Question

How many grams of Silver Nitrate must be added to the solution to completely react with Sodium Chloride according to the reaction below:

NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)

Answer 1

Answer:

5.81g of AgNO₃ must be added

Explanation:

The solution contains 2.00g of sodium chloride.

Based on the reaction, 1 mole of NaCl reacts per mole of AgNO₃. To solve this question, we need to find the moles of NaCl in 2.00g and, these moles = Moles of AgNO₃ that must be added:

moles NaCl = Moles AgNO₃-Molar mass: 58.44g/mol:

2.00g * (1mol / 58.44g) = 0.0342 moles NaCl = Moles AgNO₃

Mass AgNO₃ -Molar mass: 169.87g/mol-:

0.0342 moles * (169.87g / mol) =

5.81g of AgNO₃ must be added

Answer 2

The quantity of $AgNO_{3}$ required to be added to the solution in order to allow it to entirely react with Sodium Chloride as per the reaction provided would be:

- $5.81g$ of $AgNO_{3}$

Given that,

The amount of NaCl in the solution = 2g

As we know,

NaCl's 1 mole would react with $AgNO_{3}$'s every mole.

To find,

The quantity of $AgNO_{3}$ required to be added to the solution for complete reaction = ?

We will determine the number of moles in 2g of NaCl which would be the number to be added to the solution.

So,

NaCl moles = Moles $AgNO_{3}$ - Molar mass

$= 58.44g/mol$

Now,

$AgNO_{3}$ moles $= 2g$ × $(1mol / 58.44g)$

$= 0.0342$ moles NaCl = Moles of  $AgNO_{3}$

∵ Mass of  $AgNO_{3}$  - Molar mass

=  $5.81g$ of $AgNO_{3}$  

Thus,  $5.81g$ of $AgNO_{3}$ is the correct answer.

Learn more about 'Reaction' here:

brainly.com/question/13693578