In your previous studies last semester, you encountered reactions went to completion and were written A + B → C + D. You are now learning about reactions that achieve equilibrium and are written A + B ↔ C + D. Give the definitions of both types of reactions and justify the statement using mathematical relations that "reactions that go to completion are a subclass of the more general equilibrium reaction."

Consider the following 50.00 mL of 0.300 M acetic acid (HC2H3O2) was titrated with 0.200 M potassium hydroxide (KOH).

HC2H3O2 + KOH H2O + C2H3O2-K+

A. Calculate the pH of the solution when 20.00 mL of 0.200 M KOH is added.

B. Calculate the pH of the solution when 40.00 mL of 0.200 M KOH is added.

C. Calculate the pH of the solution when 50.00 mL of 0.200 M KOH is added.

A mixer used to prepare 1000 kg of 8 wt% sodium hydroxide (NaOH) solution. The feeds to the mixer are 10 mol% sodium hydroxide solution in water and pure water. What are the quantities (in kg) of pure water and 10 mol% sodium hydroxide solution to be added to the tank?

During the purging steps in the Schlenk line experiment, why does the chemist close the nitrogen before opening the vacuum? What gas is being evacuated?

multiple choice Q

A mixture of N₂, O₂, and Ar has mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N₂ if the total pressure of the mixture is 3.9 bar?

Two methods were used to measure fluorescence emission of a dye and following data were obtained;

A) Are the std. deviations are significantly different?

B) Are the means are significantly different?

What are three main differences between High Performance Liquid Chromatography and Gas Chromatography?

Calculate the wavelength of each of the following frequencies of electromagnetic radiation

A) 104.8 MHz (typical frequency for FM radio broadcasting)

B)1100 kHz (typical frequency for AM radio broadcasting)

C) 835.6 MHz (common frequency used for cell phone communication)

calculate the change in pH when 3.00 ml of 0.1 M HCL is added to 100 ml of a buffer solution that is 0.1 M in NH3 and 0.1 M in NH4Cl.
Calculate the change in pH when 3.00 ml of 0.1 M NaOH is added to the original buffer solution.

How will the following situations affect your final calculation of molarity of HC2H3O2? (higher, lower, unaffected. be specific) A) You wash the sides of the flask with deionized water to remove any vinegar of NaOH solution adhering to the side of the flask. B) You add 20 mL of water to the vinegar in the flask (assume no drops of vinegar adhere to the side of the flask). C) The tip of the buret is not filled when you start a titration but is filled when you finish the titration. D) The molarity of the standard NaOH solution is miscalulated and the true value is higher than the concentration given. E) As you are refilling your buret, some of the NaOH spills over the side and runs down the buret into the flask you intend to titrate.

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.128 M NaOH.

C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ)

What are the concentrations of the following ions at the equivalence point?

Na+, H3O+, OH-

C6H5CO2-

___M Na+

___M H3O+

___M OH-

___M C6H5CO2-

What is the pH of the solution?

predict the signs of delta G, delta H, delta S, of the system for the following processes

a)Ammonia melts at -60 degrees Celcius

b) ammonia melts at -77 Celcius (normal melting point of Ammonia)

c) ammonia melts at 100 Celcius

Describe the appearance of:

Silver nitrate test

Commercial 1- bromobutane: unheated? and heated?

Commercial t-butly chloride: unheated? and heated?

Sodium iodide test

Commercial 1- bromobutane: unheated? and heated?

Commercial t-butly chloride: unheated? and heated?

Part A

Determine the [OH−] of a solution that is 0.140 M in CO3.

Express your answer using two significant figures.

Part B

Determine pH of this solution.

Express your answer to two decimal places.

A 0.035 mol sample of a weak acid, HA, is dissolved in 601 mL of water and titrated with 0.41 M NaOH. After 33 mL of the NaOH solution has been added,

the overall pH = 5.281. Calculate the Ka value for the HA.

Let’s write out the acid dissociation:
HA ↔ A– + H+ Ka=???

Now, if we add NaOH (strong base), it will react with the HA (acid). So let’s construct an ICE table in moles to find out what’s left after reaction:

Can you pleae explain how they got the Change value== .0135???