Calculate the mass of AgCl formed, and the concentration of silver ion remaining in solution, when 10.0g of solid AgNO3 is added to 50.mL of 1.0x10-2 Assume there is no volume change upon addition of the solid.

The given question is incomplete. The complete question is

Calculate the mass of AgCl formed, and the concentration of silver ion remaining in solution, when 10.0g of solid is added to 50.mL of NaCl. Assume there is no volume change upon addition of the solid.

a) mass of AgCl formed = 0.072 g

b) Concentration of silver ion remaining in solution

Explanation:

To calculate the moles :

According to stoichiometry :

1 mole of require = 1 mole of

Thus 0.0005 moles of will require= of

Thus is the limiting reagent as it limits the formation of product and is the excess reagent.

As 1 mole  of NaCl give = 1 mole of AgCl

Thus 0.0005 moles of NaCl give =  of

Mass of

moles of AgCl left = (0.059-0.0005) = 0.0585

Concentration of left in solution =

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.

i think its 100

i hope this !