Answer:
The concentration of [Ca²⁺] is 8.47 x 10⁻³ M
Explanation:
We consider the solubility of hydroxyapatite,
Ca₁₀(PO₄)₆(OH)₂ ⇔ 10Ca²⁺ + 6PO₄³⁻ + 2 OH⁻
Assumed that there is <em>a</em> mol of hydoxyapatite disolved in water, yielding <em>10a</em> mol Ca²⁺ of and <em>6a</em> mol of PO₄³⁻
We also have Ksp equation,
Ksp = [Ca²⁺]¹⁰ x [PO₄³⁻]⁶ x [OH⁻]² = 2.34 x 10⁻⁵⁹
⇔ 10a¹⁰ x 6a⁶ x (5.30 x 10⁻⁶)² = 2.24 x 10⁻⁵⁹
⇔ 60a¹⁶ = 2.24 x 10⁻⁵⁹ / 5.30 x 10⁻¹²
⇔ a¹⁶ = 0.007 x 10⁻⁴⁷ = 7 x 10⁻⁵⁰
⇔ a = ![\sqrt[16]{7 . 10^{-50} }](https://tex.z-dn.net/?f=%5Csqrt%5B16%5D%7B7%20.%2010%5E%7B-50%7D%20%7D)
= 8.47 x 10⁻⁴
Hence,
[Ca²⁺] = 10<em>a</em> = 8.47 x 10⁻³ M
Answer:
The water in the tank is basic.
Explanation:
Acidity or basicity of an aqueous solution is determined through it pH value.
![pH=-log[H^{+}]](https://tex.z-dn.net/?f=pH%3D-log%5BH%5E%7B%2B%7D%5D)
, where ![[H^{+}]](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D)
is concentration of 
(in molarity) in solution.
As a matter of fact, a pH scale has been established such as:
Acidic (
), Neutral (
) and Basic (
)
As pH = 8.0 lies in the basic range of pH scale therefore the water in the tank is basic.
<u><em>In metallic bonding, the valence electrons are free to move throughout the metal structure. Metallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalized electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.</em></u>
You'd need
33.6 g
of aluminium to react with that much manganese dioxide.
So, you've got your balanced chemical equation for this reaction
3
M
n
O
2
(
s
)
+
4
A
l
(
s
)
→
3
M
n
(
s
)
+
2
A
l
2
O
3
(
s
)
The mole ratio that exists between manganese dioxide and aluminium is simply the ration between the stoichiometric coefficients placed in front of them.
In your case, the balanced chemical equation shows that you have 3 moles of manganese dioxide reacting with 4 moles of aluminium; this means that your mole ratio will be
3:4
.
Likewise, the mole ratio between aluminium and manganese dioxide will be
4:3
→
4 moles of the former need 3 moles of the latter.
You can put this mole ratio to good use by determining how many moles of aluminium are needed to react with the number of moles of manganese dioxide present in 81.2 g. So,
81.2 g MnO
2
⋅
1 mole
86.94 g
=
0.9340 moles
M
n
O
2
This means that you'll need
0.934 moles
M
n
O
2
⋅
4 moles Al
3 moles
M
n
O
2
=
1.245 moles Al
To determine the number of grams needed to get that many moles use aluminium's molar mass
1.245 moles Al
⋅
26.98 g
1 mole Al
=
33.59 g Al
Rounded to three sig figs, the answer will be
m
aluminium
=
33.6 g
