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10ml of an HCl solution gave 0.1435g AgCl when treated with excess of AgNO3. The normality of the resulting solution is a)0.1 b)3 c)0.3 d)0.2 can u explain the answer plz?
Most Upvoted Answer
10ml of an HCl solution gave 0.1435g AgCl when treated with excess of ...


Given Data:
- Volume of HCl solution = 10ml
- Mass of AgCl formed = 0.1435g

Calculating Normality:
1. Calculate the moles of AgCl formed:
- The molar mass of AgCl = 107.87 (Ag: 107.87, Cl: 35.45)
- Moles of AgCl = Mass / Molar mass = 0.1435g / 143.32g/mol ≈ 1 x 10^-3 mol

2. Since AgNO3 is in excess, the moles of Cl- ions in HCl are equal to the moles of AgCl formed:
- Moles of Cl- ions = 1 x 10^-3 mol

3. Normality is defined as the number of equivalents per liter of solution:
- Normality = (Moles of Cl- ions / Volume of solution in liters) x n factor
- Since HCl dissociates into 1 H+ ion and 1 Cl- ion, the n factor is 1 for HCl
- Volume of solution in liters = 10ml = 10 x 10^-3 L
- Normality = (1 x 10^-3 mol / 10 x 10^-3 L) x 1 = 0.1 N

Answer:
The normality of the resulting solution is a) 0.1 N.
Community Answer
10ml of an HCl solution gave 0.1435g AgCl when treated with excess of ...
N =w*1000/ew*v
0.1435*1000/143.5*10
=0.1
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10ml of an HCl solution gave 0.1435g AgCl when treated with excess of AgNO3. The normality of the resulting solution is a)0.1 b)3 c)0.3 d)0.2 can u explain the answer plz?
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