pH the Power of H

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

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

Q.

Turmeric is a natural indicator that turns

1. Yellow in acid and pinkish-red in base

2. Blue in base and red in acid

3. Yellow in base and pinkish-red in acid

4. Blue in acid and red in base

Q. What will be the resultant pH when 200 mL of an aqueous solution of HCl (pH = 2) is mixed with 300 mL of an aqueous solution of NaOH (pH = 12)?

1. 7.8
2. 11.3
3. 5.5
4. 2.7

Q.

The concentration of hydrogen ion in a sample of soft drink is $3.8\times {10}^{–3}M$. what is its pH?

Q.

What is the role of indicators in titration?

Q. The following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations
1. 60 mL $\frac{M}{10}$ HCl + 40 mL $\frac{M}{10}$ NaOH

2. 55 mL $\frac{M}{10}$ HCl + 45 mL $\frac{M}{10}$ NaOH

3. 75 mL $\frac{M}{5}$ HCl + 25 mL $\frac{M}{5}$ NaOH

4. 100 mL $\frac{M}{10}$ HCl + 100 mL $\frac{M}{10}$ NaOH

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

1. 1
2. 2
3. 3
4. 4

Q. Calculate the ph of 0.05m h2so4 solution

Q. The dissociation constant of $0.01MC{H}_{3}COOH$ is $1.8\times {10}^{-5}$ then calculate $C{H}_{3}CO{O}^{-}$ concentration in 0.1 M $HCl$ solution.

1. $1.8\times {10}^{-6}mol{L}^{-1}$
2. $1.8\times {10}^{-8}mol{L}^{-1}$
3. $3.8\times {10}^{-6}mol{L}^{-1}$
4. $3.8\times {10}^{-8}mol{L}^{-1}$

Q.

The pH of milk, black coffee, tomato juice, lemon juice and egg white are 6.8, 5.0, 4.2, 2.2 and 7.8 respectively. Calculate corresponding hydrogen ion concentration in each.

Q.

Acids turn blue litmus to ______.

Q.

pH of 0.005M Ca(OH)₂ solution is

Q.

Ionic product of water at 310 K is $2.7\times {10}^{-14}$. What is the pH of neutral water at this temperature?

Q. What is the concentration of $O_2$ in a fresh water stream in equilibrium with air at ${25}^{o}C$ and $1.0bar$ ?
Given that , at $1bar$ oxygen in air is $21\%\text{by volume}$
$K_H^{\prime }$ (Henry's law constant) for $O_2=1.3\times {10}^{-3}mol/kgbar$ at ${25}^{o}C.$

1. $8.736\times {10}^{-3}g/kg$
2. $4.16\times {10}^{-2}g/kg$
3. $24.04g/kg$
4. $114.5g/kg$

Q. Calculate the pH of a solution formed by mixing equal volume of two solutions A and B of a strong acid having $pH=6$ and $pH=4$ respectively ?
(Given: log 5.05 = 0.703)

1. 4.29
2. 5
3. 5.29
4. None of the above

Q. How many litres of water must be added to 1 L of an aqueous solution of $HCl$ with a pH of 1 to create an aqueous solution with pH of 2?

1. 0.1 L
2. 2.0 L
3. 9.0 L
4. 0.9 L

Q.

The first ionization constant of H2S is $9.1\times {10}^{-8}$. Calculate the concentration of $H{S}^{-}$ ion in its 0.1 M solution. How will this concentration be affected if the solution is 0.1 M in HCl also?
If the second dissociation constant of $H_{2}S$ is $1.2\times {10}^{-13}$, calculate the concentration of $S^{2–}$ under both conditions.

Q.

The ionization constant of acetic acid is $1.74\times {10}^{-5}$. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

Q.

When white phosphorus is boiled with alkali in an inert atmosphere and forms product ‘A’.When $1\mathrm{mol}$ A with an excess of ${\mathrm{AgNO}}_3$ in aqueous medium gives _______mol(s) of $\mathrm{Ag}$(Round to the nearest integer).

Q.

Reduction in pH of blood will

1. release bicarbonate ions by the liver

2. decrease the affinity of haemoglobin with oxygen

3. reduce the blood supply to the brain

4. reduce the rate of heartbeat

Q.

Assuming complete dissociation, calculate the pH of the following solutions:

(i) 0.003 M HCl

(ii) 0.005 M NaOH

(iii) 0.002 M HBr

(iv) 0.002 M KOH

Q. 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?

1. $3.7\times {10}^{-3}M$
2. $1.11\times {10}^{-3}M$
   
3. $1.11\times {10}^{-4}M$
4. $3.7\times {10}^{-4}M$

Q.

Calculate the pH of the resultant mixtures:

10 mL of 0.2M $Ca(OH{)}_2$ + 25 mL of 0.1M HCl

10 mL of 0.01M $H_{2}S{O}_4$ + 10 mL of 0.01M $Ca(OH{)}_2$

10 mL of 0.1M $H_{2}S{O}_4$ + 10 mL of 0.1M KOH

Q. Assertion (A): pH of pure water increases with increase in temperature. Reason (R): Self ionization of water is an endothermic reaction. Which of the following is correct?

1. Both A & R are correct but R is not a correct explanation of A.
2. A is true but R is false
3. Both A & R are correct and R is correct explanation of A.
4. A is false but R is true.

Q.

pK_a of a weak acid (HA) and pK_b of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

1. 7.0

2. 1.0

3. 7.2

4. 6.9

Q. The pH of solution is 6.0 . To this solution, sufficient acid is added to decrease the pH to 2.0. The increase in hydrogen ion concentration is:

1. ${10}^{0.5}$ times.
2. ${10}^2$ times.
3. ${10}^6$ times.
4. ${10}^4$ times.

Q.

Is ${\mathrm{Na}}_2{\mathrm{CO}}_3$ it basic salt?

Q.

Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
(a)Human muscle-fluid, 6.83
(b)Human stomach fluid, 1.2
(c) Human blood, 7.38
(d)Human saliva, 6.4.

Q. Determine the $pH$ of a solution that is 0.03 M $HCl$.

1. 4.88
2. 2.88
3. 4.52
4. 1.52

Q.

The $K_{sp}$ of $\mathrm{Mg}{\left(\mathrm{OH}\right)}_2$ is $1\times {10}^{-12}$. $0.01\mathrm{M}\mathrm{Mg}{\left(\mathrm{OH}\right)}_2$ will precipitate at the limiting pH equal to________

Q.

The ionization constant of HF, HCOOH and HCN at 298K are $6.8\times {10}^{–4},1.8\times {10}^{–4}$ and $4.8\times {10}^{–9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.