Calculate [OH -] and pH for each of the following solutions. (a) 0.0036 M RbOH [OH-] = M pH = (b) 0.0549 g of KOH in 530.0 mL of solution [OH -] = M pH =
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Calculate [OH -] and pH for each of the following solutions.
(a) 0.0036 M RbOH
| [OH-] = M | pH = |
(b) 0.0549 g of KOH in 530.0 mL of solution
| [OH -] = M | pH = |
(c) 33.1 mL of 0.00392 M Ba(OH)2 diluted to 500 mL
| [OH -] = M | pH = |
(d) A solution formed by mixing 23.0 mL of 0.000370 M Ba(OH)2 with 80.0 mL of 7.8 x 10-3 M RbOH
| [OH -] = M | pH = |
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