What is the mass of precipitate formed when 50 ml of 16.9% w/v solution of AgNO3 is mixed with 50 ml of 5.8% w/v NaCl solution?

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What is the mass of precipitate formed when 50 ml of 16.9% w/v solution of AgNO3 is mixed with 50 ml of 5.8% w/v NaCl solution?

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Answer 1 · 2017-08-17T17:31:11

Well, $w/v \equiv \frac{Mass of solute}{Volume of solution}$ $"w/v"-="Mass of solute"/"Volume of solution"$ , we should get over $7 \cdot g$ $7*g$ of silver chloride.

Explanation:

And thus $mass of silver nitrate = 16.9 % \times 50 \cdot m L = 8.45 \cdot g$ $"mass of silver nitrate"=16.9%xx50*mL=8.45*g$ .

And this represents a molar quantity of $\frac{8.45 \cdot g}{169.87 \cdot g \cdot m o l^{- 1}}$ $(8.45*g)/(169.87*g*mol^-1)$

$= 0.0497 \cdot m o l$ $=0.0497*mol$ , with respect to $A g N O_{3}$ $AgNO_3$ .

Likewise $mass of sodium chloride = 5.8 % \times 50 \cdot m L = 2.90 \cdot g$ $"mass of sodium chloride"=5.8%xx50*mL=2.90*g$ .

And this represents a molar quantity of $\frac{2.90 \cdot g}{58.44 \cdot g \cdot m o l^{- 1}}$ $(2.90*g)/(58.44*g*mol^-1)$

$= 0.0497 \cdot m o l$ $=0.0497*mol$ with respect to $N a C l$ $NaCl$ .

Clearly the reagents are present in 1:1 molar ratio. The reaction that occurs in solution is the precipitation of a curdy white mass of $A g C l (s)$ $AgCl(s)$ , i.e. and we represent this reaction by the net ionic equation.....

$A g^{+} + C l^{-} \to A g C l (s) ⏐ ↓$ $Ag^(+) + Cl^(-)rarrAgCl(s)darr$

Of course the complete reaction is....

$A g N O_{3} (a q) + N a C l (a q) \to A g C l (s) ⏐ ↓ + N a N O_{3} (a q)$ $AgNO_3(aq) + NaCl(aq) rarr AgCl(s)darr + NaNO_3(aq)$ , i.e. sodium nitrate remains in solution and can be separated (with effort) from the precipitate.

And given the stoichiometry, we gets $0.04974 \cdot m o l \times 143.32 \cdot g \cdot m o l^{- 1} = 7.11 \cdot g$ $0.04974*molxx143.32*g*mol^-1=7.11*g$ .

Of course a material such as silver halide would be very hard to isolate. Particle size is very small; it is likely to clog the filter, and filter very slowly; and moreover $A g C l$ $AgCl$ is photoactive, and would decompose under light.

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What is the mass of precipitate formed when 50 ml of 16.9% w/v solution of AgNO3 is mixed with 50 ml of 5.8% w/v NaCl solution?

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