Question

A 5.00 mL of a salt solution of unknown concentration was mixed with 35.0 mL of 0.523 M AgNO3. The mass of AgCl solid formed was 0.508 g. _ AgNO3(aq) + _ NaCl(aq) → _ AgCl(s) + _ NaNO3(aq) What is the chemical term for the silver chloride solid that is formed?

Answer 1

The chemical term of the reaction

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

Is when appears red brick in the solution indicating the formation of the precipitate

Answer 2

The chemical term in the equation for the precipitate of AgCl(s) is n=3.54*10^-3

Step-by-step explanation:

the quantity of AgCl(s) in moles is:

n = 0.508g / 143.32 g/mol = 3.54*10^-3 mol

to verify it the mass of AgNO3 involved in the reaction should be

n AgNO3 required = n = 3.54*10^-3 mol

the mass of n involved should be higher than n AgNO3

n existing = V*N = 0.523 mol/L * 35*10^-3 L = 18.305*10^-3 mol