How much heat is produced when 100ml of 0.25 m hcl (density 1.00g/ml) and 200 ml of 0.150 m naoh (densty 1.00g/ml) are mixed?
hcl + naoh ? nacl + h2o ho298= -58kj
if both solutions are the same temperatureand heat capaciy of the products is 4.19 j/gc, how much will the temperature increase? what assumption did you make in your calculation?

Explanation:

The given data is as follows.

For HCl : Volume = 100 mL,  Density = 1.00 g/ml,  Molarity = 0.25 M

For NaOH : Volume = 200 mL,  Density = 1.00 g/ml,  Molarity = 0.150 M

Therefore, mass of HCl will be calculated as follows.

              Density =

                 1.00 g/ml =

                              mass = 100 g

Also, number of moles =

Hence, no. of moles of HCl =    (as 1 ml = 1000 L)

                                              =

On the other hand, mass of NaOH will be calculated as follows.

                 Density =

                 1.00 g/ml =

                              mass = 200 g

Also, number of moles =

Hence, no. of moles of HCl =    (as 1 ml = 1000 L)

                                              =

Total mass = (100 g + 200 g) = 300 g

Since, HCl is the limiting reagent over here. So, heat produced by will be calculated as follows.

         Q =

              =

               = kJ

               =   J

Also, it is known that relation between Q and temperature change is:

                                Q =

Hence, putting the values into the above formula as follows.

                      Q =

      14.5 J =      

                    =              

Thus, we can conclude that increase in temperature is .              

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