Calculate [OH − ], pOH, and pH for each of the following. (Assume that all solutions are at 25°C.) (a) 0.00013 M Ca(OH)2 [OH − ]
2.6*10^Calculate [OH− ], pOH, and pH for (a) 0.00013 M Ca(OH)2 (b) a solution containing 29 g of RbOH per liter (c) a solution containing 150 g of LiOH per liter
1 answer:
Answer:
See image attached
Explanation:
The hydroxide ion concentration can easily be calculated from the concentration of the metal hydroxide solutions given as shown in the solution attached. The pH can now be obtained from there using pH+pOH=14. The pH value is always greater than the the pOH value as shown in the solution to the problems attached.
Question (c) contains incorrect data that cannot be used to calculate the required parameters.
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<u>Answer:</u> The equilibrium concentration of is 1.285 M.
<u>Explanation:</u>
The chemical equation for the decomposition of phosphorus pentachloride follows:
The expression for equilibrium constant is given as:
We are given:
The concentration of solid substances are taken to be 1. Thus, they do not appear in the equilibrium constant expression.
Putting values in above equation, we get:
Hence, the equilibrium concentration of is 1.285 M.