I have 0.500 Liters of water. To that 0.500 Liters, I add the following:

a. 0.100 moles HCl

b. 0.100 moles HOAc

c. 0.100 moles NH4Cl

d. 0.100 HF

e. 0.050 moles NaOH

f. 0.050 moles NaOAc

g. 0.050 moles Mg(OH)2

What is the pH of the resulting mixture of everything?

Please show individual steps, since this question is meant to be answered sequentially from a to g. Thanks!

Part B What salt is produced in each of the following neutralization reactions? HNO3(aq)+KOH(aq)→H2O(l)+? HNO3(aq)+Ca(OH)2(aq)→H2O(l)+? HCl(aq)+Ca(OH)2(aq)→H2O(l)+? HCl(aq)+KOH(aq)→H2O(l)+? Drag the appropriate items to their respective bins.

Part C Which substances are always produced in an acid-base neutralization reaction? Check all that apply. Check all that apply. a base water an acid a gas a salt

Which of the following are true concerning the limit of quantification (LOQ) of a particular analysis method? Select all that are valid.

A 21.466 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 70.668 g of water. A 11.619 g aliquot of this solution is then titrated with 0.1062 M HCl. It required 30.75 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste.

The pH of a 0.00125 M solution of an aqueous solution of XOH (X = an unknown element) is 3.55. Is XOH a strong acid, weak acid, strong base, or weak base? How do you know? Is X a metal or non-metal? Explain

1.

Which molecule or ion has the same molecular geometry as SeO₃^2–?

A.SO₃

B.NO₃^–

C.CO₃^2–

D.SO₃^2–

E.SeO₃

_2.

Which of the following processes is not exothermic?

A. Rb+(g)+e- = Rb(g)

B. Br(g)+e- = Br-(g)

C. Rb+(g)+Br-(g) = RbBr(s)

D. Rb(g) = Rb(s)

E. 1/2 Br2 (g) = Br(g)

5)A gaseous mixture composed of 16.0 g of O2 , 21.0 g of N2, and 16.0 g of He at 20.0°C is confined in a 25.0 L container.
What is the partial pressure of N2 in this mixture?
6)A gaseous mixture composed of 16.0 g of 2, 21.0 g of N2, and 16.0 g of He at 20.0°C is confined in a 25.0 L container.
What is the partial pressure of He in this mixture?
7)Assuming ideal gas behavior, what is the pressure in atm exerted by 1.57 mol Cl2(g) confined to a volume of 1.50 L at 273K?

1. The possible components of your mixture are unreacted ferrocene and the substituted ferrocene product(s) of your reaction, which should travel the farthest up the TLC plate (highest Rf) and why?

2. Which should have a higher Rf value: the mono-substituted ferrocene or the di-substituted ferrocene?

3. In the column chromatography portion of your experiment next week, you use different solvents or solvent mixtures to elute the column for separation of your product mixture. Why is this required? Why use solvent mixtures for column elution instead of pure solvents?

organic acid is an important chemical used in the manufacture of polyesters and plasticizers. It contains only C, H, and O. Combustion of 19.81 mg of the acid produces 41.88 mg CO2 and 6.45 mg H2O. If 0.340 mol of terephthalic acid has a mass of 166g/mol calculate the a) empirical formula b)calculatethe molecular formula

The herbicide 2,4-D is being analyzed in plant matter using triphenylphosphate (TPP) as an internal standard. A calibration sample is prepared by pipetting 10.0 µL of 119 µg/mL 2,4-D and 10.0 µL of 100 µg/mL TPP into 1.00 mL of acetonitrile (ACN). (Hint: What is the total volume?) Separation by HPLC gave the peaks shown in the table below. The sample was analyzed by homogenizing 5.196 g of plant material and extracting the 2,4-D into 2.4 mL of ACN. 10.0 µL of 100 µg/mL TPP was added to the ACN extract before HPLC gave the peak areas shown below.

Peak Areas    2,4-D TPP

Calibration Solution 28685    15865

Plant Extract    2217    5816

Calculate the concentration of 2,4-D in the plant material in units of ng/g (ppb).

ng/g

calculate ionization energy of He using Slater rules

Write net ionic equations for the cases where oxidation-reduction reactions between metals and metallic ions were observed. (Be sure you balance the reaction so that the electrons balance.)

Copper in silver sulfate, zinc in silver sulfate, magnesium in silver sulfate, zinc in copper sulfate, magnesium in copper sulfate, magnesium in zinc sulfate.

A sample containing 321.5 g of nitrogen gas is expanded isothermally at T=298 K from 1.023dm^3 to 57.28dm^3. Calculate q, w, delta U and delta H for four processes assuming N^2 behaves ideally:

(a.) in a vacuum

(b.) against a constant external pressure equal to the final pressure of the sample

(c.) reversibly

(d.) adiabatically (non-isothermal)

1. a. In an extraction experiment, in which three compounds are extracted from a solid mixture. Why would the percent recoveries be less that 100%? Please explain.

b. How do you know if the recystaillization was effective (did purification result)? Talk about melting points

Determination of Iron in Vitamin Supplements by Spectrophotometric Analysis

A tablet containing iron, Fe (II) fumarate (Fe2+C4H2O4 2- ) and binder was dissolved in 0.1M HCl solution and the solution was filtered to remove any insoluble binder

Fe (II) in the above step was oxidized with hydrogen peroxide to Fe (III) as follows 2 Fe2+ + H2O2 + H+ → 2 Fe3+ + 2 H2O

The solution prepared in above step 3 was transferred to a 1000 mL volumetric flask. To this flask, 1M potassium thiocyanate (KSCN) was added and volume was brought to 1000 mL with water. Reaction of Fe (III) with KSCN formed a blue color solution.

Fe3+(aq) + SCN- (aq) Fe(SCN)2+(aq)

UV absorbance at 477 nm was measured for the solution prepared in step 3 and the absorbance value was recorded in the laboratory notebook

Steps 1 through 4 was repeated for additional 5 tablets (six tablets total). 6. Following are the UV absorbance values for the FeSCN complex prepared for each tablet.

Following are the UV absorbance values for the FeSCN complex prepared for each tablet.

Tablet Number               Absorbances

1 0.639

2                              0.683

3                              0.702

4                              0.732

5                              0.722

6                              0.767

A calibration curve was prepared from a ferric chloride (FeCl3) standards from 20 to 60 µg/mL concentration range that provided the following absorbance values.

Fe (µg/mL)      Absorbance @450nm

10                           0.434

20                           0.566

30                           0.625

40                          0.880

50                           1.002

The mass of iron in milligram in each tablet was recorded in the laboratory notebook. Calculate the mass of iron from the two tables for each tablet using the spectrophotometric method (Remember to correct for the dilution factor).

I made the Calibration Curve and got this equation.

y = 16.92x + 0.0064

How do I solve for the mass of iron using this equation?