First, we need to correct the mistake in the problem statement. Sodium acetate is not NaOH; it is CH3COONa. Now, let's proceed with the calculation.To calculate the enthalpy change, we need to find the heat absorbed by the solution and then divide it by the number of moles of sodium acetate.Step 1: Calculate the heat absorbed by the solutionq = mcTwhere q is the heat absorbed, m is the mass of the solution, c is the specific heat capacity, and T is the change in temperature.Assuming that the mass of the solution is approximately equal to the mass of sodium acetate since the mass of water is not given , we have:m = 10 gc = 4.18 J/ gC T = 30C - 25C = 5Cq = 10 g 4.18 J/ gC 5C = 209 JStep 2: Calculate the total heat involved in the reactionSince the heat evolved by the reaction is 677 J, the total heat involved in the reaction is the sum of the heat absorbed by the solution and the heat evolved by the reaction.Total heat = Heat absorbed by the solution + Heat evolved by the reactionTotal heat = 209 J + 677 J = 886 JStep 3: Calculate the number of moles of sodium acetateThe molar mass of sodium acetate CH3COONa is approximately 82 g/mol.Moles of sodium acetate = mass / molar massMoles of sodium acetate = 10 g / 82 g/mol = 0.122 molStep 4: Calculate the enthalpy changeEnthalpy change = Total heat / Moles of sodium acetateEnthalpy change = 886 J / 0.122 mol = 7260 J/molThe enthalpy change for the hydrolysis of 10 grams of sodium acetate at 25C is 7260 J/mol.