1. During a titration, it took 35.8mL of 0.10 M Be(OH)₂ to neutralize 65mL of HCl.

1. Write the balanced chemical reaction.
2. How many moles of beryllium hydroxide are needed to neutralize 2 moles of HCl?
3. What is the molarity of the HCl solution?

2. Consider a titration of 0.15M NaOH and 250 mL of 0.10M HBr.

1. What is the pH of the HBr solution before any base is added?
2. What is the pH after 50 mL NaOH is added?
3. What is the pH after 125 mL NaOH is added?
4. What is the pH after 150 mL NaOH is added?
5. Sketch the titration curve. Label the equivalence point on the graph and label the pH value at that point.

An engineer is designing a product in which a copper wire will carry large amounts of electricity. The resistive heating of a 66 g copper wire is expected to add 550 J of heat energy during a 10-minute operating cycle.

By what percentage does the volume increase because of the temperature increase?

(Note: Remember to always use unrounded values in calculations then round final answers to the correct significant figures.)

You may use the following information about copper to answer the question:

specific heat = 0.385 J g^-1 °C^-1

density = 8.94 g/cm³

coefficient thermal expansion = 6.5 µm m^-1 K^-1

Choose an organic compound to describe in depth; do not choose a nonmetal already selected

by another student. Include information on whether it is found in nature, how it can

be synthesized, its physical and chemical properties, and its uses or applications.

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.