HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.026 M in NaClO at 25 °C?

You run an ion exchange column, eluting your protein with a high NaCl buffer. Would you be able to run a size exclusion column immediately after the IEX column or would you have to dialyze your sample to change the buffer first?

1. A 15.00 gram sample of ammonium chloride was dissolved in 100.00 grams of water. How much heat is produced by the dissolution (absorbed from the solution) if the solution temperature goes from 22.0 *C to 1.0 *C. The specific heat of the solution is 4.18 J/g*C

2. 300.0 mL of a 2.500 M Solution X was mixed with 300.0 mL of a 2.500 M Solution Y in a calorimeter. Both of the solutions were at the same temperature initially. Determine the heat of neutralization (kj/mole) if the temperature goes from 12.0 *C to 29.0 *C. Assume a molar ratio of 1:1. The specific heat of the solution is 4.281 J/ g*C. The density of the mixture is 1.050 g/mL.

3. Sketch a crude time-temperature graph for an endothermic reaction

4. Why, on an exothermic time-temperature graph, does the temperature eventually fall?

In polymer chemistry, Suppose we have two polypropylene samples.  One is atactic and one is isotactic.

a) Explain the microstructural difference between the two;

b) Would you expect the atactic sample to be stronger, weaker, or the same strength as the isotactic sample?  Explain.

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.040 M in NH4Cl at 25 °C?

An electrochemical battery is used to provide 1 milliwatt (mW) of power for a (small) light. The chemical reaction in the battery is: 1/2 N2 (g) + 3/2 H2 (g) → NH3 (g)

a. What is the free-energy change for the reaction at 25o C, 1 bar?

b. Calculate the free-energy change for the reaction at 50o C, 1 bar. State any assumptions made for this calculation.

c. The limiting reactant in the battery is 100 g of H2. Calculate the maximum length of time (seconds) the light can operate at 25o C

Use the data from the most concentrated solution of acetic acid to calculate the Ka value for acetic acid. Clearly show all of your work below. mot concentrated solution of acetic acid is 0.116m..ph = 2.85

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?