salt is 3.5 $ \times $ 10^$-$6 then find out solubility product.

A

1.7 $ \times $ 10^$-$6

B

1.7 $ \times $ 10^$-$16

C

1.7 $ \times $ 10^$-$18

D

1.7 $ \times $ 10^$-$12

Question 60: Palette 60/64

NEET 2001 MCQ

In HS^$-$, I^$-$, R $-$ NH₂, NH₃ order of proton accepting tendency will be

A

I^$-$ > NH₃ > R $-$ NH₂ > HS^$-$

B

NH₃ > R $-$ NH₂ > HS^$-$ > I^$-$

C

R $-$ NH₂ > NH₃ > HS^$-$ > I^$-$

D

HS^$-$ > R $-$ NH₂ > NH₃ > I^$-$

Question 61: Palette 61/64

NEET 2001 MCQ

Ionisation constant of CH₃COOH is 1.7 $ \times $ 10^$-$5 and concentration of H⁺ ions is 3.4 $ \times $ 10^$-$4. Then find out initial concentration of CH₃COOH molecules.

A

3.4 $ \times $ 10^$-$4

B

3.4 $ \times $ 10^$-$3

C

6.8 $ \times $ 10^$-$4

D

6.8 $ \times $ 10^$-$3

Question 62: Palette 62/64

NEET 2001 MCQ

Correct relation between dissociation constants of a dibasic acid is

A

K_a1 = K_a2

B

K_a1 > K_a2

C

K_a1 < K_a2

D

K_a1 = ${1 \over {{K_{{a_2}}}}}$

Question 63: Palette 63/64

NEET 2000 MCQ

Conjugate acid of NH₂^$-$ is

A

NH₄OH

B

NH₄⁺

C

NH₂^$-$

D

NH₃

Question 64: Palette 64/64

NEET 2000 MCQ

Which statement is wrong about pH and H⁺?

A

pH of neutral water is not zero.

B

Adding 1 N solution of CH₃COOH and 1 N solution of NaOH, pH will be seven.

C

[H⁺] of dilute and hot H₂SO₄ is more than concentrated and cold H₂SO₄

D

Mixing solution of CH₃COOH and HCl. pH will be less than 7.