\( \mathrm{AgCl} \) dissolves in a solution of \( \mathrm{NH}_{3} \...

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\( \mathrm{AgCl} \) dissolves in a solution of \( \mathrm{NH}_{3} \) but not in water because
\( \mathrm{P} \)
(1) \( \mathrm{NH}_{3} \) is a better solvent than \( \mathrm{H}_{2} \mathrm{O} \)
(2) \( \mathrm{Ag}^{+} \)forms a complex ion with \( \mathrm{NH}_{3} \)
W
(3) \( \mathrm{NH}_{3} \) is a stronger base than \( \mathrm{H}_{2} \mathrm{O} \)
(4) The dipole moment of water is higher than \( \mathrm{NH}_{3} \)
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