A student wishes to make a buffer that has a pH of 4.65. The student has HNO2 and NaNO2. Nitrous Acid (HNO2) has a pKa of 3.40 The student makes 100.0 mL of a 0.100 M solution of HNO2. What mass (in grams) of NaNO2 should the student add to the solution to make a buffer that buffers at a pH of 4.25. (Hint: use the Henderson-Hasselbalch equation to find the molarity, then find the number of moles required to achieve that concentration in 100.0 mL of solution.)
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.
A student wishes to make a buffer that has a pH of 4.65. The student has HNO2 and NaNO2. Nitrous Acid (HNO2) has a pKa of 3.40
The student makes 100.0 mL of a 0.100 M solution of HNO2. What mass (in grams) of NaNO2 should the student add to the solution to make a buffer that buffers at a pH of 4.25. (Hint: use the Henderson-Hasselbalch equation to find the molarity, then find the number of moles required to achieve that concentration in 100.0 mL of solution.)
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