Sn + 2Cl2 ------> SnCl4
from reaction 2 mol 1 mol
from the problem 2.85 mol x mol
x=2.85*1/2≈1.43 mol SnCl4
Answer:
A
Explanation:
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Answer is: H+ will increase and OH− will decrease.
pH = 11.4.
pH = -log[H+].
[H+] = 10∧(-pH).
[H+] = 10∧(-11.4).
[H+] = 4·10⁻¹² mol/L.
[H+] · [OH-] = 1·10⁻¹⁴ mol²/dm⁶.
[OH-] = 0.0025 mol/L.
pH value (potential of hydrogen - [H+]) is a logarithmic scale that specify the acidity or basicity of an aqueous solution.
When pH is greater than seven, aqueous solution is basic, below seven is acidic and when pH is equal seven, solution is neutral.
Answer:
Kc = 6x10⁻⁶
Explanation:
For the reaction:
4NH₃(g) + 3O₂(g) ⇄ 2N₂(g) + 6H₂O(g)
Kc is defined as:
Kc =[N₂]² [H₂O]⁶ / [NH₃]⁴ [O₂]³
The equilibrium concentrations of the gases is -Because volume of the container is 1.00L-:
[N₂] = 2X = 1.96x10⁻³; <em>X = 9.8x10⁻⁴</em>
[H₂O] = 6X; 6ₓ9.8x10⁻⁴ = 5.88x10⁻³
[NH₃] = 0.0150M - 4X = 0.01108M
[O₂] = 0.0150M - 3X = 0.01206M
Replacing in Kc expression:
Kc =[1.96x10⁻³]² [5.88x10⁻³]⁶ / [0.01108M]⁴ [0.01206M]³
<h3>Kc = 6x10⁻⁶</h3>
We can conclude that the solution is an <em>acid buffer</em>. A buffer system is when a weak acid is mixed with its salt. Its purpose is to resist changes in pH when small amounts of acid or base is added.
