The pKa of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton. 1. Suppose you dissolve 0.200 mol of MOPS in 1.00 Lof water. Calculate the pH of the solution. е. g. Use the pKa of MOPS to determine the ratio [A]/[HA] at pH 6.95. h. If you have 0.200 mol of MOPS dissolved in water, would you add NaOH or HCl to reach a pH of 6.95? And how many moles of the acid or base would you need to add? If you use a 100 mM MOPS buffer at pH 6.95 for a biochemical reaction which produces a maximum of 10 mM H*, which pH would you predict at the end of the reaction? i.
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.
![he pka of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton.
f.
Suppose you dissolve 0.200 mol of MOPS in 1.00 L of water. Calculate the pH of the
solution.
g.
Use the pKa of MOPS to determine the ratio [A]/[HA] at pH 6.95.
h. If you have 0.200 mol of MOPS dissolved in water, would you add NaOH or HCI to reach
a pH of 6.95? And how many moles of the acid or base would you need to add?
If you use a 100 mM MOPS buffer at pH 6.95 for a biochemical reaction which produces
a maximum of 10 mM H*, which pH would you predict at the end of the reaction?
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