1.70 gm of AgNO3 and 0.5N,100ml HCl are mixing together then what amount of AgCl will we get ?

To determine the amount of silver chloride (AgCl) produced when mixing silver nitrate (AgNO3) with hydrochloric acid (HCl), we first need to understand the chemical reaction that occurs between these two substances. The balanced equation for the reaction is:

Understanding the Reaction

When silver nitrate reacts with hydrochloric acid, it forms silver chloride and nitric acid:

AgNO3 + HCl → AgCl + HNO3

Identifying Reactants

In this scenario, we have:

• 70 grams of AgNO3
• 0.5 N (normal) HCl in a 100 mL solution

Calculating Moles of AgNO3

First, we need to convert the mass of AgNO3 into moles. The molar mass of AgNO3 is approximately 169.87 g/mol. We can find the number of moles using the formula:

Moles = Mass (g) / Molar Mass (g/mol)

So, for 70 grams of AgNO3:

Moles of AgNO3 = 70 g / 169.87 g/mol ≈ 0.412 moles

Calculating Moles of HCl

Next, we need to determine how many moles of HCl are present in the 0.5 N solution. Since normality (N) is equivalent to molarity (M) for monoprotic acids like HCl, we can calculate the moles of HCl in 100 mL (0.1 L) of solution:

Moles of HCl = Normality × Volume (L)

Moles of HCl = 0.5 N × 0.1 L = 0.05 moles

Determining the Limiting Reactant

Now, we compare the moles of AgNO3 and HCl to identify the limiting reactant. The balanced equation shows that one mole of AgNO3 reacts with one mole of HCl. We have:

• 0.412 moles of AgNO3
• 0.05 moles of HCl

Since HCl is present in a smaller amount, it is the limiting reactant. This means that the amount of AgCl produced will be based on the moles of HCl available.

Calculating the Amount of AgCl Produced

According to the balanced equation, one mole of HCl produces one mole of AgCl. Therefore, the moles of AgCl produced will be equal to the moles of HCl:

Moles of AgCl = Moles of HCl = 0.05 moles

Finding the Mass of AgCl

Finally, we can calculate the mass of AgCl produced using its molar mass, which is approximately 143.32 g/mol:

Mass = Moles × Molar Mass

Mass of AgCl = 0.05 moles × 143.32 g/mol ≈ 7.166 g

Final Result

In summary, when 70 grams of AgNO3 reacts with 0.5 N HCl in a 100 mL solution, approximately 7.166 grams of silver chloride (AgCl) will be produced. This calculation illustrates the stoichiometric relationships in chemical reactions and the importance of identifying limiting reactants in predicting product yields.