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25.0 mL of 1.0M HCl is combined with 35....

25.0 mL of 1.0M HCl is combined with 35.0 mL of 0.5 M NaOH. The initial temperatures of the solutions is `25^@C`, the density of the solution is 1.0 g/mL, the specific heat capacity of the solution is `4.184 J//g .^(@)C`, the reaction is completed in insulated beaker, and the standard enthalpy of reaction for `H^(+)(aq) + OH^(-)(aq) rarr H_(2)O (l)` is `-56 kJ//mol` . What is the final temperature of the solution?

A

`27^@C`

B

`28.9^@C`

C

`30.1^@C`

D

`32.8^@C`

Text Solution

Verified by Experts

The correct Answer is:
B
Heat Liberated due to neutralisation `=56 xx (0.5 xx 3.5 xx 10^(-3)) kJ = 0.98 kJ`
[Meq. `H_2O` formed = `0.5 xx 35` ]
`implies " "`Heat Liberated due to neutralisation = Heat gained by the system
`implies 980 = (60 xx 1) xx 4.18 xx (T - 25) [ :' "Total volume of solution" = 60 ml] implies T = 28.9^(@)C`. [ Total volume of solution = 60 ml]
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