Salt of Strong Acid and Strong Bases

Q.

50 mL of 0.1 M HCl and 50 mL of 2.0 M NaOH are mixed. The pH of the resulting solution is -

Consider $log\left(2\right)=0.30$

1. 1.3
2. 4.2
3. 12.7
4. 11.7

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. 1
2. 7
3. 1.3
4. 2

Q. Calculate pH of a solution which contains 9.9 mL of 1 M $HCl$ and 100 mL of 0.1 M $NaOH$.
Take $log\left(9.1\right)=0.96$

1. 10.96
2. 5.96
3. 7.96
4. 12.96

Q.

A solution of NaCl is

1. Acidic in nature

2. Alkaline in nature

3. Neutral in nature

4. Amphoteric in nature

Q. What will be the resultant pH when 150 mL of an aqueous solution of $HCl$ $(pH=2.0)$ is mixed with 350 mL of an aqueous solution of $NaOH(pH=12.0)$?
Take $log\left(2\right)=0.3$

1. 8.6
2. 12.6
3. 11.6
4. 10.6

Q. The salt that forms neutral solution in water is

1. $N{H}_{4}Cl$
2. $NaCl$
3. $N{a}_{2}C{O}_3$
4. $K_{3}B{O}_2$

Q. A $25mL$ solution of $0.2MN{H}_{4}OH$ is titrated against $0.2MHCl$. Find the $pH$ of the solution when $25mL$ of $HCl$ is added.
$p{K}_b\left(N{H}_{4}OH\right)=4.74$

1. 8.37
2. 4.74
3. 5.13
4. 3.55

Q. What will be the resultant pH when 150 mL of an aqueous solution of $HCl$ $(pH=2.0)$ is mixed with 350 mL of an aqueous solution of $NaOH(pH=12.0)$?
Take $log\left(2\right)=0.3$

1. 8.6
2. 12.6
3. 11.6
4. 10.6

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 pH of a solution which contains 9.9 mL of 1 M $HCl$ and 100 mL of 0.1 M $NaOH$.
Take $log\left(9.1\right)=0.96$

1. 7.96
2. 12.96
3. 10.96
4. 5.96