How might you explain the difference between the ph values of the 0.01 m hcl (ph = 1.1) and the 0.01 m hc2h3o2 (ph = 3.6)? hcl p
1 answer:
Answer:
HCl ionizes more
Explanation:
pH is inversely proportional to the concentration of hydronium ions. It may be calculated by the formula .
Hydrochloric acid is one of the six strong acids and it ionizes to hydronium cations and chloride anions to an extent of about 100 %, meaning the molarity of hydronium would be equal to the initial molarity of hydrochloric acid.
Acetic acid is a weak acid which only partially ionizes, while the majority of acid stays in a molecular form. The same molarity of acetic acid would produce a much lower amount of hydronium as a result.
Therefore, pH of a weak acid would be greater than pH of a strong acid considering we start with the same molarity of eah.
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Answer:
The standard enthalpy of formation of ethanoic acid is -484 kJ/mol.
Explanation:
...[1]
..[2]
..[3]
The standard enthalpy of formation of ethanoic acid :
..[4]
Using Hess's law to calculate :
2 × [1] + 2 × [2] - [3] = [4]
The standard enthalpy of formation of ethanoic acid is -484 kJ/mol.