The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample. :math> Ag + ( a q ) + Cl + ( a q ) → AgCl ( s ) ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample. :math> Ag + ( a q ) + Cl + ( a q ) → AgCl ( s ) ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
Solution Summary: The author explains the process of using chemical equation to calculate the relative masses of reactants and products involved in a reaction is called stoichiometry.
The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample.
:math>
Ag
+
(
a
q
)
+
Cl
+
(
a
q
)
→
AgCl
(
s
)
ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
Le Châtelier’s Principle is described in terms of adding/removing reactants or products. While it is easy to add reactants/products, describe how you were able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for:
The following reaction is examined:HSO4¯ (aq) + H2O (l) ⇌ SO42¯ (aq) + H3O+ (aq) Obtain about 5 mL (one small test tube) of “NaHSO4 solution” and “Na2SO4 solution” in two appropriately labeled test tubes. In a well plate, take 10 drops of NaHSO4 into wells A1, A2 and A3, and 20 drops to wells A4 and A5 using a pipet. Add 1 drop of Thymol Blue indicator solution to wells A1 to A5. Thymol Blue is red in very acidic solution, and changes from red to yellow between pH 1.2-2.8. Add one drop of Na2SO4 to well A1. Continue to add drops of Na2SO4 to well A1 until you see a color change, making sure to mix the solution after the addition of each drop (do not use the pipet tip to mix the…
Express the reverse equilibrium constant for the following reaction
6CH3Cl (g) + 3Cl2 (g) -> 6CH2Cl2 (g) + 3 H2 (g)
PH of diluted calcium hydroxide=7.01
1.) Hydronium ion concentration in dilute solution,M?
2.)Hydroxide ion concentration in diluted solution, M?
M1 V1= M2 V2 V1=100mL V2=5mL saturated solution M1=#2
Hydroxide in concentration in saturated solution,M?
Calculate solubility product of calcium hydroxide
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