I have some problems on solving for K in equilbrium. I need a clear understanding for a test coming up early next week. I would appreciate a complete explanation with the work. Thank you for the help.
1. At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.28. What is the Ksp of the salt at 22 °C?
2. Given that Ka for HCN is 6.2 × 10-10 at 25 °C, what is the value of Kb for CN- at 25 °C?
Given that Kb for NH3 is 1.8 × 10-5 at 25 °C, what is the value of Ka for NH4 at 25 °C?
3. Write the equation for the reaction associated with the Ka2 of sulfuric acid, H2SO4.
Write the equation for the reaction associated with the Kb2 of carbonate, CO32-.
4. At a certain temperature, 0.860 mol of SO3 is placed in a 3.50-L container.
At equilibrium, 0.100 mol of O2 is present. Calculate Kc.
The expert finds the K values.
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