Determine the molar concentration of each ion present in the solutions that result from each of the following mixtures: (Disregard the concentration of H* and OH' from water and assume that volumes are additive.) (a) 55.6 mL of 0.25 MHCI and 69.8 mL of 1.73 M HCI 0.25 1.73 0.53 MH* (b) 111 mL of 0.85 M CaCl2 and 111 mL of 0.21 M CaCl₂ 1.06 MCI мСа2+ MCI (c) 37.0 mL of 0.316 M NaOH and 21.9 mL of 0.226 MHCI M Na MCI MH* MOH' (d) 11.9 mL of 0.671 M H₂SO4 and 22.3 mL of 0.146 M NaOH M Na* M504²- MH* MOH
Ionic Equilibrium
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.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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For d, the answer you got for the second box, 0.1858 is wrong.
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