If a particular ore contains 55.4 % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosp
1 answer:
You might be interested in
<u>Answer:</u> The pH of the solution in the beginning is 1.89 and the pH of the solution after the addition of base is
<u>Explanation:</u>
- <u>For 1:</u> At the beginning
To calculate the pH of the solution, we use the equation:
We are given:
Nitric acid is a monoprotic acid and it dissociates 1 mole of hydrogen ions. So, the concentration of hydrogen ions is 0.013 M
Putting values in above equation, we get:
- <u>For 2:</u>
To calculate the number of moles, we use the equation:
- <u>For nitric acid:</u>
Molarity of nitric acid solution = 0.013 M
Volume of solution = 15 mL
Putting values in above equation, we get:
- <u>For methylamine:</u>
Molarity of methylamine solution = 0.017 M
Volume of solution = 10 mL
Putting values in above equation, we get:
- The chemical equation for the reaction of nitric acid and methylamine follows:
As, the mole ratio of nitric acid and methyl amine is 1 : 1. So, the limiting reagent will be the reactant whose number of moles are less, which is methyl amine.
By Stoichiometry of the reaction:
1 mole of methyl amine produces 1 mole of
So, of methyl amine will produce =
To calculate the of base, we use the equation:
where,
= base dissociation constant =
Putting values in above equation, we get:
- To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:
We are given:
Putting values in above equation, we get:
To calculate pH of the solution, we use the equation:
Hence, the pH of the solution is 4.59
Answer:
1.8 × 10⁻¹⁶ mol
Explanation:
(a) Calculate the solubility of the Sr₃(PO₄)₂
Let s = the solubility of Sr₃(PO₄)₂.
The equation for the equilibrium is
Sr₃(PO₄)₂(s) ⇌ 3Sr²⁺(aq) + 2PO₄³⁻(aq); Ksp = 1.0 × 10⁻³¹
1.2 + 3s 2s
(b) Concentration of PO₄³⁻
[PO₄³⁻] = 2s = 2 × 1.20× 10⁻¹⁶ mol·L⁻¹ = 2.41× 10⁻¹⁶ mol·L⁻¹
(c) Moles of PO₄³⁻
Moles = 0.750 L × 2.41 × 10⁻¹⁶ mol·L⁻¹ = 1.8 × 10⁻¹⁶ mol