Calculate the moles of H+ delivered to each sample based on your experimental data and record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sample and record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sample and record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2 for each sample and record these values in Data Table 1. Molar solubility = moles / Liter . Calculate the K sp for each trial and the average Ksp and record these values in Data Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml .7ml 1.0ml Final HCl Volume in Syringe .7ml .2ml .55ml Volume of HCl Delivered .3ml .5ml .45ml Moles of HCl Delivered Moles of OH- in Sample Moles of Ca2+ in Sample Molar Solubility (M) Calculated Ksp Average Calculated Ksp
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.
Calculate the moles of H+ delivered to each
sample based on your experimental data
and record these values in Data Table 1.
0.1M HCl = 0.1 moles HCl / 1 Liter solution
Calculate the moles of OH- in each sample
and record these values in Data Table 1.
H+ + OH- H2O
Calculate the moles of Ca2+ in each sample
and record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH
. Calculate the molar solubility of Ca(OH)2
for each sample and record these values in
Data Table 1.
Molar solubility = moles / Liter
. Calculate the K
sp
for each trial and the
average Ksp
and record these values in
Data Table 1.
Ksp = [Ca2+][OH-]2
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Sample 1 |
Sample 2 |
Sample 3 |
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Mass of Erlenmeyer Flask |
25.47 |
25.47 |
25.47 |
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Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) |
28.32 |
28.30 |
28.43 |
|
Mass of Calcium Hydroxide Solution |
2.85 |
2.83 |
2.96 |
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Volume of Ca(OH)2 Density = 1.000 g/mL |
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Concentration of HCl (M) |
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Initial HCl Volume in Syringe |
1.0ml |
.7ml |
1.0ml |
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Final HCl Volume in Syringe |
.7ml |
.2ml |
.55ml |
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Volume of HCl Delivered |
.3ml |
.5ml |
.45ml |
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Moles of HCl Delivered |
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Moles of OH- in Sample |
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Moles of Ca2+ in Sample |
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Molar Solubility (M) |
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Calculated Ksp |
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Average Calculated Ksp |
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