A student has a mixture of salt (NaCl) and sugar (C12H22O11). To determine the percent composition, the student measures out 5.84 g of the mixture and dissolves the sample in 100.0 mL of water. The student knows aqueous NaCl will react with aqueous silver nitrate (AgNO3) to form solid silver chloride (AgCl). The student determines the sugar will not react with silver nitrate. Write a balanced net ionic equation for the reaction of NaCl with AgNO3. How many mL of 1.0 M AgNO3 will be required to precipitate 5.84 g of AgCl

1. Net ionic equation:

2. Volume of 1.0M AgNO₃

Explanation:

1. Net ionic equation for the reaction of NaCl with AgNO₃.

i) Molecular equation:

It is important to show the phases:

ii) Dissociation reactions:

Determine the ions formed:

iii) Total ionic equation:

Substitute the aqueous compounds with the ions determined above:

iv) Net ionic equation

Remove the spectator ions:

2.  How many mL of 1.0 M AgNO₃ will be required to precipitate 5.84 g of AgCl

i) Determine the number of moles of AgNO₃

The reaction is 1 to 1: 1 mole of AgNO₃ produces 1 mol of AgCl

The number of moles of AgCl is determined using the molar mass:

ii) Determine the volume of AgNO₃

Round to two significant figures: 41ml ← answer

i believe the answer is a.

it is the most commonly accepted one