Answer:
pH of the solution after addition of 8 ml 0,296 molar HCl = 7.94
Explanation:
In this case buffer exist between hypochlorous acid HClO is a weak acid and its conjugate base hypochlorite ion ClO⁻ which are deliver to the solution by NaOCl ( sodium hypochlorite ).
The salt is completely dissociate
[NaOCl] = [ClO⁻]
Using Henderson equation to find pH of this buffer
pH = pKa + log![\frac{[Conjugate base]}{[Acid]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BConjugate%20base%5D%7D%7B%5BAcid%5D%7D)
or, = 7.53 + log
or, = 7.53 + 0.4
or, = 7.94
Answer:
What changes do you notice? The white you see have undergone coral bleaching. At high temperatures, corals may lose their zooxanthellae, causing corals to lose their color and their main source of food. Once bleaching occurs, the coral colony usually dies.
Explanation:
study well
Arigato
For a tragedy of the commons to occur a resource must be scarce, rivalrous in consumption, and non-excludable. Solutions to the tragedy of the commons include the imposition of private property rights, government regulation, or the development of a collective action arrangement.
Answer:
Substances that dissolve most readily in water include ionic compounds and polar covalent compounds. aqueous solution. water that contains dissolved substances. solvent. the dissolving medium in a solution.
Explanation:
Answer:
83.64%.
Explanation:
∵ The percent yield = (actual yield/theoretical yield)*100.
actual yield of CO₂ = 2300 g.
- We need to find the theoretical yield of CO₂:
For the reaction:
<em>CH₄ + 2O₂ → 2H₂O + CO₂,</em>
1.0 mol of CH₄ react with 2 mol of O₂ to produce 2 mol of H₂O and 1.0 mol of CO₂.
- Firstly, we need to calculate the no. of moles of 1000 g of CH₄ using the relation:
<em>no. of moles of CH₄ = mass/molar mass</em> = (1000 g)/(16.0 g/mol) = <em>62.5 mol.</em>
<u><em>Using cross-multiplication:</em></u>
1.0 mol of CH₄ produces → 1.0 mol of CO₂, from stichiometry.
∴ 62.5 mol of CH₄ produces → 62.5 mol of CO₂.
- We can calculate the theoretical yield of carbon dioxide gas using the relation:
∴ The theoretical yield of CO₂ gas = n*molar mass = (62.5 mol)(44.0 g/mol) = 2750 g.
<em>∵ The percent yield = (actual yield/theoretical yield)*100.</em>
actual yield = 2300 g, theoretical yield = 2750 g.
<em>∴ the percent yield</em> = (2300 g/2750 g)*100 = <em>83.64%.</em>
