Calculate the mass of NaCl that must be added to completely react with 1.50 L of a 0.150 M AgNO3 solution according to the reaction below: NaCl (aq) + AgNO3 (aq) → AgCl (s) + NaNO3 (aq)

Explanation:

Hello,

In this case, since the reaction is:

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

And it is properly balanced, given 1.50 L of 0.150-M AgNO3, the first step is to compute the moles of reacting silver nitrate as follows given its volume and concentration:

Next, by applying stoihiometry, given the 1:1 mole ratio between silver nitrate and sodium chloride, we compute the mass of NaCl by also using its molar mass (58.45 g/mol):

Regards.

sry but any answer choices