Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate all of the Ca2+ ions as the insoluble phosphate (310.2 g/mol). If 4.51 g calcium phosphate is produced, what is the Ca2+ concentration in the calcium chloride solution in g/L?

Put the elements 14 N, 16 O, and 40Ar in order of increasing nuclear stability and justify your answer mathematically.

please show all work, units, and equations!

Two 20.0 g ice cubes at −12.0 ∘C are placed into 255 gof water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts.

At a certain temperature, 0.860 mol of SO3 is placed in a 1.50-L container. At equilibrium, 0.100 mol of O2 is present. Calculate Kc.

The data in the table below were obtained for the reaction: 2ClO2(aq) + 2OH-(aq) ---> ClO3-(aq) + ClO2-(aq) + H2O(l) Experiment number [ClO2](M) [OH-](M) Initial Rate (M/s)

1 .020 .030 .00276

2 .060 .030 .0248

3 .020 .090 .00828

a. What is the order of the reaction with respect to ClO2?

b. What is the order of the reaction with the respect to OH-?

c. What is the overall order of the reaction?

d. What is the magnitude of the rate constant for the reaction?

What is the coordination number for each of the following complexes or compounds?

1. [Co(NH3)4(H2O)2]3+[Co(NH3)4(H2O)2]3+
2. [Mg(EDTA)]2−[Mg(EDTA)]2−
3. [Cu(NH3)4]2+[Cu(NH3)4]2+
4. [Ag(NH3)2]NO3[Ag(NH3)2]NO3

Enter the coordination numbers, in the order that the complexes are listed, as four integers separated by commas (e.g., 1,2,3,4).

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Part B

What is the charge on each of the following complex ions?

1. hexaaquamanganese(II), [Mn(H2O)6]?[Mn(H2O)6]?
2. tris(carbonato)cobaltate(III), [Co(CO3)3]?[Co(CO3)3]?
3. amminepentabromoplatinate(IV), [Pt(NH3)Br5]?[Pt(NH3)Br5]?

Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).

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Part C

What is the oxidation number of the central metal ion in each of the following complexes or compounds?

1. [NiCl2Br2]2−[NiCl2Br2]2−
2. [Cr(H2O)2(NH3)4]3+[Cr(H2O)2(NH3)4]3+
3. Na[Ag(CN)2]Na[Ag(CN)2]

Express the oxidation numbers numerically, in the order that the complexes are listed, separated by commas. For a nonzero oxidation number, be sure to include the sign (e.g., +1,-2,+3).

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In glucose, which carbon is the anomeric carbon?

Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water.

what is the mechanism through which water activity prevents microbial proliferation?

Question 5a

1. Oxygen gas dissolves in lake water. (This is how fish get the oxygen they need to survive.) What happens to the solubility of oxygen gas when it is cold outside? Why does this happen?

   Chose from the options below. More than one answer could be correct.

   	1.	The solubility does not change.
   	2.	The solubility increases.
   	3.	The solubility decreases.
   	4.	In general, the solubility of gas solutes in liquid solvents increases as temperature decreases.
   	5.	In general, the solubility of gas solutes in liquid solvents decreases as temperature decreases.
   	6.	In general, the solubility of gas solutes in liquid solvents increases as the pressure of the gas above the liquid increases.
   	7.	In general, the solubility of gas solutes in liquid solvents increases as the pressure of the gas above the liquid decreases.
   	8.	In general, the solubility of solid solutes in liquid solvents increases as the temperature increases.
   	9.	In general, the solubility of solid solutes in liquid solvents increases as the temperature decreases.

0.8 points

Question 5b

1. Why does your pop lose it's fizz over time after the pop bottle (or can) has been opened?

   Chose from the options below. More than one answer could be correct.

   	1.	The solubility does not change.
   	2.	The solubility increases.
   	3.	The solubility decreases.
   	4.	In general, the solubility of gas solutes in liquid solvents increases as temperature decreases.
   	5.	In general, the solubility of gas solutes in liquid solvents decreases as temperature decreases.
   	6.	In general, the solubility of gas solutes in liquid solvents increases as the gas pressure above the liquid increases.
   	7.	In general, the solubility of gas solutes in liquid solvents decreases as the gas pressure above the liquid increases.
   	8.	In general, the solubility of solid solutes in liquid solvents increases as temperature increases.
   	9.	In general, the solubility of solid solutes in liquid solvents increases as temperature decreases.

PLEASE ANSWER ALL 4 THANK YOU VERY MUCH!!!!

1. How was the Periodic Table originally organized? Explain the current organization of the Periodic Table and why it is a more accurate layout of the elements.

2. What is the difference between groups and periods? What are the common names for groups IA, IIA, VIIA, VIIIA?

3. Why were elements in group 18, VIIIA, formerly known as inert gases? How is the current name of “noble gases” more appropriate? Provide examples of involved elements.

4. Hydrogen can belong to two groups on the Periodic Table, what are they? Which group do you believe hydrogen fits best in? Explain why.

A 0.100 g sample of an organic compound of an organic acid contains C, H, and O was combusted to determine the empirical formula. The combustion produced 0.2921 grams of CO2 and 0.0951 grams of H2O. Determine the number of moles of carbon in the compound, the number of moles of hydrogen in the compound, the number of grams of carbon, the number of grams of hydrogen, the number of grams oxygen as well as the empirical formula. The molecular weight of the compound was found to be 660 grams per mole, determine the molecular formula.

A gas with 65% hydrogen exits a reactor at 2310 psia and 700°F. Select an appropriate material for the piping at the exit of the reactor. (Hint: Find a good version of the Nielson Curves).