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 solve this problem, we need to determine the molar concentration of AgNO3 needed to completely react with 1 L of 0.10 M HCl. We also need to find the amount of product (AgCl) that will be formed in terms of moles and volume.
First, let's establish the balanced chemical equation for the reaction:
HCl(aq) + AgNO3(aq) -> AgCl(s) + HNO3(aq)
The stoichiometry of the equation tells us that 1 mole of HCl reacts with 1 mole of AgNO3 to produce 1 mole of AgCl.
Given that the molarity of HCl is 0.10 M, we know that there are 0.10 moles of HCl present in 1 L of solution.
Since the stoichiometry of the reaction is 1:1, we need an equal number of moles of AgNO3 to completely react with the HCl.
Therefore, the molar concentration of AgNO3 needed to react with 0.10 moles of HCl is also 0.10 M.
As for the amount of product formed, we can conclude that 1 mole of AgCl will be produced since the stoichiometry of the balanced equation is 1:1.
To find the volume of the product, we need to consider the volume of the solution. Since the solutions are both 1 L, the volume of the product will also be 1 L.
In summary:
- The molar concentration of the required AgNO3 solution is 0.10 M.
- 1 mole of AgCl product will be formed.
- The volume of the product (AgCl) will be 1 L.