what is the most soluble salt of the following set?
a) AgCN with Ksp=6.0 x 10^-17
b) Al(OH)3 with Ksp = 1.9x10^-33
c) Fe(OH)3 with Ksp = 2.6 x 10^-39
d) Sn(OH)2 with Ksp = 1.6 x 10^-19
To determine the most soluble salt among the given set, we need to compare the solubility product constants (Ksp) of each salt. The salt with the highest Ksp value will be the most soluble.
a) AgCN with Ksp = 6.0 x 10^-17
b) Al(OH)3 with Ksp = 1.9 x 10^-33
c) Fe(OH)3 with Ksp = 2.6 x 10^-39
d) Sn(OH)2 with Ksp = 1.6 x 10^-19
Comparing the Ksp values, we find that:
- AgCN has the highest Ksp value of 6.0 x 10^-17.
- Sn(OH)2 has a Ksp value of 1.6 x 10^-19.
- Al(OH)3 has a Ksp value of 1.9 x 10^-33.
- Fe(OH)3 has the lowest Ksp value of 2.6 x 10^-39.
Therefore, among the given set, AgCN (Silver Cyanide) is the most soluble salt.
To determine the most soluble salt from the set provided, you need to compare the solubility product constants (Ksp) of each salt. The salt with the highest Ksp value is considered the most soluble.
Let's compare the Ksp values of the salts in the set:
a) AgCN with Ksp = 6.0 x 10^-17
b) Al(OH)3 with Ksp = 1.9 x 10^-33
c) Fe(OH)3 with Ksp = 2.6 x 10^-39
d) Sn(OH)2 with Ksp = 1.6 x 10^-19
Comparing the Ksp values, we can see that:
Ksp of AgCN = 6.0 x 10^-17
Ksp of Al(OH)3 = 1.9 x 10^-33
Ksp of Fe(OH)3 = 2.6 x 10^-39
Ksp of Sn(OH)2 = 1.6 x 10^-19
The highest Ksp value among these salts is for AgCN, which has a Ksp value of 6.0 x 10^-17. Therefore, the most soluble salt from the set is AgCN.
I don't know of any way to do this short of solving three problems. You can eliminate 1 of the Fe/Al hydroxides; i.e., Al(OH)3 is more soluble than Fe(OH)3 because Ksp is larger. However, you may not compare Ksp directly for purposes of determining solublility with salts that are not the same kind; i.e. 1:1 as in AgCN, 1:2 as in Sn(OH)2 and 1:3 as in Al(OH)3.
For AgCN, solublity is sqrt(Ksp)
Can you handle the other two?