for the first part of the experiment, in which you are varying the amount of tyrosinase, how many millimeters of 15mM L-DOPA will be in each tube?

What volume (to the nearest 0.1 mL) of 6.00-M NaOH must be added to 0.400 L of 0.250-M HNO₂ to prepare a pH = 4.30 buffer?

What volume (to the nearest 0.1 mL) of 5.50-M HCl must be added to 0.250 L of 0.200-M K₂HPO₄ to prepare a pH = 7.10 buffer?

Determine the Theorethical Oxygen Demand(ThOD) for sewage containing 150 mg/L of CH₂(NH₂)COOH and 40 mg/L of NH₃.

Find,

(1) mg/L of oxygen for both carbon and nitrogen compounds

(2) grams of oxygen per gram of CH2(NH2)COOH (oxygen used only for carbon oxidation)

(3) grams of oxygen per gram of NH3 (oxygen used only for nitrification)

1.Acids commonly dissociate to give hydrogen ions insolution (H+), while bases dissociate to give hydroxide ions in solution (OH-). Why is it important to know the difference between acids and bases, in terms of safety? 2.Ionic bonds, covalent bonds and hydrogen bonds all help to hold chemical entities together. Distinguish between these types of bonding and explain which type of bonding is responsible for matching the base pairs in DNA.

calculate the cost/gram of crude and recrystallized product for the reaction given the following: salycylamide ($0.38/g); NaI ($0.78/G); 6% (W/V) NaOCl ($1.34/l); sodium thiosulfate ($10.16/L); ethanol (absolute and 95%) ($11.17/L).You can ignore the cost of 10% HCl since the amount used was not determined accurately and it is dirt cheap. The product you made is not readily available from commercial suppliers so we could have to conclude this reaction is economically feasible!

Calculate the pH at the equivalence point for titrating 0.160 M solutions of each of the following bases with 0.160 MHBr.

- hydroxylamine (NH2OH)

- aniline (C6H5NH2)

Summarize IR Spectroscopy and what are real-life analogies to IR spectroscopy?

Please Explain! Thank you so much.

An aqueous solution of ethyl acetate at room temperature has an itial concentration of 0.15 M. Calculate the equilibrium concentrations of ethyl acetate (CH3COOC2H5), ethanol (C2H5OH) and acetic acid if the equilibrium constant at this temperature is Kc= 3.00.

Part B. Repeat this calculation for initial ehtyl acetate concentrations of 0.25 M and 0.35 M. Are your answers in agreement with Le Chatelier's Principle?

1. Find the MSDS for potassium chlorate. a) Are there any health hazards associated with this material, and what conditions produce these hazards?
b) Under what conditions does it produce fire or explosion hazards?
c) Since this experiment involves high temperatures, what are the melting point and decomposition temperature for potassium chlorate? melting temperature _________ decomposition temperature _________
d) Based on these values, what will you see happening to the potassium chlorate solid as you begin heating it to high temperatures

A chemist at a pharmaceutical company is measuring equilibrium constants for reactions in which drug candidate molecules bind to a protein involved in cancer. The drug molecules bind the protein in a 1:1 ratio to form a drug-protein complex. The protein concentration in aqueous solution at 25 ∘C is 1.58×10⁻⁶ M . Drug A is introduced into the protein solution at an initial concentration of 2.00×10^-6 M. Drug B is introduced into a separate, identical protein solution at an initial concentration of 2.00×10^-6 M. At equilibrium, the drug A-protein solution has an A-protein complex concentration of 1.00×10^-6 M, and the drug B solution has a B-protein complex concentration of 1.40×10^-6 M.

Part A: Calculate the K_c value for the A-protein biding reaction.

Part B: Calculate the K_c value for the B-protein biding reaction.

Part C: Assuming that the drug that binds more strongly will be more effective, which drug is the better choice for further research?

Calculate the pH of 6.6 × 10-8 M HCl. Report your answer to the hundredths place.

What is the change in pH when 10.0 mL of 0.250 M KOH (aq) is added to 100.0 mL of a buffer that is 0.150 M in HCOOH (aq) and 0.100 M in HCOO^– (aq)? pK_a = 3.75 for HCOOH (aq).

Select one:

a. –0.26 pH unit

b. +0.18 pH unit

c. +0.00 pH unit

d. –0.81 pH unit

QUESTION 2

What is the molarity of an aqueous barium hydroxide solution if it takes 59.9 mL of 0.100 M HCl (aq) to neutralize 21.6 mL of the Ba(OH)₂ (aq) solution?

Select one:

a. 0.208 M

b. 0.277 M

c. 0.139 M

d. 0.0693 M

Given a solution of 0.125 M CH₃COOH (aq) and a solution of 0.150 M NaCH₃COO (aq), how would you prepare 100.0 mL of a buffer solution with a pH of 4.400? pK_a = 4.740 for CH₃COOH (aq).

Select one:

a. Mix 68.6 mL of the CH₃COOH (aq) with 31.4 mL of the NaCH₃COO (aq)

b. Mix 27.6 mL of the CH₃COOH (aq) with 72.4 mL of the NaCH₃COO (aq)

c. Mix 72.4 mL of the CH₃COOH (aq) with 27.6 mL of the NaCH₃COO (aq)

d. Mix 50.0 mL of the CH₃COOH (aq) with 50.0 mL of the NaCH₃COO (aq)

QUESTION 2

If 15.9 grams of NH₄Cl (s) are added to 250.0 mL of 0.350 M NH₃ (aq) solution, what is the resulting pH? Assume no change in volume upon adding the NH₄Cl (s). pK_a = 9.25 for NH₃ (aq).

Select one:

a. 8.55

b. 8.38

c. 9.06

d. 8.72

A mixture is made by combining 11.5 mL of 8.5×10−3 M KSCN, 6.3 mL of 3.7×10−2 M Fe(NO3)3, and 10.4 mL of 0.397 M HNO3. Calculate the concentraion of Fe3+ in the solution.

1. Assume that the rate law for a reaction is rate = k[A][B]^2

a) what is the overall order of the reaction?

b) if the concentration of both A and B are doubled, how will this affect the rate of the reaction?

c) how will doubling the concentration of A, while the concentration of B is kept constant, affect the value of k (assume that temperature does not change)? how is the rate affected?

2. It is found for the reaction 2A + B ---> C that doubling the concentration of either A or B while maintaining the other concentration constant quadruples the reaction rate. Write a rate law for the reaction.