A solution has a pH of 2.4. What happens to the solution if the hydronium ion concentration is increased?
2 answers:
Answer:
The pH would decrease and the solution would become more acidic
Explanation:
pH of a solution is a measure of its hydronium ion (H3O+) concentration. Mathematically it is given as:
It is given that pH of the solution = 2.4
Therefore based on equation (2), the [H3O+] would be:
If the [H3O+] concentration were increased then based on equation (1) the pH of the solution would decrease i.e. it would become more acidic.
For example, lets say that the new [H3O+] = 5.0 * 10⁻³ M, then
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Answer:
The equilibrium value of [CO] is 1.04 M
Explanation:
Chemical equilibrium is the state to which a spontaneously evolving chemical system, in which a reversible chemical reaction takes place. When this situation is reached, it is observed that the concentrations of substances, both reagents and reaction products, they remain constant over time. That is, the rate of reaction of reagents to products is the same as that of products to reagents.
Reagent concentrations and products in equilibrium are related by the equilibrium constant Kc. Being:
aA + bB ⇔ cC + dD
Then this constant Kces equals the multiplication of the concentrations of the products raised to their stoichiometric coefficients between the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients.
In this case:
You know:
- Kc= 14.5
- [H₂]= 0.322 M
- [CH₃OH] =1.56 M
Replacing:
Solving:
[CO]= 1.04 M
The equilibrium value of [CO] is 1.04 M