If 1 L HCl has a molarity of 0.10 M, what molar concentration of 1 L AgNO 3 is needed for HCl to completely react? How much product (moles and volume) will be formed?

HCl(aq)+ AgNO3(aq) ->AgC(s)+HNO3(aq)

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To determine the molar concentration of AgNO3 needed for HCl to completely react, you need to use stoichiometry. The balanced equation for the reaction is:

HCl(aq) + AgNO3(aq) -> AgC(s) + HNO3(aq)

From the equation, you can see that the stoichiometric ratio between HCl and AgNO3 is 1:1. This means that for every 1 mole of HCl, you need 1 mole of AgNO3 to completely react.

Given that the molarity of HCl is 0.10 M and the volume is 1 L, you can calculate the number of moles of HCl using the formula:

moles = molarity x volume
moles = 0.10 M x 1 L
moles = 0.10 moles

Since the stoichiometric ratio between HCl and AgNO3 is 1:1, you need 0.10 moles of AgNO3 to completely react with 0.10 moles of HCl.

Now, to determine the molar concentration of AgNO3, you need to know the volume of AgNO3 solution required. If the volume of AgNO3 is also 1 L, then the molar concentration of AgNO3 would also be 0.10 M, since the number of moles remains the same.

As for the product formed, the reaction produces AgCl and HNO3. The balanced equation tells us that for every 1 mole of HCl, you will get 1 mole of AgCl and 1 mole HNO3.

So, if you start with 0.10 moles of HCl, you will also produce 0.10 moles of AgCl and 0.10 moles of HNO3. The volume of the product depends on the densities and molar volumes of the substances involved.

In summary:
- To completely react 1 L of 0.10 M HCl, you need 0.10 moles of AgNO3.
- The molar concentration of 1 L AgNO3 needed is 0.10 M.
- The amount of product formed is 0.10 moles of AgCl and 0.10 moles of HNO3, the volume depends on the densities and molar volumes of the substances involved.