Question

What is the mass of precipitate formed when 50ml of 16.9% solution AgNO3 is mixed wth 50ml 5.8 % NaCl solution

Answer 1

moles of AgNo3= 50x 16.9/100x169.8
                           = 0.05mole
Moles of NaCl = 50x5.8/100x58.5
                       =0.05mole
AgNo3 + NaCl ----> AgCl + NaNo3
mass of AgCl = mole x molar mass
                       =0.05 x 143.5
                       = 7.16 g

Answer 2

Precipitation is the process of converting dissolved material into an insoluble solid from a super-saturated solution in an aqueous solution, and the solid created is known as the precipitate.

Solution:

Given:

Volume of $AgNO_{3}$ solution = 50ml

The concentration of $AgNO_{3}$ solution = 16.9%

The volume of NaCl Solution = 50ml

The concentration of NaCl Solution = 5.8%

To find:

Mass of precipitate formed =?

Step by step explanation:

• Moles of $AgNO_{3}$ = $50*16.9/100*169.8 = 0.05 mole$
• Moles of NaCl = $50*5.8/100*58.5= 0.05 mole$
• Balanced Equation for the reaction will be:

$AgNO_{3} + NaCl$ ⟶ $AgCl + NaNO_{3}$

• Mass of AgCl precipitate= Mole × Molar mass
• = 0.05 * 143.5 = 7.16g
• Hence, 7.16 g AgCl will be precipitated out.

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