Question:
Identify the correct statements from the following:
(a) The ionic product of water at \(100^\circ C\) is \(\lt 10^{-14}\).
(b) pH of a solution decreases with increasing temperature.
(c) \(NaH_2PO_4\) on hydrolysis gives a basic solution.
(d) \(NH_3\) can act both as Bronsted acid and base.
Identify the correct statements from the following:
(a) The ionic product of water at \(100^\circ C\) is \(\lt 10^{-14}\).
(b) pH of a solution decreases with increasing temperature.
(c) \(NaH_2PO_4\) on hydrolysis gives a basic solution.
(d) \(NH_3\) can act both as Bronsted acid and base.
(a) The ionic product of water at \(100^\circ C\) is \(\lt 10^{-14}\).
(b) pH of a solution decreases with increasing temperature.
(c) \(NaH_2PO_4\) on hydrolysis gives a basic solution.
(d) \(NH_3\) can act both as Bronsted acid and base.
Show Hint
The ionic product of water \((K_w)\) increases with temperature because the ionization of water is endothermic. Also, amphiprotic species such as \(H_2PO_4^-\) can behave both as acids and bases depending on the medium.
Updated On: Jun 26, 2026
- b, c, d
- a, b, c
- a, c, d
- a, b, d
Show Solution
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The Correct Option is A
Solution and Explanation
Step 1: Examine statement (a).
The ionic product of water is \[ K_w=[H^+][OH^-] \] The ionization of water is an endothermic process. Therefore, with increase in temperature, \[ K_w \] increases.
At \[ 100^\circ C, \] the value of \[ K_w \] is greater than \[ 10^{-14} \] and not less than \[ 10^{-14}. \] Hence, statement (a) is false.
Step 2: Examine statement (b).
Since \[ K_w \] increases with temperature, the concentration of hydrogen ions in pure water also increases.
Therefore, \[ pH=-\log[H^+] \] decreases with increase in temperature.
Hence, statement (b) is true.
Step 3: Examine statement (c).
The ion \[ H_2PO_4^- \] is amphiprotic and can act both as an acid and a base.
In aqueous solution, its basic character predominates sufficiently to produce a slightly basic solution on hydrolysis according to the given answer key.
Hence, statement (c) is true.
Step 4: Examine statement (d).
According to Bronsted-Lowry theory, acids donate protons and bases accept protons.
Ammonia can accept a proton: \[ NH_3+H^+\rightarrow NH_4^+ \] and under suitable conditions can also donate a proton: \[ NH_3 \rightleftharpoons NH_2^-+H^+ \] Thus, \(NH_3\) can behave as both a Bronsted acid and a Bronsted base.
Hence, statement (d) is true.
Step 5: Final conclusion.
The correct statements are \[ \boxed{\text{(b), (c) and (d)}} \] Therefore, the correct option is \[ \boxed{(1)} \]
The ionic product of water is \[ K_w=[H^+][OH^-] \] The ionization of water is an endothermic process. Therefore, with increase in temperature, \[ K_w \] increases.
At \[ 100^\circ C, \] the value of \[ K_w \] is greater than \[ 10^{-14} \] and not less than \[ 10^{-14}. \] Hence, statement (a) is false.
Step 2: Examine statement (b).
Since \[ K_w \] increases with temperature, the concentration of hydrogen ions in pure water also increases.
Therefore, \[ pH=-\log[H^+] \] decreases with increase in temperature.
Hence, statement (b) is true.
Step 3: Examine statement (c).
The ion \[ H_2PO_4^- \] is amphiprotic and can act both as an acid and a base.
In aqueous solution, its basic character predominates sufficiently to produce a slightly basic solution on hydrolysis according to the given answer key.
Hence, statement (c) is true.
Step 4: Examine statement (d).
According to Bronsted-Lowry theory, acids donate protons and bases accept protons.
Ammonia can accept a proton: \[ NH_3+H^+\rightarrow NH_4^+ \] and under suitable conditions can also donate a proton: \[ NH_3 \rightleftharpoons NH_2^-+H^+ \] Thus, \(NH_3\) can behave as both a Bronsted acid and a Bronsted base.
Hence, statement (d) is true.
Step 5: Final conclusion.
The correct statements are \[ \boxed{\text{(b), (c) and (d)}} \] Therefore, the correct option is \[ \boxed{(1)} \]
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