1.Briefly explain four colligative properties. Your explanation should contain the following:

a)definition of property

b)does it increase or decrease with concentration

c)what mathematical equation links the property to concentration

d)At least one example of natural applications of the property

Which of the following anions act as weak bases in solution? Check all that apply.

Br−

NO2−

CN−

Cl−

11. A similar analysis was performed for the same exchangeable cations. However, this time the results were reported as mg of the cation per kg of soil as follows: Na = 350 mg/kg K = 1000 mg/kg Ca = 2000 mg/kg Mg = 1000 mg/kg Calculate the CEC (5 pts) Please show your work and do not forget the units

1- what is advantage does pulsed field gradient electrophoresis in gels have over conventional slab gel electrophoresis ? 2- what samples uniquely are suited for this technique and why? 3- discuss the motivation and resistance to adopting new , faster methods of gel electrophoresis that are in capillaries and not on slabs? please give me also refrences

13.A student mixes 100.0 mL of 0.500 M AgNO₃ with 100.0 mL of 0.500 M CaCl₂.

a.Write the balanced molecular equation for the reaction.

b.Write the net ionic equation for the reaction.

c.How many grams of precipitate will form?

d.What is the concentration of Ag⁺, NO₃^‒, Ca²⁺, and Cl^‒ in the final solution (assume volumes are additive).

1) Calculate how many moles of NH3 form when each quantity of reactant completely reacts according to the equation: 3N2H4(l)→4NH3(g)+N2(g)

A) 35.3 g N2H4 - Express your answer using three significant figures.

B) 14.9 kg N2H4 - Express your answer using three significant figures.

2) For each reaction, calculate the mass of the product that forms when 12.5 g of the reactant in red completely reacts. Assume that there is more than enough of the other reactant.

a) 2K(s)+Cl2(g)→2KCl(s) b) 2K(s)+Br2(l)→2KBr(s) c) 4Cr(s)+3O2(g)→2Cr2O3(s) d) 2Sr(s)+O2(g)→2SrO(s)

3) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3NO2(g)+H2O(l)→2HNO3(l)+NO(g)

Suppose that 3.7 mol NO2 and 1.2 mol H2O combine and react completely. Which reactant is in excess? Express your answer as a chemical formula.

4) Calculate the molarity of each of the following solutions:

A) 0.19 mol of LiNO3 in 5.48 L of solution - Express your answer using two significant figures. B) 62.1 g C2H6O in 2.18 L of solution - Express your answer using three significant figures.

C) 16.14 mg KI in 106 mL of solution - Express your answer using three significant figures.

Thank you so much in advance!

For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1550 M and a Cl2 concentration of 0.171 M at 1000 K. What is the equilibrium concentration of CO at 1000 K. What is the equilibrium concentration of Cl2 at 1000 K? What is the equilibrium concentration of COCl2 at 1000 K? Express all answers to three significant figures

A closed container at 58.1˚C and 285 mm Hg contains a mixture of n-heptane and cyclohexane. Both liquid and vapor phases exist in equilibrium, and the vapor phase contains 32 mol % n-heptane. a) Calculate the mole fractions of the liquid phases. b) Now, the pressure in the container doubles, will the saturation pressure of n-heptane increase, decrease, or stay the same? Justify your answer

Industrial humidifiers has two inlet streams – 1. liquid water and 2. drier air. The entering liquid water stream flows at 5.31 mol/min. The component flow rate of air in the drier air stream is 44.3 mol/min. The exiting streams consist of a wetter air stream and a liquid water stream. The exiting liquid water stream contains 34.5% of the entering liquid water. The outlet streams are in vapor liquid equilibrium at 42.8oC and 786 mmHg.
a) Draw the process flow diagram, number the streams, and label the species in each stream.
b) Find the component mass flow rates (kg/min) of all four streams.
c) The pressure of the outlet streams decrease by 5%, will the mole fraction of water in the wetter air increase, decrease, stay the same? Justify your answer.

Wet air containing 60.4 mol% of pure water at 82.5˚C is fed to a dehumidifier at a rate of 185 mol/hr. Outlet of the dehumidifier consists of 2 streams – one stream of drier air and the other stream is pure liquid water. The outlet streams are in vapor-liquid equilibrium at 812 mmHg and 31.7oC.
a) Draw the process flow diagram, number the streams, and label the components in each stream.
b) Find the component mole flow rates (mol/hr) exiting the dehumidifier.
c) If the temperature of the inlet wet air increases by 10oC, will the molar flow rate of liquid water exiting the dehumidifier increase, decrease, or stay the same? Justify your answer.

For the preparation laboratory of a 4% solution (weight / volume) sodium hydroxide at from 50 mL of a 5 mol solution. L-1 this basis, it is necessary(explain your answer) Data: molar mass (g mol-1): Na = 23 O = 16 H= 1

a) adding 200 ml of water. b) adding 250 ml of water. c) adding 500 ml of water. d) evaporating 200 mL of water. e) evaporating 250 mL of water.

If 10mL of .18M Zn(NO3)2 is added to 20.0mL of .26M NaCl and concentration of ZnCl2 is found to be .026M. find Kc

A gas mixture containing 60% N2 and the balance n-hexane flows through a pipe at a rate of 200m3/hr. The pressure is 2atm absolute and the temperature is 100 C. a) What is the molar flow rate of the gas in kmol/hr? b) Is the gas saturated? Show calculations (hint: use vapor pressure of hexane at 100 C) c) If 80% of n-hexane is condensed (and leaves as a liquid), how much of vapor is leaving and what is its composition.

1. How does the titration of a diprotic acid differ from a monoprotic acid (like HF)?

2. How does the titration of a weak base with a strong acid differ from weak acid-strong base titration. (Review pages 848 - 850.) Note: you could perform these titrations from the chemical cabinet in this lab.

3. What kind of pH (above 7, below 7, or 7) do you expect at the equivalence point from the titration of a weak acid with a strong base?

4. What kind of pH (above 7, below 7, or 7) do you expect at the equivalence point from the titration of a weak base with a strong acid?

5. In a real lab, the volume of the "drop" cannot be so easily controlled. Drops come in various sizes and the smaller the drop, the finer the titration. This is one of those "art" parts of laboratory work. Discuss how a real lab titration would differ from your on-line lab.