mix 10ml NaBr 3.i000M wth 10ml water & 10ml AgNo3 3.3.1000M KspAgBr=5.25.1000 .what is the situation at equilibrium
You need to read your post. A concn of 3.3.1000 doesn't mean anything to me. Nor does 3.i000
To determine the situation at equilibrium, we need to consider the reaction and calculate the concentrations of the ions involved.
The given reaction is:
NaBr (aq) + AgNO3 (aq) ⟶ AgBr (s) + NaNO3 (aq)
First, let's calculate the moles of each reactant:
moles of NaBr = concentration (M) × volume (L) = 3.1000 × 0.010 L = 0.031 moles
moles of AgNO3 = concentration (M) × volume (L) = 3.31000 × 0.010 L = 0.033 moles
Note: The water is not involved in the reaction and does not affect the equilibrium.
Next, let's determine the limiting reactant. Since both reactants have equal moles, they will fully react.
The balanced equation shows that 1 mole of NaBr reacts with 1 mole of AgNO3 to produce 1 mole of AgBr.
Therefore, based on stoichiometry, the moles of AgBr produced will be equal to the moles of NaBr (0.031 moles).
Now, let's calculate the concentration of Ag+ and Br- ions in the saturated solution at equilibrium:
Volume of the final solution = volume of NaBr + volume of AgNO3
= 0.010 L + 0.010 L = 0.020 L
Concentration of Ag+ ions = moles of AgBr / volume of solution (L)
= 0.031 moles / 0.020 L
= 1.550 M
Concentration of Br- ions = moles of AgBr / volume of solution (L)
= 0.031 moles / 0.020 L
= 1.550 M
Since the Ksp value for AgBr is given as 5.251000, we can compare the product of the ion concentrations with the value of Ksp to assess the situation at equilibrium.
Ksp = [Ag+][Br-] = (1.550 M)(1.550 M) = 2.4025
Since the calculated value of the product of the ion concentrations (2.4025) is less than the Ksp value (5.251000), the solution is unsaturated. This means that more AgBr can dissolve, and the reaction has not reached equilibrium.
In summary, at the given concentrations of NaBr and AgNO3, the solution is unsaturated, and more AgBr can dissolve.