What is the ph of a solution made by combining 157 ml of 0.35 m nac2h3o2 with 139 ml of 0.46 m hc2h3o2? the ka of acetic acid is 1.75 × 10-5?

The first step is to calculate the molarity of each compound:
final volume of solution = 157 + 139 = 296 mL
molarity of nac2h3o2 = (157 x 0.35) / 296 = 0.1856 molar
molarity of hc2h3o2 = (139 x 0.46) / 296 = 0.216 molar

Then, we calculate the pH as follows:
pKa of acetic acid = -log(1.75 × 10^-5) = 4.7569
pH = pKa +  log ([salt] / [acid]) 
     = 4.7569 + log(0.1856 / 0.216)
     = 4.691

True, the standard unit for volume is liters which can be represented by either a lower case "l" or a capital "l"

Answer : option c) heat is released during the process.explanation :

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.