Calculate the final concentration of each of the following diluted solutions.

0.50 L of a 4.0 M HNO3 solution is added to water so that the final volume is 8.0 L .

Water is added to 0.35 L of a 6.0 M KOH solution to make 2.0 L of a diluted KOH solution.

A 65.0 mL sample of 8.0 % (m/v) NaOH is diluted with water so that the final volume is 200.0 mL .

A 8.0 mL sample of 50.0 % (m/v) acetic acid (HC2H3O2) solution is added to water to give a final volume of 25 mL .

What is the concentration of EACH solution in these reactions...

Table 1: Concentrations Used of H2O2 and KI
Trial	H2O2	KI
1	5 mL of 3% H2O2	10 mL of 0.60M KI
2	5 mL of 3% H2O2	10 mL of 0.30M KI
3	5 mL of 2.25% H2O2	10 mL of 0.60 M KI

When pure carbon is burnt in air some of it is oxidized to C02 and some to CO. If the molar ratio of N2 to 02 is 7.18 and the molar ratio of CO to C02 is 2, what is the percentage excess air used? Exit gases contain only N2, O2, CO and C02.

What is the Q (IP) when 284 mL of 0.053 M solution of Na2CO3(aq) are mixed with 243 mL of 0.072 M solution of BaCl2(aq). The solid product is BaCO3

Would using a spectroscopic method to determine equilibrium constant of a solution work if there was no isosbestic point in the absorption spectra?Why or why not?

At a given temperature, 1.43 atm of H2 and 3.15 atm of I2 are mixed and allowed to come to equilibrium. The equilibrium pressure of HI is found to be 1.844 atm. Calculate Kp for the reaction at this temperature. H2(g) + I2(g) <=> 2 HI(g).

A reduction reaction can be carried on many organic compounds. It is the reverse of an oxidation reaction. Which of the following statements is true? A reduction reaction can be carried on many organic compounds. It is the reverse of an oxidation reaction. Which of the following statements is true? Reduction reactions are characterized by the increase in the number of carbon-oxygen bonds. Reduction reactions are characterized by the decrease in the number of carbon-oxygen bonds. Alcohols are reduced to aldehydes. Reduction reactions are characterized by the decrease in the number of hydrogen atoms.

Van der Waals Gases

Under what conditions of volume does a van der Waals gas behave like an ideal gas? Use the van der Waals equation of state to justify your answer.

What is the pH of a 0.56 M solution of methylammonium chloride, CH3NH3Cl? What is the concentration of methylamine in the solution? Kb (methylamine) = 4.4×10-4 pH = ___________ [MeNH2] =________M

Part A

At a pH of 7.40, what is the ratio of the molar concentrations of HPO42− to H2PO4−? Express your answer using two significant figures.

Part B

At a pH of 7.40, what is the ratio of the molar concentrations of H2PO4− to H3PO4? Express your answer using two significant figures.

Part C

At a pH of 7.40, what is the ratio of the molar concentrations of CO32− to HCO3−? Express your answer using two significant figures.

23. In the following reaction, how many grams of sodium sulfate are needed to react with 3.08 moles of strontium nitrate? (Hint: stoichiometry mol Na2SO4: mol Sr(NO3)2 = 1 mol: 1 mol) Sr(NO3)2 (aq) + Na2SO4 (aq) --> SrSO4 (s) + 2 NaNO3 (aq) (balanced?)

A cylinder with a piston contains 0.300 mol of oxygen at 2.50×105 Pa and 360 K . The oxygen may be treated as an ideal gas. The gas first expands isobarically to twice its original volume. It is then compressed isothermally back to its original volume, and finally it is cooled isochorically to its original pressure.

a. Find the heat added to the gas during the initial expansion

b. Find internal-energy change of the gas during the initial expansion.

c. Find the heat added during the final cooling;

d. Find the internal-energy change during the isothermal compression.

1. The lines observed in H-lamp are parts of Balmer Series. All these lines are due to a transition from various higher n value to a common n. What is this common lower n value for all these lines?

0

1

2

3

2. The lines on Absorption Atomic Spectra correspond to energies needed for electrons to be excited from a lower energy level to a higher energy level. Assume that the energy needed for an electron in 2p orbital in an O atom to jump to 3s orbital is 3.6*10-19 J, what is its wavelength of the line atomic spectra in nanometer (nm)?

3. Given: In Atomic Spectra lab, a student obtained his best-fit line equation to be y = 0.29 x + 46.8 when he plotted his Vernier reading on the y-axis and wavelength in nm on the x-axis.

4. The only electron in a hydrogen atom moved from n=2 to n=6. What is the wavelength of photon (in nm) being associated with this transition? Use whole numbers of nm without any decimal places, such as "415", "1125".

5.

Which of the following transitions in H will absorb the longest wavelength photon?

n=1 to n=2

n=2 to n=4

n=10 to n=3

n=3 to n=100

6. A student obtained the Rydberg constant to be 2.17*10-18 J. What is the % error of the measurement? Answer as percentage and keep one decimal place.

chlorine gas can be prepared in the lab by the reaction of hydrochloric acid with manganese oxide. you add 42.5g of MnO2 to a solution containing 48.9g of HCL.

A-what is the theoretical yield of Cl2?

B- if the yield of the reaction is 79.5%, what is the actual yield of chlorine?

A 0.582 gram sample of a metal, M, reacts completely with sulfuric acid according to:M(s)+H2SO4(aq)--->MSO4(aq)+H2(g).A volume of 269 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr and the temperature is 25 °C. Calculate the molar mass of the metal.