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1 Jul 2020

Two solutions of and were mixed in a flask. The volume of the original solutions are , respectively. After mixing, a solid was formed in the mixture. What is the identity of the solid and much did the solid weigh?

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Solve problems involving solutions and mixtures

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For this experiment, you will need the folloing:

0.1% bromothymol blue in 20% Ethanol: about 10mL

0.2M salt water: about 150mL

0.1M NaH2PO4: about 80mL

0.1M NaHPO4 :About 80mL

1M HCL: in a drop bottle

1M NaOH: In a dropper

Lable 3 Volumetric flasks 1,2, and 3. Add the amounts found below and dilute to exactly 50mL.

Flask1: 1.0mL bromothymol blue 30.0mL H2PO4^-1 10mL HPO4^-2

Flask2: 1.0mL bromothymol blue 20.0mL H2PO4^-1 20.0mL HPO4^-2

Flask3: 1.0mL bromothymol blue 10.0mL H2PO4^-1 30.0mL HPO4^-2

Make two more flasks, one with a strongly acidic mixture (25mL saltwater, 4 drops of HCL, then dilute to 50mL of salt water) and a strongly basic solution (25mL saltwater, 4 drops of NaOH, then dilute to 50mL of salt water).

Record the pH and absorbance. Don't measure pH for strong acid/base solutions.

DATA:

Type	pH	A450	A615	color
Strong acid	-	0.564	0.000	Yellow
#1	6.36	.0449	0.118	Lime Green
#2	6.71	0.490	0.395	Dark Green
#3	7.67	0.254	.1.186	Dark Blue
Strong Base	-	0.226	1.323	Blue

This is where I have no idea what to do with my data.

Flask#	[H3O^+]	Ka (Method 1)	Ka (method 2)
#1	M
#2	M
#3	M

Average Ka (method 1)=_____ pKa=_______

Average Ka (method 2)=______ pKa=_____

I dont know how to find the Molarity of H3O^+.

I do have the equations for Method 1 and Method 2.

Method 1:

K_a= [H₃O⁺] (A₆₁₅^Buffer * A₄₅₀^Acid/ A₄₅₀^Buffer *A₆₁₅^Base)

Method 2:

K_a= [H₃O⁺] (A₆₁₅^Buffer * A₄₅₀^Acid/ ( A₄₅₀^Buffer *A₆₁₅^Base) - (A₆₁₅^Buffer* A₄₅₀^Base)

Then there is a back with questions but I can't do them unitl I figure this out. please let me know if you need anymore information

The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of Copper (II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of Potassium hydroxide.

Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed.
Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.

turquoisecheetah392

Consider two solutions, the first being 50.0 mL of 1.00 M CuSO₄ and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 to 27.7 °C. (a) Before mixing, how many grams of Cu are present in the solution of CuSO₄? (b) Predict the identity of the precipitate in the reaction. (c) Write complete and net ionic equations for the reaction that occurs when the two solutions are mixed. (d) From the calorimetric data, calculate ∆H for the reaction that occurs on mixing. Assume that the calorimeter absorbs only a negligible quantity of heat, that the total volume of the solution is 100.0 mL, and that the specific heat and density of the solution after mixing are the same as those of pure water.