pH the Power of H

Q. The $pH$ of ${10}^{-3}M{H}_{2}S{O}_4$ is :

1. 3
2. 11.7
3. 2.69
4. None of the above

Q.

A certain weak acid has $Ka=1.0\times {10}^{-4}$. Calculate the equilibrium constant for its reaction with a strong Base.

1. 

2. 

3. 

4. 

Q.

The pH of $0.1\text{M}$ $\mathrm{NaOH}$ is

1. $10$

2. $11$

3. $12$

4. $13$

Q.

Which of the following process energy is liberated -

1. Cl = Cl+ + e-

2. HCl =H+ + Cl-

3. Cl + e-=Cl-

4. O- + e- =O-2

Q. What is the pH of 0.02 M Sodium Hydroxide solution?

1. 2
2. 12
3. 1.7
4. 12.3

Q.

Balanced ionic equation for the reaction of Potassium Dichromate (VI) K₂Cr₂O₇ with Sodium Sulphite Na₂SO₃ in acid solution to give Chromium (III) ion and sulphate ion is

1. Cr₂O₇^-2_(aq) + 3SO₃^2-_(aq) + 8H⁺_(aq) → 2Cr³⁺_(aq) + 5SO₄^2-_(aq) + 4H₂O_(liq)

2. Cr₂O₇^-2_(aq) + 3SO₃^2-_(aq) + 8H⁺_(aq) → 2Cr³⁺_(aq) + 3SO₄^2-_(aq) + 4H₂O_(liq)

3. Cr₂O₇^-2_(aq) + 3SO₃^2-_(aq) + 5H⁺_(aq) → 2Cr³⁺_(aq) + 3SO₄^2-_(aq) + 4H₂O_(liq)

4. Cr₂O₇^-2_(aq) + 2SO₃^2-_(aq) + 8H⁺_(aq) → 2Cr³⁺_(aq) + 3SO₄^2-_(aq) + 4H₂O_(liq)

Q.

Gastric juice contains 3.0g of $HCl$ per litre. If a person produces 2.5 litre of gastric juice per day. How many antacid tablets each containing 400 mg of $Al$($OH{)}_3$ are needed to neutralize all the $HCl$ produced in one day ?

1. 18

2. 14

3. 17

4. 20

Q. At a certain temperature for a aqueous solution, the value of $p{K}_w$ is 13.4 and the measured pH of the solution is 7. What is the nature of the solution?

1. Acidic
2. Basic
3. Neutral
4. Unpredictable

Q. The $pOH$ of ${10}^{-8}MHCl$ is :

1. 8
2. 6
3. between 6 and 7
4. between 7 and 8

Q. The $K_w$ for water for the equillibrium, $2H_{2}O\rightleftharpoons H_3{O}^{+}O{H}^{-}$ changes from ${10}^{-14}$ at $25{}^{\circ }\text{C}$ to $9.62\times {10}^{-14}$ at $60{}^{\circ }\text{C}$.
Calculate the $pH$ and nature at $60{}^{\circ }\text{C}$

1. $pH=5.51$, solution is basic
2. $pH=6.51$, solution is neutral
3. $pH=5.51$, solution is acidic
4. $pH=6.51$, solution is basic

Q. Which of the following is the weakest acid? ($p{K}_a$ values given at ${25}^{o}C$)

1. $H_{2}S:p{K}_a=7.0$
2. $HF:p{K}_{a}3.2$
3. $H{N}_3:p{K}_a=4.7$
4. $HCN:p{K}_a=9.2$

Q.

At ${25}^{\circ }C$, the ionization constants of $C{H}_{3}COOH$ and $N{H}_3$ are almost equal. The pH of a solution of $0.01MC{H}_{3}COOH$ is 4.0 at ${25}^{\circ }C$. The pOH of 0.01 $MN{H}_{4}OH$ at the same temperature will be :

1. 3.0

2. 4.0

3. 10.0

4. 10.5

Q. Acetic acid is the principal ingredient in vinegar that's why it tastes sour. At equilibrium. a solution contains $\left[C{H}_{3}C{O}_{2}H\right]=0.0787M$ and $\left[H_3{O}^{+}\right]=\left[C{H}_{3}C{O}_2^{-}\right]=0.00118M.$ what is the values of $K_a$ for acetic acid?

1. $1.77\times {10}^{-5}$
2. $2.55\times {10}^{-6}$
3. $2.77\times {10}^{-5}$
4. $2.77\times {10}^{-7}$

Q. An indicator has $p{K}_{in}=\mathrm{5.3.}$ In a certain solution, this indicator is found to be $20\%$ ionised. Calculate the pH of the solution?

1. $1.6$
2. $6$
3. $5.3$
4. $4.7$

Q.

For two acids A and B, $p{K}_a$ = $1.2$, $p{K}_b$ = $2.8$ respectively in value, then which of the following

is true

1. A and B both are equally acidic

2. A is stronger than B

3. B is stronger than A

4. Neither A nor B is strong

5. None of the options are correct.

Q. Calculate the $pH$ at which an acid indicator $\left(HIn\right)$ having $K_{In}={10}^{-5}$ changes its colour.
Given, the $HIn$ concentration is ${10}^{-3}M$.

1. $2$
2. $3$
3. $5$
4. $8$

Q. The pH value of $0.001M$ aqueous solution of NaCl is:

1. 7
2. 4
3. 11
4. unpredictable

Q. A certain indicator (an organic dye) has $p{K}_a=5$ for which of the following titrations may it be suitable.

1. Acetic acid against NaOH
2. Aniline hydrochloride against NaOH
3. Sodium carbonate against HCl
4. Barium hydroxide against oxalic acid

Q. Equilibrium constant of $T_{2}O$ (T or ${}_1^{3}H$ is an isotope of ${}_1^{1}H$) and $H_{2}O$ are different at 298 K. At 298 K, pure $T_{2}O$ has pT (like pH) of 7.62. The pT of a solution prepared by adding 10 mL of 0.2 M $TCl$ to 15 mL of 0.25 M $NaOT$ is:

1. $2-log7$
2. $14+log7$
3. $13.24-log7$
4. $13.24+log7$

Q. Choose the correct statement regarding Methyl Orange indicator:

1. Colour transition range for Methyl Orange is nearly $(3.2-4.4)$
2. Colour transition range for Methyl Orange is nearly $(6-8.6)$
3. Colour transition range for Methyl Orange is nearly $(8.3-10)$
4. Colour transition range for Methyl Orange is nearly $(6.2-7.4)$

Q.

A list of solutions is given below:

Aqueous solution of sodium chloride, acetic acid, lemon juice and an aqueous solution of ammonia.

Select a solution having pH equal to 7.

Q. Cu+HNO3 -> Cu(NO3)2 +NO2+ H2O Balance the given rection using ion electron method.

Q. 100 ml of 3 mol H2SO4 reacts with 100 ml of 2 NaOH. Enthalpy of neutralisation of reaction is- (1) - 57.1 kJ/mol (2) - 2 * 57.1 kJ/mol (3) - 0.3 * 57.1 kJ/mol (4) - 3 * 57.1 kj/mol (Explain with concept of n-factor and equivalent weight)

Q.

The pH of blood is 7.4. If the buffer in bloods is $C{O}_{2}andHC{O}_3^{-}$, calculate the ratio of conjugate base to acid $\left(H_{2}C{O}_3\right)$ to maintain the pH of the blood. Given $K_1$ of $H_{2}C{O}_3=4.5\times {10}^{-7}$

1. 8.5

2. 10.0

3. 11.25

4. None of these

Q.

Aqueous solution of $HCl$ has the pH = 4. Its molarity would be

1. 4 M

2. 0.4 M

3. 0.0001 M

4. 10 M

Q. Consider a weak monobasic acid $HA$ having a concentration C with degree of dissociation, $\alpha <<1.$. The pH of this weak acid in terms of acid dissociation constant $K_a$ and concentration $C$ is :

1. $-lo{g}_{10}\left(\sqrt{\frac{K_a}{C}}\right)$
2. $-lo{g}_{10}\sqrt{K_a.C}$
3. $pH=-lo{g}_{10}\sqrt{K_a.C^2}$
4. $pH=-lo{g}_{10}\sqrt{K_a^2.C}$

Q. Assumed $Ca(OH{)}_2$ to be completely ionized the $pH$ of 0.01 M molar aqueous solution of calcium hydroxide is approximately:

1. 10.5
2. 11.8
3. 13.7
4. 12.3

Q. Buffer capacity of acid buffer solution is more when
A) $P^{Ka}=p^H$
B) $\left[Salt\right]=\left[Acid\right]$
C) $P^{Ka}=7$
D) $[H+]$ = $P^{Ka}$

1. All are correct
2. A and B are correct
3. C and B are correct
4. B, C and D are correct

Q.

At ${90}^{\circ }$C pure water has [${H_{3}O}^{+}$] = ${10}^{-6}$mol ${litre}^{-1}$. The value of $K_W$ at ${90}^{\circ }$C is

1. ${10}^{-6}$

2. ${10}^{-12}$

3. ${10}^{-14}$

4. ${10}^{-8}$

Q. Calculate the $pH$ at which a basic indicator $\left(InOH\right)$ with $K_{In}=1\times {10}^{-10}$ changes its colour.
Given : The concentration of indicator is $1\times {10}^{-2}M$.

1. 8
2. 4
3. 2
4. 10