Question

0.2 mol of NasPOs and 0.5 mol of Ba(NO3)2 are mixed in 1 L of solution. Which of the following
statements are correct about this solution ?
(A) 0.2 mol of barium phosphate precipitate is obtained.
(B) 0.1 mol of barium phosphate precipitate is obtained.
(C) Molarity of Ba?ion in the resulting solution is 0.2 M.
(D) Molarities of Na* and NOS ions are 0.6 M and 10 M respectively

Answer 1

Answer:

(B) otion is correct

Explanation:

(B)0.1 mole of barium phosphate precipitate is obtained.

Answer 2

Answer:

The correct options for this question are options B, C, and D.

Explanation:

The appropriate balanced reaction is:

2Na₃PO₄(aq) + 3Ba(NO₃)₂(aq) → Ba₃(PO₄)₂(aq)↓ + 6NaNo₃(aq)

So, Na₃PO₄ is used up completely and serves as the limiting reagent.

Moles of Ba₃(PO₄)₂ formed = $\frac{0.2}{2}$ mol = 0.1 mol

Moles of unreacted Ba(NO₃)₂ = (0.5 − 0.3) mol

⇒ 0.2 = mol of Ba²⁺ ion.

The reacted 0.3 Ba²⁺ will be precipitated as 0.1-mole barium phosphate.

Moles of Na⁺ in solution = 0.2 × 3 = 0.6

Moles of NO₃⁻ in solution = 0.5 × 2 = 1

An inorganic salt called barium phosphate is utilized in the chemical and optical industries to make pulsed lasers and glasses. A salt that is classified as inorganic is barium phosphate. The chemical formula for barium phosphate is Ba₃(PO₄)₂. Although barium phosphate is typically thought of as a colorless solid, it does have a fading odour resembling acetic vinegar. Many general chemistry conclusions are based on the fact that barium phosphate precipitates from aqueous solutions of barium salt and phosphate salt.

Thus, the insoluble nature of barium phosphate is demonstrated by the appearance of a solid white precipitate.