Identify the correct statements from the foll | vedclass

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(A) The ionic product of water $(K_w)$ at $100^{\circ} C$ is approximately $51.3 	imes 10^{-14}$,which is greater than $10^{-14}$. Thus,statement $(A

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$B, C, D$

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(A) The ionic product of water $(K_w)$ at $100^{\circ} C$ is approximately $51.3 	imes 10^{-14}$,which is greater than $10^{-14}$. Thus,statement $(A)$ is incorrect.$(B)$ The dissociation of water is an endothermic process. As temperature increases,$K_w$ increases,which leads to a decrease in the $pH$ of neutral water $(pH = -\log[H^+])$. Thus,statement $(B)$ is correct.$(C)$ $NaH_2PO_4$ is a salt of a strong base $(NaOH)$ and a weak acid $(H_3PO_4)$. However,the anion $H_2PO_4^-$ acts as an acid $(K_a > K_b)$,making the solution acidic,not basic. Thus,statement $(C)$ is incorrect.$(D)$ $NH_3$ can accept a proton to form $NH_4^+$ (acting as a Bronsted base) and can donate a proton to form $NH_2^-$ (acting as a Bronsted acid). Thus,statement $(D)$ is correct.Note: Based on the analysis,only $(B)$ and $(D)$ are correct. However,if the question implies $Na_2HPO_4$ in option $(C)$,it would be basic. Given the options provided,there is a discrepancy in the standard interpretation.

Identify the correct statements from the following.
$(A)$ The ionic product of water at $100^{\circ} C$ is $< 10^{-14}$.
$(B)$ $pH$ 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.

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Identify the correct statements from the following.$(A)$ The ionic product of water at $100^{\circ} C$ is $< 10^{-14}$.$(B)$ $pH$ 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.