Answer:
Ksp= 7.98 × 10^-13
Explanation:
According to the question, we are to calculate the solubility constant (Ksp) of Zinc carbonate (ZnCO3) in a dissolved solution.
The equilibrium of the reaction is:
ZnCO3 (aq) ⇌ Zn2+ (aq) + CO32- (aq)
According to this; 1 mole of Zinc carbonate (ZnCO3) dissolves to give 1 mole of Zinc ion (Zn2+) and 1 mole of carbonate ion (CO32-).
This illustrates that:
(Zn2+) = 1.12 x 10-4 g/L
(CO32-) = 1.12 x 10-4 g/L
However, 1.12 x 10-4 g/L is the solubility in mass concentration of ZnCO3, we need to convert it to molar concentration in mol/L by dividing by the relative molar mass of ZnCO3.
To calculate the molar mass of ZnCO3, we say:
Zn (65.4) + C (12) + 03 (16×3)
= 65.4+12+48
= 125.4g/mol.
Hence, molar concentration= 1.12 x 10-4 g/L / 125.4 g/mol
= 8.93 × 10^-7 mol/L.
Therefore;
Zn2+) = 8.93 x 10-7 mol/L
(CO32-) = 8.93 x 10-7 mol/L
Ksp = [Zn2+] [CO32-]
Ksp = (8.93 x 10-7) × (8.93 x 10-7)
Ksp = 7.98 × 10^-13
Answer:
the scattering and reflection of light by dust particles
Answer:
10.96
Explanation:
<em>A solution is prepared at 25 °C that is initially 0.14 M in diethylamine, a weak base with Kb = 1.3 × 10⁻³, and 0.20 M in diethylammonium chloride. Calculate the pH of the solution. Round your answer to 2 decimal places.</em>
Step 1: Calculate the pOH of the solution
Diethylamine is a weak base and diethylammonium (from diethylammonium chloride) its conjugate acid. Thus, they form a buffer system. We can calculate the pOH of this buffer system using the Henderson-Hasselbach's equation.
pOH = pKb + log [acid]/[base]
pOH = -log 1.3 × 10⁻³ + log 0.20 M/0.14 M
pOH = 3.04
Step 2: Calculate the pH of the solution
We will use the following expression.
pH + pOH = 14
pH = 14 - pOH = 14 -3.04 = 10.96
The answer is potential energy...
Hope this helped :)
