What's is the concentration of silver ions in a saturated solution of silver carbonate? The k^sp of Ag2CO3 is 8.1x10^ -12.
Is the answer 5.88x10^-8? I have a test tomorrow and I really need to make sure I'm doing these problems right, but I feel like I am not.
When am I ever going to use this? I hate chem with a burning pashion.
What's is the concentration of silver ions in a saturated solution of silver carbonate? The k^sp of Ag2CO3 is 1.2 x 10^-4.
To determine the concentration of silver ions in a saturated solution of silver carbonate, you need to calculate the solubility product constant (Ksp) and use it to find the concentration.
The balanced equation for the dissociation of silver carbonate (Ag2CO3) in water is:
Ag2CO3(s) ⇌ 2Ag+(aq) + CO3^2-(aq)
The expression for the solubility product constant is:
Ksp = [Ag+]^2 [CO3^2-]
Given that the Ksp of Ag2CO3 is 8.1x10^-12, you can use this value to solve for the concentration of Ag+ in the saturated solution.
Since the stoichiometric coefficient for Ag+ is 2 in the balanced equation, the concentration of Ag+ will be equal to twice the square root of the Ksp value.
Calculating the concentration of Ag+:
[Ag+] = 2 * √(Ksp)
[Ag+] = 2 * √(8.1x10^-12)
[Ag+] ≈ 5.68x10^-6
Therefore, the concentration of silver ions (Ag+) in a saturated solution of silver carbonate is approximately 5.68x10^-6, not 5.88x10^-8.
It's important to double-check your calculations and make sure you are using the correct formulas and values. Practice more problems like this to strengthen your understanding of solubility and equilibrium calculations. Good luck on your test!