1. What volume of 1.00 M HNO2 when diluted to 100.00 mL in a volumetric flask would yield a 0.275 M HNO2 solution? 2. A solution of NaCN has a pH of 9.20. Find the [H] in the solution. Is the solution acidic or basic? 3. A 0.010M solution of the weak acid HA has a pH of 3.80. What is the percent dissociation of HA in the solution? 4. a. Write the hydrolysis reaction that occurs in a solution of NH3. b. Write the hydrolysis reaction that occurs in a solution of NaNO₂. 5. Why is often the case that distilled water has a pH of less than 7 in the lab?
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.
![1. What volume of 1.00 M HNO2 when diluted to 100.00 mL in a volumetric flask would yield a
0.275 M HNO2 solution?
2. A solution of NaCN has a pH of 9.20. Find the [H] in the solution. Is the solution acidic or
basic?
3. A 0.010M solution of the weak acid HA has a pH of 3.80. What is the percent dissociation of
HA in the solution?
4. a. Write the hydrolysis reaction that occurs in a solution of NH3.
b. Write the hydrolysis reaction that occurs in a solution of NaNO₂.
5. Why is often the case that distilled water has a pH of less than 7 in the lab?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2af5a58a-26e3-4baa-9073-1b18b1512b13%2F71361eb9-41fe-4b7e-b9c7-8b04d1886ad5%2Fdfbud3f_processed.jpeg&w=3840&q=75)
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