Determine the Ksp of an acidic salt through titration. Using a .10M solution of NaOH titrate a saturated 20mL of KHT. Doing the experiment, the following are my numbers. I have seen so many formulas written in so many ways I am now confused. Please help me by showing process. Temperature of room 25 C Molarity of NaOH M Trial 1 Trial 2 Trial 3 Initial grad cyl 10mL 10mL 10mL Final grad cyl 1.1mL 1.4mL .9mL vol NaOH (mL) Used 8.9mL 8.6mL 9.1mL Vol NaOH (L) .0089L .0086L .0091L moles of NaOH mol mol mol moles of HT− mol mol mol Volume of HT− mL mL mL Volume of HT− L L L molarity of HT− M M M molarity of K+ M M M Ksp Average Ksp of KHT (from your experiment) = Average Molar solubility of KHT =
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.
Determine the Ksp of an acidic salt through titration. Using a .10M solution of NaOH titrate a saturated 20mL of KHT. Doing the experiment, the following are my numbers. I have seen so many formulas written in so many ways I am now confused. Please help me by showing process.
|
Temperature of room |
25 C |
|
Molarity of NaOH |
M |
|
|
Trial 1 |
Trial 2 |
Trial 3 |
|
Initial grad cyl |
10mL |
10mL |
10mL |
|
Final grad cyl |
1.1mL |
1.4mL |
.9mL |
|
vol NaOH (mL) Used |
8.9mL |
8.6mL |
9.1mL |
|
Vol NaOH (L) |
.0089L |
.0086L |
.0091L |
|
moles of NaOH |
mol |
mol |
mol |
|
moles of HT− |
mol |
mol |
mol |
|
Volume of HT− |
mL |
mL |
mL |
|
Volume of HT− |
L |
L |
L |
|
molarity of HT− |
M |
M |
M |
|
molarity of K+ |
M |
M |
M |
|
Ksp |
|
|
|
|
Average Ksp of KHT (from your experiment) |
= |
|
Average Molar solubility of KHT |
= |
Step by step
Solved in 5 steps with 4 images
