Discuss the fundamental principles, instrumentation, and analytical capabilities of thefollowing techniques:

•Potentiometry

•Cyclic voltammetry

•Anodic Stripping voltammetry

(b) Which technique is most selective for the determination of Calcium? Explain.

(c) Using a typical example, discuss the mechanism of ionization used in mass spectrometry

Acid/Base Equilibrium - Weak Acids/Bases

1. Estimate the initial [HClO] in an aqueous solution in which the [OCl^-] is 0.0000114 M at equilibrium (make an exact calculationassuming that initial concentration is not equal to the equilibrium concentration).

(Constant = K_a=3.50×10^-8)

HClO = OCl^- + H⁺

^{_________________ M}

3. Calculate the molar concentration of H⁺ ion of a 1.31×10^-2 M solution of the weak acid HClO (make an exact calculationassuming that initial concentration is not equal to the equilibrium concentration). Round your answer to 3 significant digits.

(Constant = K_a=3.50×10^-8)

HClO = OCl^- + H⁺

How many grams of dry NH4Cl need to be added to 2.20 L of a 0.600 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.50? Kb for ammonia is 1.8×10−5.

Calculate ? H for the reaction: C4H4(g) + 2 H2(g) — > C4H8(g) ? H = ?

Given,

C4H4(g) + 5 O2(g) — > 4 CO2(g) + 2 H2O(l) DH = -2341 kJ

C4H8(g) + 6 O2(g) — > 4 CO2(g) + 4 H2O(l) DH = -2755 kJ

H2(g) + ½ O2(g) — > H2O(l) DH = -286 kJ

Calculate the pH during the titration of 40.00 ml of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid.

A) 29.00 ml
B) 39.00 ml
C) 48.00 ml

A 9.15-L container holds a mixture of two gases at 27 °C. The partial pressures of gas A and gas B, respectively, are 0.214 atm and 0.618 atm. If 0.210 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

Can the number and type of defects be varied and controlled? How? Explain the exponential variation of the concentration of defects with temperature. Explain each term of the equation in terms of their physical significance

Using Appendix 4 for ∆Hf ° and ΔS˚, which of the following reactions is spontaneous:

(5.a) 2 H₂S(g) + 3 O₂(g) → 2 H₂O(g) + 2 SO₂(g)

(5.b) SO₂(g) + H₂O₂(ℓ) → H₂SO₄(ℓ)

(5.c) S(g) + O₂(g) → SO₂(g)

You must determine whether a given reaction (i) is exothermic or endothermic, (ii) has a positive or negative entropy, and (iii) if a given reaction is spontaneous only at low temperature or only at high temperature, or at all temperatures.

Methyl methacrylate was polymerized at a mass concentration of 200g dm^-3 in toluene using azobisisobutyronitrile as initiator at a mass concentration of 1.64 X 10^-2 g dm^-3 and a reaction temperature of 60 degree C. Calculate the initial rate of polymerization and the molar mass of the poly(methyl methacrylate) formed in the initial stages of the reaction given that the relevant rate coefficients at 60 degrees C are:

Initiator dissociation: k sub d= 8.5 X 10 ^-6 reciproical seconds

Propagation k sub p= 8.33 dm^3 mol^-1 s^-1

termination, k sub t= 9.3 X 10 ^6 dm ^3 mol ^-1 s^-1

transfer to monomer k sub trm= 3.93 X 10 ^-3 dm^3mol^-1s^-1

Transfer to solvent k sub trS= 7.34 X 10 ^-3 d, ^3 mol ^-1 s^-1

Assume that the initiator efficiency f=0.7 that the termination by combinaition is negligible, and that the density of the initial solution of MMA in toluene is 860 g dm^-3

Use Coulomb's law to estimate the average distance between the sodium nucleus and the 3s electron.

1. Why is it not possible to reuse a heat pack in term of the chemistry?

2. Compare the specific heat of water to the specific heat of metal (Copper). Which would heat up faster (with less energy required)?

3. Why would metal make a poor ingredient in a heat pack?

4. If there was a delay between measuring the initial temperature of a hot object and its transfer to the calorimeter, how would the heat capacity of the object be affected? How would the calculation of the heat capacity of the calorimeter be affected (too high, too low, or no affect)?

What is the pH of an aqueous solution with a hydrogen ion concentration of [H ] = 4.9 × 10–8 M?

The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction: AgNO3(aq)+HCl(aq)→AgCl(s)+HNO3(aq) When you combine 90.0 mL of 0.150 M AgNO3 with 90.0 mL of 0.150 M HCl in a coffee-cup calorimeter, the temperature changes from 23.49 ∘C to 24.47 ∘C

Calculate ΔHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and C=4.18J/g⋅∘C as the specific heat capacity.