For each of the following five reactions, circle the specific chemical species that is: reduced, and draw a box around the specific chemical species that is oxidized:

a) MnO₂ (s) + 2 I^- (aq) +4 H⁺ (aq) --> Mn²⁺ (aq) + I₂ (aq) + 2 H₂O (l)
b) Cd (s) + 2 NiO(OH) (s) + 2 H₂O (l) --> 2 Ni(OH)₂ (s) + Cd(OH)₂ (s)
c) NH₄⁺ (aq) + 2 O₂ (g) --> NO₃^- (aq) + 2 H⁺ (aq) + H₂O (l)
d) 2 CuFeS₂ (s) + 4 O₂ (g) --> Cu₂S (s) + 2 FeO (s) + 3 SO₂ (g)
e) 2 K₂FeO₄ (aq) + 3 Zn (s) --> Fe₂O₃ (s) + ZnO (s) + 2 K₂ZnO₂ (aq)

A) What is the rate constant for the reaction with an average time of 48.6 seconds, between 3.00 ml of 0.1 M t-butyl chloride, 3 ml 0.01 M NaOH, 4 ml water with 3 drops bromophenyl blue solution.

B) What is the rate constant for the reaction with an average time of 48.6 seconds, between 3.00 ml of 0.1 M t-butyl chloride, 6 ml 0.01 M NaOH, 1 ml water with 3 drops bromophenyl blue solution.

Name the kinds of attractive forces that must be overcome in order to perform the following tasks. Select all that apply.

1) Dissolve CsI in liquid HF:

Dipole-dipole interactions

Ionic Bonding

Ion-dipole interactions

Dispersion Forces

Hydrogen Bonding

2) Melt potassium metal:

Dipole-dipole interactions

Ionic Bonding

Ion-dipole interactions

Dispersion Forces

Hydrogen Bonding

A generic solid, X, has a molar mass of 80.4 g/mol. In a constant-pressure calorimeter, 16.0 g of X is dissolved in 337 g of water at 23.00 °C.

The temperature of the resulting solution rises to 28.70 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. How much heat was absorbed by the solution?

how much heat was absoped

waht is the enthrapy

a. explain in structure and words the observation that soap does not work properly in very low PH water or hard water which has calcium and magnesium ions.

b. would a soap made form N,N,N-trimethyl octadecyl ammonium chloride have thesame problems as a long chain of carboxylic acid? Explain

Consider the titration of a 28.0-mL sample of 0.180 M CH3NH2 with 0.145 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.)

Determine the pH after adding 6.0 mL of acid beyond the equivalence point.

Express your answer using two decimal places.

Describe the preparation of 3.00 L of 0.150 M glycine buffer, pH 8.1, from glycine and 1.00 M NaOH. What mass of glycine is required? The appropriate pKapKa of glycine is 9.6. Apply appropriate significant figures.

Chemistry Charles's Law Post-Laboratory Questions

1. Serveral students performed this experiment without paying adequate attention to the details of the procedure. Briefly explain what effect each of the following procedural changes would have ont the size of the volume-to-temperature ratio calculated by the students.

A) One student failed to replenish the boiling water in the boiling-water bath as the flask was being heated. At the end of the 6 min of heating, the boiling water in the bath was only in contact with the lower portion of the flask.

B) Following the proper heating of the flask in the boiling water, a student removed the flask from the boiling-water bath but only partially immersed the flask in the ice-water bath during the cooling period.

C) A student neglected to close the pinch clamp before removing the flask from the boiling-water bath and immersing it in the ice-water bath.

D) One student neglected to measure the volume of the flask before leaving the laboratory. Because the procedure called for a 125-mL Erlenmeyer flask, the student used 125 mL as the volume of the flask.

Calculate the pH of a solution made by mixing 100.0 mL of 0.044 M NH_3 with 100.0 mL of 0.126 M HCl. (Kb for NH_3 = 1.8 x 10^-5)

Explain what Vmax and Km describe

1.Write the equilibrium expression for the dissociation of KHT (s) in water. B. Develop an ICE chart for the dissociation of KHT in water.

1. Show calculations and briefly describe how you will make the following solutions:

   1. 50.00 mL of 0.200 M Fe(NO3)3(aq) solution from iron(III) nitrate nonahydrate

   2. 200.00 mL of a 2.00 mM KSCN(aq) solution from potassium thiocyanate.

   3. 100.00 mL of 1.00 M CoCl2(aq) solution from cobalt(II) chloride hexahydrate.

2. Write the equilibrium expression for parts A, B, and C of the lab based on the equations that are shown in the prior section.

3. Look at the expression for cobalt complexation with chloride ions (Part B of the lab). How would doubling the amount of water in the reaction vessel affect the product concentrations compared to the reactant concentrations?

4. How is the [ ] used in metal complexes like the cobalt tetrachloride complex [CoCl4]2- different from the [ ] used in the general equilibrium expression that follows?

K=[B]2[C]/[A

Explain why using deionized water to rinse the walls of the flask have no effect on the reported results of titrations performed.

Which is (are) the spectator ion(s) in the following precipitation reaction (equation not balanced)? (NH4)3PO4(aq) + Al2(SO4)3(aq) --> AlPO4(s) + (NH4)2SO4(aq)