Answer:
25.11 g.
Explanation:
- It is clear from the balanced equation:
<em>Ag₂O + 2HCl → 2AgCl + H₂O.</em>
<em></em>
that 1.0 mole of Ag₂O reacts with 2.0 moles of HCl to produce 2.0 mole of AgCl and 1.0 moles of H₂O.
- 7.8 g of HCl reacts with excess Ag₂O. To calculate the no. of grams of Ag₂O that reacted, we should calculate the no. of moles of HCl:
<em>no. of moles of HCl = mass/atomic mass</em> = (7.9 g)/(36.46 g/mol) = <em>0.2167 mol.</em>
- From the balanced equation; every 1.0 mol of Ag₂O reacts with 2 moles of HCl.
∴ 0.2167 mol of HCl will react with (0.2617 mol / 2 = 0.1083 mol) of Ag₂O.
<em>∴ The mass of reacted Ag₂O = no. of moles x molar mas</em>s = (0.1083 mol)(231.735 g/mol) = <em>25.11 g.</em>
This problem is asking for the dissolution reaction of barium fluoride, both the equilibrium and Ksp expressions in terms of concentrations and x and its molar solubility in water. Thus, answers shown below:
<h3>Solubility product</h3>
In chemistry, when a solid is dissolved in water, one must take into account the fact that not necessarily its 100 % will be able to break into ions and thus undergo dissolution.
In such a way, and specially for sparingly soluble solids, one ought to write the dissolution reaction at equilibrium as shown below for the given barium fluoride:

Next, we can write its equilibrium expression according to the law of mass action, which also demands us to omit any solid and refer it to the solubility product constant (Ksp):
![Ksp=[Ba^{2+}][F^-]^2](https://tex.z-dn.net/?f=Ksp%3D%5BBa%5E%7B2%2B%7D%5D%5BF%5E-%5D%5E2)
Afterwards, one can insert the reaction extent, x, as it stands for the molar solubility of this solid in water, taking into account the coefficients balancing the reaction:

Finally, we solve for the x as the molar solubility of barium fluoride as shown below:
![2.5x10^{-5}=(x)(2x)^2\\\\2.5x10^{-5}=4x^3\\\\x=\sqrt[3]{\frac{2.5x10^{-5}}{4} } \\\\x=0.0184M](https://tex.z-dn.net/?f=2.5x10%5E%7B-5%7D%3D%28x%29%282x%29%5E2%5C%5C%5C%5C2.5x10%5E%7B-5%7D%3D4x%5E3%5C%5C%5C%5Cx%3D%5Csqrt%5B3%5D%7B%5Cfrac%7B2.5x10%5E%7B-5%7D%7D%7B4%7D%20%7D%20%5C%5C%5C%5Cx%3D0.0184M)
Learn more about chemical equilibrium: brainly.com/question/26453983
Answer:
pH = 9: Basic; pH = 2.3: acidic; pH = 11: basic; pH = 5: Acidic; [H⁺] = 0.0056M: Acidic; [H⁺] = 3.45E-9M: Basic
Explanation:
A solution is defined as acidic when pH < 7 and as basic when pH > 7.
Also, pH = -log[H⁺].
Thus:
pH = 9: >7 → Basic
pH = 2.3: <7 → Acidic
pH = 11: >7 → Basic
pH = 5: <7 → Acidic
[H⁺] = 0.0056M, pH = -log0.0056M = 2.25: <7: Acidic
[H⁺] = 3.45E-9M, pH = 8.46: > 7: Basic