- 1(current)
Q. No.Subtopic: Salt Hydrolysis & Titration |
Level 3: 35%-60%
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In the following reaction, HCl formed is titrated with 0.2 moles of NaOH.
Calculate the mass of \(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2\) taken initially:
\(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2+\mathrm{NaNO}_2 \xrightarrow{\mathrm{HCl}} \mathrm{A} \xrightarrow{\mathrm{H}_2 \mathrm{O}} \mathrm{HCl}+\text { Alcohol }+\mathrm{N}_2\)
1. 4
2. 6
3. 9
4. 8
Calculate the mass of \(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2\) taken initially:
\(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2+\mathrm{NaNO}_2 \xrightarrow{\mathrm{HCl}} \mathrm{A} \xrightarrow{\mathrm{H}_2 \mathrm{O}} \mathrm{HCl}+\text { Alcohol }+\mathrm{N}_2\)
1. 4
2. 6
3. 9
4. 8
Subtopic: Salt Hydrolysis & Titration |
79%
Level 2: 60%+
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What is the \(\text{pH}\) of \(\mathrm{CH}_3 \mathrm{COO}^{-} \mathrm{NH}_4^{+}\) salt?
Given: \(\mathrm{K}_{\mathrm{a}} \text { of } \mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-6}\)
\(\mathrm{K}_{\mathrm{b}} \text { of } \mathrm{NH}_4 \mathrm{OH}=1.8 \times 10^{-6}\)
1. \(7\)
2. \(9\)
3. \(8.9\)
4. \(7.8\)
Given: \(\mathrm{K}_{\mathrm{a}} \text { of } \mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-6}\)
\(\mathrm{K}_{\mathrm{b}} \text { of } \mathrm{NH}_4 \mathrm{OH}=1.8 \times 10^{-6}\)
1. \(7\)
2. \(9\)
3. \(8.9\)
4. \(7.8\)
Subtopic: Salt Hydrolysis & Titration |
87%
Level 1: 80%+
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Given below are two statements:
| Assertion (A): | Phenolphthalein is a pH dependent indicator, remains colourless in acidic solution and gives pink colour in basic medium. |
| Reason (R): | Phenolphthalein is a weak acid. It doesn’t dissociate in basic medium. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
Subtopic: Salt Hydrolysis & Titration |
70%
Level 2: 60%+
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The plot of pH-metric titration of weak base \(\mathrm{NH_4OH}\) vs strong acid \(\mathrm{HCl}\) looks like:
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Salt Hydrolysis & Titration |
Level 3: 35%-60%
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\(200 ~mL\) of \(0.2~ M~ {HCl}\) is mixed with \(300 mL \) of \(0.1 ~M ~NaOH\). The molar heat of neutralization of this reaction is \(–57.1~ kJ\). If the increase in temperature of the system on mixing is \(x\times 10^{-2}\). Find the value of \(x\) :
[Given: Specific heat of water \(=4.18~J~g^{-1}K^{-1}\) ; Density of water \(=1.00~\text{g cm}^{-3}]\)
(Assume no volume change on mixing)
1. 84
2. 82
3. 90
4. 92
Subtopic: Salt Hydrolysis & Titration |
65%
Level 2: 60%+
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3g of acetic acid is added to 250 mL of 0.1 M HCl and the solution made up to 500 mL. To 20 mL of this solution 0.5 mL of 5 M NaOH is added. The pH of the solution is :
[Given : pka of acetic acid =4.75, molar mass of acetic acid \(=60 \mathrm{~g} / \mathrm{mol}, \log 3=0.4771 \)]
1. 2.63
2. 5.23
3. 7.08
4. 9.30
[Given : pka of acetic acid =4.75, molar mass of acetic acid \(=60 \mathrm{~g} / \mathrm{mol}, \log 3=0.4771 \)]
1. 2.63
2. 5.23
3. 7.08
4. 9.30
Subtopic: Salt Hydrolysis & Titration |
64%
Level 2: 60%+
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