The enthalpy of the following acid-base neutralization reaction is -58 kJ/mol:\[ \text{HCl(aq) + NaOH(aq) } \rightarrow \text{ H}_2\text{O + NaCl (aq)} \]a. 15.0 mL of 0.25M HCl is mixed with 35.0 mL of 0.25 M NaOH in an insulated coffee-cup calorimeter. Both solutions are initially at 20.0°C. What will be the final temperature of the solution once thermal equilibrium is reached? (density of solution is 1.0 g/mL, and you can assume that the specific heat of solution is 4.2 J/g°C)b. 35.0 mL of 0.25M HCl is mixed with 15.0 mL of 0.25 M NaOH in an insulated coffee-cup calorimeter. Both solutions are initially at 20.0°C. What will be the final temperature of the solution once thermal equilibrium is reached?c. Suppose you wanted to maximize the amount of heat released by mixing these two solutions together, subject to the constraint that the total volume of your mixture must be 50.0 mL. What volume of each solution should you use? Explain your reasoning.d. How would your answer to part (c) be different if the concentration of NaOH used was 0.50M and the concentration of HCl remained at 0.25M?

Dear Subscriber! There are four independent questions posted here. As per our authoring guidelines, we have solved the first one(a) here. Please repost the remaining separately for us to address. The given neutralization reaction is HCl (aq)+NaOH(aq)→H2O+NaCl(aq) ∆H=-58kJ/molWe can use the following relationN1V1=N2V2where N1 is normality of HCl, V1 is the volume of HCl, N2 is the normality of NaOH, and V2 is volume of NaOHin terms of n factor( number of moles)mmol of HCl=n1M1V1=1×0.25×15 =3.75 mmol, or 3×10-3molSimilarlymmol of NaOH=n2M2V2=1×0.25×35=8.75mmol, or 8.75×10-3molWe can see that HCl is the limiting reactant here, so that the absolute enthalpyof the reaction isQ=58 kJ/mol×3×10-3mol=0.174 kJ, or 174 JMass of solution, m=density×volume=1 g/mL×(15+35)mL=50 gUsing the relationQ=mCp∆Twhere Cp is heat capacity of solution and ∆T is change in temperature174 J=50 g×4.2 J/goC×(Tfinal-20oC)Tfinal=20.828oCHence the solution will be at 20.828oC when the equilibrium is reached