A nitric acid solution is composed of 63.75 g of HNO3 and 205.65 mL of pure water. What is the percent by mass of the nitric acid solution? Use the density of water as 0.9984 g/mL.

A. Assume that the 1.0 M (NH4)2 CO3 solution that you used was 1.00 M (NH4) 2 CO3. If Ka of H2CO3 is 5.6 x 10^-11 combine K's to obtain the equilibrium coonstant for NH4 + CO3^2 = NH3 + HCO3-

B. Show that a [Co3^2-] = 0.07 sub(9) M is consistent with the Kyou calculated in (a).

C. Now Calculate the pH of this solution.

D. Compare your calculated pH with the pH of the NH3/ NH4+ buffer( pH buffer: 11.62) . Has this bufferserved its function? Discuss.

E. Using the question above and the Ksp (=6.8x10^-6) of MgCO3 is there enough CO3^2- ion in a 1.0 M (NH4)2CO3 solution to precipitate MgCO3 from a 0.2 M Mg(H2O)6^2+ solution?

F. Is the equilibrium: Mg(H2O) 6^2+ +HCO3+ NH3= MgCO3 + NH4 + 6H2O readily attained? Y or N. State how you know.

Calculate the apparent solubility of benzoic acid at pH 5. Benzoic acid is a weak acid, with pK_a = 4.2 and solubility of nonionized species S₀ = 0.028 mol/L.
Please show steps

Explain how you would separate a solid mixture of sand and salt using any of the following methods either distillation, chromatography, or crystallization.

1. enter the net ionic equation, including phases, for the reaction of AgNO3(aq) and KCI(aq).

2. 76.0 mL of a 1.50 M solution is diluted to a total volume of 288 mL. A 144-mL portion of that solution is diluted by adding 127 mL of water. what is the final concentration? assume the volumes are additive.

3. what is the concentration of a solution made by diluting 35 mL of 6.0 M HCI to a final volume of 750 mL?

4. calculate the molarity of the following solutions.

a) 0.850 mol of Na2S in 1.85 L of solution.

b) 22.3 g of MgS in 981 mL of solution.

5. complete this equation for the dissociation of Na2CO3(aq). omit water from the equation because it is understood to be present.

Na2CO3(aq) --------->

Thermodynamics

A 1 m³ rigid tank has propane at 100 kPa and 300 K. The tank is connected to another 0.5 m³ rigid tank which has propane at 250 kPa and 400 K by a ball valve. The valve is opened and both tanks come to a uniform state at 325 K.

1-      State all assumptions you need to solve the problem.

2-      Calculate the final pressure of propane in both tanks?

3-      Calculate the mass of propane before and after opening the valve in each tank.

4-      Sketch the process on a P-V diagram.

5-      Find the compressibility factor of propane in each tank before opening the valve.

6-      Calculate the change in internal energy and enthalpy of propane in each tank.

Determine the initial concentration of Al in experiment #4. Include your units. 4 Al(g) + 3 O2(g) ⟶ 2 Al2O3(g)

A glucose solution contains 74.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing and boiling point of the solution.

In the bad old days, or even today for the few people who are doing very precise work, users had to calibrate volumetric flasks. Write down the required steps for a 100-mL volumetric flask, considering such things as temperature, atmospheric pressure, and buoyancy corrections

About how bad an error, by percent, would you make if you skipped the buoyancy correction (assume standard temperature and pressure

1. Assuming that the formation of an aqueous solution of Al(NO3)3 is obtained by mixing solid Al(OH)3 and aqueous nitric acid . Write a balanced net ionic equation?

       2. Which of the following combination will produce a precipitate?

Pb(NO3)2 (aq) and HCl (aq)

Cu(NO3)2 (aq) and KC2H3O2 (aq)

KOH (aq) and HNO3 (aq)

AgC2H3O2 (aq) and HC2H3O2 (aq)

NaOH (aq) and Sr(NO3)2 (aq)

         3 . In the following reaction, which species is reduced?

Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)

Complete and correctly sequence the steps for drawing Lewis Structures

WORD CHOICES: eight, one, valence, four, subtract, central, single, surrounding, higher, add, bonding, core, six, lower, more, multiple, less, two, pairs, Ione, octet, singles

A. Draw a ___ bond from each surrounding atom to the central atom, and ___ two valence electrons for each bond.

B. Determine the total number of ___ electrons available. For polyatomic ions, ___ one electron for each negative charge, or ___ one electron for each positive charge.

C. Place the atoms realtive to each other. Place the atom with ___ group number in the center because it has the ___ electronegativity. If atoms have the same group number, place the atom with the ___ period number in the center.

D. If the ___ atom still does not have a(n) ___, make a ___ bond by changing a ___ pait from on of the ___ atoms into a ___ pair to the ___ atom.

E. Distribute the remaining electrons as ___ so that each atom ends up with ___ electrons (or___for H). First place ___ pairs on ___ (___ electronegative) atoms to give each an ___. If any electrons remain, place them on the ___ atom. Then check that each atom has ___ electrons.

Using half equations for the oxidation and reduction, develop the redox equation for the oxidation of cyclohexanone under acid conditions.

The following data show the rate constant of a reaction measured at several different temperatures.

1.Use an Arrhenius plot to determine the activation barrier for the reaction.

2.Use an Arrhenius plot to determine frequency factor for the reaction.

1. Explain how Na2CO3 of primary standard grade can be prepared from primary standard grade NaHCO3? 2. Why is it common practice to boil the solution near the equivalence point in the standardization of acid with Na2CO3? 3. Calculate the molar concentration of a dilute HCl solution if titration of 0.2694 g of primary standard Na2CO3 required 38.77 mL of the acid (products CO2 and H2O).