Salt of Strong Acid and Strong Bases

Q. $100\text{mL}$ of a $0.1\text{M}NaCl$ solution is added to $300\text{mL}$ of a $0.2\text{M}$ $MgC{l}_2$ solution. $100\text{mL}$ of this solution was further diluted with $400\text{mL}$ of water. The molarity of $C{l}^{-}$ ions in the resultant solution is:

1. $0.725\text{M}$
2. $0.055\text{M}$
3. $0.045\text{M}$
4. $0.065\text{M}$

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

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

Q. What will be the normality of a solution obtained by mixing $0.45\text{N}$ and $0.60\text{N}$ $NaOH$ in the ratio $2:1$ by volume?

1. $0.4\text{N}$
2. $0.5\text{N}$
3. $1.05\text{N}$
4. $0.15\text{N}$

Q. What is the $pH$ of a solution in which $25\text{mL}$ of $0.1\text{M}NaOH$ is added to $25\text{mL}$ of $0.08\text{M}HCl$ and final solution is diluted to $500\text{mL}?$

1. $3$
2. $11$
3. $12$
4. $13$

Q. $100mL$ of $0.1MHCl$ is titrated against the $0.1MNaOH$ solution. What will be the $pH$ of the solution when $100mLNaOH$ is added ?

1. 7
2. 1.3
3. 1
4. 2

Q. $50mL$ of $0.2MHCl$ is titrated against the $0.1MNaOH$ solution. What will be the $pH$ of the solution when $20mLNaOH$ is added ?

1. 4.2
2. 1.25
3. 2.69
4. 0.95

Q. The pH of an aqueous solution containing $0.025M{H}_{2}S{O}_4$ and $0.005MHCl$ is:
${\log }_{10}\left(5.5\right)=0.74$

1. 0.74
2. 1.26
3. 0.26
4. 1.74

Q. $100\text{mL}$ of $0.1\text{M NaOH}$ solution is titrated with $100\text{mL}$ of $0.05\text{M}{H}_{2}S{O}_4$ solution. The $pH$ of the resulting solution is : $(\text{for}{H}_{2}S{O}_4,K{a}_1=\infty ,K{a}_2={10}^{-2})$

1. 7.2
2. 7.4
3. 6.8
4. 7

Q.

Which of these salts will have highest value of ph in water and why

Kcl

Nacl

Na2Co3

Cuso4

Q. In what volume ratio NH4Cl and NH4OH having 1M concentration should be mixed to get a buffer solution of pH=9.26 (pK_b of NH4OH = 4.74?

Q. What will be the $H^{+}$ ion concentration of a solution prepared by mixing 50 mL of 0.20 M $NaCl$, 25 mL of 0.10 M $NaOH$ and 25 mL of 0.30 M $HCl$?

1. 0.5 M
2. 0.05 M
3. 0.02 M
4. 0.10 M

Q.

Calculate the pH of the following solutions:

a) 2 g of TlOH dissolved in water to give 2 litre of solution.

b) 0.3 g of Ca(OH)₂ dissolved in water to give 500 mL of solution.

c) 0.3 g of NaOH dissolved in water to give 200 mL of solution.

d) 1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.

Q. What is the molality of a dilute aqueous 0.02N $H_{3}P{O}_4$ solution?

1. 0.0050
2. 0.0200
3. 0.00330
4. 0.0067

Q. Which of the following solutions will have pH equal to 1.0?

1. 55 mL of $\frac{M}{10}$ HCl + 45 mL of $\frac{M}{10}$ NaOH
   
2. 50 mL of $\frac{M}{5}$ HCl + 50 mL of $\frac{M}{5}$ NaOH
   
3. 75 mL of $\frac{M}{5}$ HCl + 25 mL of $\frac{M}{5}$ NaOH
   
4. None of the above

Q. 25 mL of a 2 N $HCl$ solution , 50 mL of a 4 N $HN{O}_3$ solution and $x$ mL of a 5 M $H_{2}S{O}_4$ solution are mixed together and the total volume is made upto 1 litre with water. 50 mL of this acid mixture exactly neutralizes 25 mL of a 1 N $N{a}_{2}C{O}_3$ solution. The value of $x$ is:

1. 25 mL
2. 40 mL
3. 60 mL
4. 50 mL

Q. A solution of $NaCl$ is .

1. acidic
2. alkaline
3. neutral

Q. $0.56$ litre each of three samples of $H_2{O}_2$ labelled as $10vol,15vol$ and $20vol$ are mixed. The resultant normality of $H_2{O}_2$ solution is:

1. $1.68\text{N}$
2. $2.68\text{N}$
3. $4.5\text{N}$
4. $8.0\text{N}$

Q. How many g moles of HCl will be required to prepare one litre of buffer solution (containing NaCN and HCN) of pH= 8.5 using 0.01 gm formula mass of NaCN. $K_a\left(HCN\right)=4.1\times {10}^{–10}$

1. 0.0089 mole
2. 0.0081 mole
3. 0.0082 mole
4. 0.0080 mole

Q. Find the pH of an aqueous solution formed on mixing equal volumes of $0.05M{H}_{2}S{O}_4$ and $0.1MHCl$ solution.

1. 1
2. 0.5
3. 1.5
4. 0.25

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

$a.60mL\frac{M}{10}HCl+40mL\frac{M}{10}NaOH$
$b.55mL\frac{M}{10}HCl+45mL\frac{M}{10}NaOH$
$c.75mL\frac{M}{5}HCl+25mL\frac{M}{5}NaOH$
$d.100mL\frac{M}{10}HCl+100mL\frac{M}{10}NaOH$

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

1. d
2. b
3. c
4. a

Q. Find the weight of $NaN{O}_3$ in grams (Rounded off to nearest integer), required to make 50 mL of an aqueous solution containing 70 mg per mL of $N{a}^{+}$ ions

[Given:Atomic weight in $gmo{l}^{-1}[Na:23;N:14;O:16]$

Q. Which of the following is best scientific method to test presence of water in a liquid?

1. Taste
2. Smell
3. Use of litmus paper
4. Use of anhydrous copper sulfate

Q. Classify $Na{H}_{2}P{O}_2$ and $NaHS{O}_4$ salts as acid salt or normal salt.

Q. The molarity of $C{l}^{-}$ ion in a 100 mL aqueous solution which has 2 % $\left(\frac{w}{v}\right)NaCl$, 4 % $\left(\frac{w}{v}\right)CaC{l}_2$ and 6 % $\left(\frac{w}{v}\right)N{H}_{4}Cl$ will be:

1. 0.342 M
2. 0.721 M
3. 1.121 M
4. 2.181 M

Q. The $K_w$ for $2H_{2}O\rightleftharpoons H_3{O}^{+}+O{H}^{-}$ changes from ${10}^{-14}$ at ${25}^{o}C$ to $9.62\times {10}^{-14}$ at ${60}^{o}C$. The $pH$ and nature of water at ${60}^{o}C$ will be:
(given: $\sqrt{9.60}=3.10,\log 3.10=0.49$)

1. $6.51$, neutral
2. $6.51$, acidic
3. $6.51$, alkaline
4. $7.51$, alkaline

Q. What is the pH number of hydrochloric acid?

1. Below 7
2. 7
3. Above 7
4. Between 8 and 10

Q. $500mL$ of a strong acid solution of pH = 2 is mixed with $500mL$ of another strong base solution of pOH = 3. The pH of resulting solution will be :
[Given, $\log \left(4.5\right)=0.65$]

1. 3.65
2. 2.35
3. 3.35
4. 2.65

Q. One litre of a buffer solution contains 0.01M $N{H}_{4}Cl$ and 0.1 M $N{H}_{4}OH$. The $p^{kb}$ of base is 5. $p^H$ value of the solution is:

1. 10
2. 4
3. 9
4. 6

Q. The $pH$ of a solution formed by mixing $40mL$ of $0.1M$ $HCl$ with $10mL$ of $0.45M$ of $NaOH$ is:

1. $12$
2. $14$
3. $4$
4. $5$

Q.

Calculate the pH of the resultant mixtures:

a) 10 mL of 0.2M Ca(OH)₂ + 25 mL of 0.1M HCl

b) 10 mL of 0.01M H₂SO₄ + 10 mL of 0.01M Ca(OH)₂

c) 10 mL of 0.1M H₂SO₄ + 10 mL of 0.1M KOH