36.

What is the net ionic equation for the acid–base reaction of hydrobromic acid with sodium hydroxide?

A)

NaOH(aq) + HBr(aq) → H2O(l) + NaBr(aq)

B)

Na+(aq) + –OH(aq) + H+(aq) + Br–(aq) → H2O(l) + Na+(aq) + Br–(aq)

C)

Na+(aq) + –OH(aq) + H+(aq) + Br–(aq) → H+(aq) + –OH(aq) + Na+(aq) + Br–(aq)

D)

–OH(aq) + H+(aq) → H2O(l)

Which salt forms a basic solution when dissolved in water?

A) KCl B) NH4Br C) LiNO3 D) Na3PO4

44.

A solution containing a low concentration HCl is a weak acid.

A) True B) False

Mole fraction of n2

Mole fraction of o2

Answers given without the use of the given temperatures, pressures, and densities are wrong and have already been tried.

A gaseous mixture consists of 76.0 mole percent N₂ and 24.0 mole percent O₂ (the approximate composition of air). Suppose water is saturated with the gas mixture at 25°C and 1.00 atm total pressure, and then the gas is expelled from the water by heating. What is the composition in mole fractions of the gas mixture that is expelled? The solubilities of N₂ and O₂at 25°C and 1.00 atm are 0.0175 g/L H₂O and 0.0393 g/L H₂O, respectively.

(b) A vessel separated into two parts, A and B, by a bilayer lipid membrane contained an aqueous solution of KCl with concentration 0.01 mol L-1 in part A and 0.1 mol L-1 in part B and of NaCl with concentration 0.1 mol L-1 in part A and 0.01 mol L-1 in part B. The membrane included potassium channels, which made it permeable for K+ ions. The temperature of the vessel was kept at 30 o C. (i) Calculate the electrical potential between the two sides of the membrane (membrane potential). (ii) Explain how an increase of temperature and an addition of NaCl to part B will affect the membrane potential. Assume ideal behaviour of the solutions.

(a) A vessel is separated into two parts, A and B, by a bilayer lipid membrane containing Na+ channels. Part A holds an aqueous solution of NaCl with concentration 0.15 mol L-1 and of disaccharide sucrose with concentration 0.01 mol L-1 . Part B holds an aqueous solution of NaCl with concentration 0.015 mol L-1 . Calculate the electrical potential between the two sides of the membrane at 30 oC and at 50 oC. Neglect the effect of temperature on the molarity of the solutions. Assume that the membrane is not permeable for glucose and for Cl ions.

Calculate the molarity of each of the following solutions:

(a) 0.195 g of cholesterol, C27H46O, in 0.100 L of serum, the average concentration of cholesterol in human serum

(b) 4.25 g of NH3 in 0.500 L of solution, the concentration of NH3 in household ammonia

(c) 1.49 kg of isopropyl alcohol, C3H7OH, in 2.50 L of solution, the concentration of isopropyl alcohol in rubbing alcohol

(d) 0.029 g of I2 in 0.100 L of solution, the solubility of I2 in water at 20 °C

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(a) A vessel is separated into two parts, A and B, by a bilayer lipid membrane containing Na+ channels. Part A holds an aqueous solution of NaCl with concentration 0.15 mol L-1 and of disaccharide sucrose with concentration 0.01 mol L-1 . Part B holds an aqueous solution of NaCl with concentration 0.015 mol L-1 . Calculate the electrical potential between the two sides of the membrane at 30 oC and at 50 oC. Neglect the effect of temperature on the molarity of the solutions. Assume that the membrane is not permeable for glucose and for Cl ions.

The relative energies of the eg and t2g orbitals are different for octahedral and tetrahedral complexes.

a. Draw both diagrams with labeled d orbitals (which d orbitals are which)

b. Explain why the different geometries have different orbital diagrams.

c. Why is the delta T always smaller than delta O?

Consider the four coordinate complexes [FeCl4]2-, [Ni(CN)4]2- or [AuCl4]-.

a. Which of these complexes do you expect to be square planar? Why?

b. Explain why this geometry is preferred using a crystal field splitting diagram and words.  

Draw and label crystal field splitting diagrams (including orbital labels) for the following complexes. Calculate he ligand field stabilization energy as a factor of Delta for each complex.

a. [Co(OH2)6]2+

b. [RH(NH3)6]2+

c. [NiCl4]2-

Calculate the freezing point and melting point of a solution containing 10.0 g of naphthalene (C₁₀H₈) in 100.0 mL of benzene. Benzene has a density of 0.877 g/cm³

Determine the molarity of each of the following solutions:

(d) 2.76 kg of CuSO4?5H2O in 1.45 L of solution

(e) 0.005653 mol of Br2 in 10.00 mL of solution

(f) 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solution

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Write the chemical formula or name the following complexes and draw AND LABEL all possible isomers (ignore counter-ions in drawing).

a. [CoCl3(OH2)3]-

b. [MoCl(NH3)5]SO4

c. diaquotetracarbonylruthenium(III)

d. diamminedichloroplatinum(II)

Compare the energy available from the combustion of a given volume of methane and the same volume of hydrogen at the same temperature and pressure. (Standard enthalpy of formation of methane is -75 kJ/mol)

Convert the following equivalents to masses/volumes (g or mL):
1. 1.5 equivalents of KOH
2. 1.4 equivalents of RCO3H
3. 1.2 equivalents of NaOH
4. 0.2 equivalents of NaOH
5. 3.5 equivalents of ethyl bromide

1. Use information in the balanced chemical formula below to answer the next 4 questions

   C2H6                    +       7   F2             →           2 CF4             +         6 HF

mw = 30.06 amu                           mw = 37.99 amu                           mw = 88.00 amu               mw=20.00 amu         

a) How many moles of C2H6 would be consumed when reacted with 9.24 moles of F2?

b) If you consume 7.50 moles of F2, how many grams of HF are produced?

c) If 10.32 g of HF are generated, what mass of C2H6 was utilized as starting material?

d) What is the number of molecules of F2 required to completely consume 25.0 g of C2H6?