Can anyone help me with this question

Question

How much NaCl should be added to 0.35 L of a 0.15 M solution of AgNO3 so that it reacts completely with the silver to form AgCl(s)?
A. 8.8 g
B. 0.0525 g
C. 0.89 mg
D. 3.07 g

Answer 1

Write down the reaction:

NaCl + Ag(+) ---> AgCl + Na(+)

The main thing to note here is that 1 mol of NaCl reacts completely with 1 mol of silver to form the required product.

How many moles of Ag do we have?
(It will be equal to the number of moles of AgNO3, since one mole of silver nitrate contains one mole of silver)

Molarity = (number of moles)/(volume of solution)
(number of moles) = (Molarity) * (volume)
= (0.15) * (0.35)

When you solve this, you will get the number of moles of AgNO3. This will be equal to the number of moles of Ag in the solution, and the number of moles of NaCl to be added.

Given the number of moles of NaCl, can you convert this into the mass required?

Answer 2

3.07 g