Estimate the pH of the resulting solution prepared by mixing 1.0 mole of solid disodium phosphate and 1.25 mole of hydrochloric acid. The pKas of phosphoric acid are 2.1,7.2,12.4. The answer is 2.1<pH<7.2. Please explain.

0.5 mole of a monatomic ideal gas is loaded into a cylinder and contained by a frictionless piston. The piston is set so that there is an initial volume of 2L. The gas in the cylinder is at a temperature of 298K. The gas is allowed to expand adiabatically against 1 atm of pressure. Calculate V/n initial, q per mole, w per mole, delta U per mole, delta S per mole and delta H per mole. What is the final temperature of the gas in Kelvin and Celcius?

1. What is natural radioactivity? Speak to the different types of radiation that an unstable nucleus may emit, and the different types of radiation involved.
2. Why is it important to be able to write a balanced nuclear equation for radioactive decay? Go into some of the specifics of what is involved in writing an equation.
3. What is a “half-life” and why is it important to know the half-life of a radioisotope? List a few applications of how scientists make use of having this knowledge. Why would it be so important to know the half-lives of radioisotopes when it comes to medical applications?
4. Briefly describe how we can make use our knowledge of radioactivity in medicine. Speak about the characteristics of the radioisotopes used in these types of applications. What might they have in common? What process(es) do we use to detect these radioisotopes?

1A. Determine the pH of a KOH solution made by mixing 0.251 g KOH (s) with enough water to make 1.00 × 102 mL of solution. Assume 100% purity for the KOH (s).

1B. Predict the direction in which the equilibrium will lie for the following reaction:     H3PO4(aq) + HSO4−(aq) H2PO4−(aq) + H2SO4(aq).    Ka1(H3PO4) = 7.5 × 10−3;

Ka(H2SO4) = very large    

2. For H3PO4, Ka1 = 7.3 × 10−3, Ka2 = 6.2 × 10−6, and Ka3 = 4.8 × 10−13. An aqueous solution of Na3PO4 therefore would be?

2B. Calculate the pH of a solution of 0.10 M HA- (aq). The acid H2A has Ka1 = 6.5 × 10−2 and Ka2 = 6.1 × 10–5.  

HClO(aq) = Cl2 (aq) E^o = + 1.611V

MnO4^-1(aq) = MnO2(s) E^o = + 1.679V

In a particular cell, E_cell is measured to be +0.038v when the pH in both half-cells is 4.00 and [Cl2] = 0.20 M, [HClO] = 0.10 M. What is [MnO4^-1] in the solution?

A student is given two unknown samples continuing two different compounds with the same molecular formula, C3H7NO, he annaylzes them by IR and 1H NMR

Compound A:

IR: 3366, 3189, 2976, 1662 cm-1

1H NMR: 1.15 ppm, 3H, t

2.24 ppm, 2H, q

6.21 ppm, 2H, broad

Compound B:

IR: 3294, 3099, 2946, 1655 cm-1

1H NMR: 1.98 ppm, 3H, s

2.79 ppm, 3H, s

6.40 ppm, 1H, broad

Identify the structure of each compound and justify your answer.

Use Molecular Orbital Theory to describe bonding in the following. Also find the bond order and decide if stable or not. Is species dia or paramagnetic?

i. C₂⁺   ii. Be₂⁺   iii. Ne₂

Discuss the nature of the three main types of atomic line broadening and include the relative magnitude of broadening for each. Also, discuss what can be done, if anything, to reduce the magnitude of each type in specific experiments.

Calculate the percent ionization of formic acid solutions having the following concentrations. Ka = 1.8x10-4

Part B 0.460 M Express your answer using two significant figures.

Express your answer using two significant figures.

c) 0.110 M Express your answer using two significant figures.

d)5.40×10−2 M Express your answer using two significant figures.

What volumes of 0.53 M HNO₂ and 0.53 M NaNO₂ must be mixed to prepare 1.00 L of a solution buffered at pH = 3.25?

Calcuate the pH when 80 mL of 1.25 M HCL is added to 779 mL of 1.60 M of sodium acetate.

Please show all calculations. Thanks! :)

For

the

questions

below,

give

full

structural

diagrams

and

names

for

all

reactants

and

products.

Also

indicate

the

TYPE

OF

REACTION.

2. The

formation

of

2,2--?pentanediol

from

1--?pentyne.

3. The

reaction

between

trans--?2--?hexene

with

hydrogen

bromide.

4. The

formation

of

2--?butanol

from

an

alkene.

5. The

reaction

between

2

moles

of

water

with

2--?pentyne.

6. The

oxidation

of

2--?butanol.

7. The

combustion

of

2--?pentanol.

8. Show

the

formation

of

2--?butene

from

an

alcohol.

9. Show

the

reaction

between

water

and

cyclohexene.

1) A 28.6 mL sample of 0.226 M methylamine, CH₃NH₂, is titrated with 0.221 M nitric acid.
After adding 11.5 mL of nitric acid, the pH is

2) A 24.0 mL sample of 0.372 M methylamine, CH₃NH₂, is titrated with 0.381 M hydrochloric acid.
After adding 35.9 mL of hydrochloric acid, the pH is