The pH and electrical conductivity of four different mixtures were measured: Mixtures Conductivity (Ma) PH a) 0.1 mol L-1 HCl 260 1 b) 0.1 mol L-1 CH3OOH 5 3 c) Mixture made by mixing equal valumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d) Mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 a) Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A is lower than the pH of B. Include relevant equations in your answer. b) Explain why the pH of mixture C is the same as the pH of mixture A. c) Why is the conductivity of mixture C larger than the conductivity of mixture A? d) Why is the pH of mixture D the same as the pH of mixture B? Part B – Determine the final pH for the following two solutions a) Solution A after mixing 500mL 0.2M HCl and 300 mL 0.6M HCl b) Solution B after mixing 400mL 0.3M HCl and 200mL 0.8M NaOH
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.
The pH and electrical conductivity of four different mixtures were measured:
| Mixtures | Conductivity (Ma) | PH |
| a) 0.1 mol L-1 HCl | 260 | 1 |
| b) 0.1 mol L-1 CH3OOH | 5 | 3 |
| c) Mixture made by mixing equal valumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl | 340 | 1 |
| d) Mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO | 80 | 3 |
a) Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A is
lower than the pH of B. Include relevant equations in your answer.
b) Explain why the pH of mixture C is the same as the pH of mixture A.
c) Why is the conductivity of mixture C larger than the conductivity of mixture A?
d) Why is the pH of mixture D the same as the pH of mixture B?
Part B –
Determine the final pH for the following two solutions
a) Solution A after mixing 500mL 0.2M HCl and 300 mL 0.6M HCl
b) Solution B after mixing 400mL 0.3M HCl and 200mL 0.8M NaOH
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
d) Why is the pH of mixture D the same as the pH of mixture B?
by Bartleby ExpertPart B – follow on from the above question?
Determine the final pH for the following two solutions
a) Solution A after mixing 500mL 0.2M HCl and 300 mL 0.6M HCl
b) Solution B after mixing 400mL 0.3M HCl and 200mL 0.8M NaOH
by Bartleby Expert
