Answer:
Hydrogen sulphide\[({{H}_{2}}S)\] is
a stronger acid \[({{K}_{a}}=1.0\times {{10}^{-7}})\] than water \[({{K}_{a}}=1.0\times
{{10}^{-14}})\] because S-H bond is longer than O-H bond. Its bond dissociation
enthalpy is therefore, less as compared to that of O-H bond in \[{{H}_{2}}O\].
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