A dilute solution of hydrochloric acid with a mass of 607.23 g and containing 0.33131 mol of HCl was exactly neutralized in a calorimeter by the sodium hydroxide in 614.70 g of a comparably dilute solution. The temperature increased from 15.848 to 19.739 °C. The specific heat of the HCl solution was 4.031 J·g^-1·°C^-1; that of the NaOH solution was 4.046 J·g^-1·°C^-1. The heat capacity of the calorimeter was 77.99 J·°C^-1.

Enter the balanced equation for the reaction. Include states in your answer.

Use the data above to calculate the heat evolved. What is the heat of neutralization per mole of HCl? Assume that the original solutions made independent contributions to the total heat capacity of the system following their mixing.
ΔH = ___ kJ/mol

1. What is oxidation?  How do you know if a molecule/atom has undergone oxidation.

2. Describe the reactivity of alcohols (1˚, 2˚, and 3˚) to oxidation.  

3. What are two ways besides IR that we can determine if we have the right product? Please explain what molecular property is measured and how borneol and camphor will show up differently in the technique.

4. When we take the IR of borneol and camphor, how will the spectra look different?

5. Why is the Camphor reaction considered “green”?

Calculate the pH of a buffer solution after the addition of 15.00 mL of 0.100 M NaOH to 50.00mL of the buffer that originally contains 0.100 M propanoic acid and 0.0750 M Sodium propionate. The Ka for propanoic acid is 1.3x10-5.

Problem 3 Grapefruit juice is known to effect drug oral bioavailability. Briefly describe the Grapejuice Effect on drug bioavailability

25.000 mL of 0.1438 M butanoic acid solution is titrated with 0.1247 M NaOH. Calculate the pH of titrant mixture at the following volumes of NaOH added. Ka butanoic acid = 1.52 x 10^-5

a.) 0.00 mL

b.) 16.04 mL

c.) 28.83 mL (Equivalence point)

d.) 30.30 mL

My answers were:

a.) 2.830

b.) 4.917

c.) 8.821

d.) 11.521

The active ingredient in a zinc nutritional supplement is ZnSO4·7H2O (molar mass = 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these ten tablets was 10.165 g. A 1.830 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted in the precipitation of ZnNH4PO4. The precipitate was filtered and dried, then ignited to produce 0.234 g of Zn2P2O7 (molar mass = 304.76 g/mol). What is the mass percent of ZnSO4·7H2O in each tablet?

2-What is the average mass of the active ingredient ZnSO4·7H2O and inactive filler in each tablet?

I need to second part (2)?

The density of NaCl (an fcc crystal) is 2.16 g/cm3. Find the distance that ions are from their nearest neighbors.

Which method is better for purifying a mixture of two liquids that boil at nearly the same temperature: simple distillation of fractional distillation? Explain your answer (Hint: your answer should explain the term "theoretical plates" and how they apply in this situation).

A sample of 6.33 g of solid calcium hydroxide is added to 28.0 mL of 0.500 M aqueous hydrochloric acid. Enter the balanced chemical equation for the reaction.

What are the limiting reactant?

How many grams of salt are formed after the reaction is complete?

How many grams of the excess reactant remain after the reaction is complete?

Compare the structure of xylenol orange to phenolphthalein. Do some research to determine why phenolphthalein changes color under acidic or basic conditions. Based on the chemistry of phenolphthalein, explain why xylenol orange is a different color in the presence and absence of zinc ions. It is useful to note that the xylenol orange-zinc complex that is red must absorb light around 500-550 nm while the free xylenol orange molecule is yellow, so must absorb light around 400-450 nm.

Titration of Phosporic acid.

Calculate the pH after 25mL, 50mL, 100mL, 150mL, 200mL, 250mL, 300mL, and 350mL of base is added.

Ka1=7.5E-3, Ka2=6.2E-8, Ka3=4.2E-13

(Multiple choice)
Which one of the following statements is true? Explain why T/F for each.
(a) In fiber reinforced composites, the dispersed phase will not have the same composition as
the matrix phase.
(b) When continuous-fiber reinforced composites are loaded longitudinally, the stress in the
fibers equals the stress in the matrix.
(c) Sandwich panels are useful because of their high weight-to-stiffness ratio.
(d) Approximately 30% of the overall strength of fiberglass is contributed by the matrix.
(e) The stiffness of aligned discontinuous-fiber reinforced composites loaded along the fiber
direction depends on the weight fraction of matrix in the composite.

Suppose a biochemist decided to use a HEPES buffer system to purify her His-tagged protein. HEPES is a sulfonic acid with a relevant pKa of 7.5. What volume of 1M NaOH would she need to add to a 250mL solution of 20mM HEPES to raise the pH from 7.5 to 8.0 (remember the HEPES is a weak acid).

Will Beer's law apply if in lab we choose to use concentrations in g/L, instead of moles? Explain