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Because all strong acids and bases are totally ionised in dilute solution, the enthalpy of neutralisation for both a strong acid and a strong base is always the same. When an acid and an alkali react, heat is emitted, hence the enthalpy changes that occur during neutralisation are always negative. The enthalpy of neutralisation of a strong acid (hydrochloric acid) and a strong base (potassium hydroxide) is the goal of the neutralisation reaction (sodium hydroxide).
What is Standard Enthalpy Change?
Under normal conditions, the standard enthalpy change for neutralization is the enthalpy change, as the acid and alkaline solutions react with each other to produce 1 mol of water. Note that the enthalpy neutralization shift is always measured per mole of water produced. When an acid reacts with a base to release heat, the neutralization change in enthalpy is often negative. For reactions with strong acids and strong bases, the values are very similar, with values ranging from 57 to 58 kJ mol1. It depends on the combination of acid and alkali.
Neutralization reaction
Heat is produced during the neutralisation of an acid with an alkali, according to theory. It is essentially the combination of one equivalent of hydrogen ions with one equivalent of oxygen ions that causes the neutralisation reaction of a strong acid with a strong base to take place.The enthalpy of neutralisation is the amount of heat released when one gramme equivalent of acid is completely neutralised by one gramme equivalent of base in dilute solution, and it is measured in degrees Celsius.
The following is a description of the chemical reaction.
H+ and OH– combine to form H2O and 13.7 kcal.
H+(aq) + Cl–(aq) + Na+(aq) + OH–(aq) Na+(aq) + Cl–(aq) + H2O + 13.7 kcal H+(aq) + Cl- (aq) + H2O + 13.7 kcal
In the neutralisation process, 13.7 kcal of heat is released, which is the heat of neutralisation for all strong acids and bases. Hess discovered the heat of neutralisation to be a constant value of 13.7kcal in almost all cases of strong acids and strong bases in 1840 and published his findings in 1841.
FORMULA
Enthalpy change during neutralization of 100ml of 0.2M HCl
= (200*W)*(t1-t2)*4.2
herefore, the enthalpy change during neutralization of 1000ml of 1M HCl
= (((200*W)*(t1-t2)*4.2)/0.2)*1000/100
Enthalpy of neutralization = (((200*W)*(t1-t2)*4.2)/0.2*100 KJ
PROCESS TO CALCULATE HEAT EVOLVED WHEN THE TWO SOLUTIONS ARE MIXED BY RATIO PROPORTION METHOD
Fill the container with 100ml of 0.2M hydrochloric acid solution.Now, take note of the temperature of the acid solution in the container.Take a second vessel and fill it with 100ml of 0.2M sodium hydroxide solution. Set this vessel aside.Make a note of the temperature at which the sodium hydroxide was first applied.Wait until the temperature of both solutions reaches the same level.In a hurry, add 100mL of sodium hydroxide solution to the hydrochloric acid in a separate container.Insert the cork, which has a thermometer and a stirrer in the mouth, as soon as possible.Stir the solution thoroughly, taking note of the temperature at regular intervals of time throughout the experiment.The temperature should be noted down indefinitely until the temperature becomes constant.Make a note of the highest temperature that was reached.Calculate the amount of heat that is released when the two solutions are mixed together using the ratio proportion method.
CONCLUSION
In the reaction of HCl with NaOH, the enthalpy of neutralisation is kJ. In the reaction, the H+ ions of Hydrogen in an acid combine with the OH- (hydroxide) ions of the basic solution, and this is how water is formed from neutralization. The neutralized solution usually has a ph seven value, but the pH value can differ depending on the acidic or basic strength of the reactants. When the neutralization process takes place between a strong acid and a weak base, then the pH level would be less than 7, and conversely for a reaction between a strong base and weak acid will result in a solution of pH value more than 7
