In an acid-base titration experiment, 50 mL of a 0.05 M solution of acetic acid (Ka = 1.75 x 10-5 ) was titrated with a 0.05M solution of NaOH at 25 oC. The system will acquire this pH after addition of 40 mL of the titrant:

Answer: 5.36

How do you solve this?

Given 100.0 ml of a buffer that is 0.50 M in HOCl and 0.40 M in NaOCl, what is the pH after 10.0 ml of 1.0 M NaOH has been added?

(Ka for HOCl =3.5 x 10^-8)

A 10 g object at 50^oC is placed in 100 g water at 39.8^oC in a calorimeter. The temperature of the water and the object equilibrated at 40.0^oC. Identify the metal.

Please explain this. Thanks!

The objective of this experiment is to identify real world applications of quantum mechanics. Write a paper with a minimum of 1200 words discussing real world applications of quantum mechanics. Do NOT copy and paste off the internet!

A 10 g ice cube at 0^oC is melted in 100 g water initially at 20^oC. The equilibrium temperature of the mixture is 10.93^oC.

Calculate:

a) The heat lost by the water.

b) The heat gained by the melted water of the ice cube.

c) The heat absorbed by the ice to achieve melting.

Given the following reactions:

COBr₂ (g) --------------- > CO (g) + Br₂ (g)              K = .190 at 73 °C

2 BrCl (g) ------------ > Br₂ (g) + Cl₂ (g)          K = 310 at 73 °C (estimated)

Find the equilibrium constant at 73 °C for: CO + BrCl ------- > COBr₂ + Cl₂

Sulfuryl chloride,SO2Cl2,a compound with very irritating vapors, is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature it decomposes. Given: SO2Cl2 (g)  SO2 (g) + Cl2 (g) Kc = 0.0450 A sample of 6.70 g SO2Cl2 was placed in a 1.00 L container and heated to 375 oC a. Calculate the concentrations of all species after equilibrium is reached (Assume, in this case that “x” is neg. for computation purposes). Show with approximation if possible.

100 moles/hour of pure ethane at 25 degrees Celsius and 1.0 atm are burned with 50.0% excess air producing a desired product of carbon dioxide and an undesired product of carbon monoxide. The fractional conversion of the ethane is 80.0% (on a molar basis). 95% of ethane that reacts goes to carbon dioxide. Determine the molar flow rate and molar composition of the gaseous product stream, which is at 400 degrees Celsius and 1.0 atm.

Completely label your diagram, list the temperature, pressure, flow rate, and composition (mole fractions with indexes) for eac stream, supply values and units for knowns and question marks for unknowns.

Chemical Reactions:
I: __C2H6 + __O2 ---> __CO2 + __ H2O
II: __C2H6 + __O2 ---> ___CO + ___H2O

Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:

Part A) 0.15M HF

Part B) 0.15M NaF

Part C) a mixture that is 0.15M in HF and 0.15M in NaF

A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial concentrations of Pb2+ and Cu2+ are 5.00×10−2 M and 1.50 M , respectively

What is the initial cell potential?

0.51V

What is the cell potential when the concentration of Cu2+ has fallen to 0.200 M ?

0.45V

Part C What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.360 V ?

I need help with Part C

A sample of carbonic acid (0.125 L, 0.199 M, pK_a1 = 6.35, pK_a2 = 10.33) was titrated with 1.75 M NaOH. Calculate the pH at the following points:

Before the titration.

At the 1st midpoint.

At the 1st stoichiometric (equivalence) point.

At the 2nd midpoint.

At the 2nd stoichiometric (equivalence) point.

Given the formula equation, write the complete ionic equation, net ionic equation, and identify the spectator ions for the following reaction: (NH4)2SO4 (aq) + 2 NaOH (aq) —> Na2SO4 (aq) + 2 H2O (l) + 2 NH3 (g)

Liquid octane (CH3(CH2)6CH3) will react with gasous oxygen (O2) to produce gasous carbon dioxide (CO2) and gasous water (H2O).

What is the theoretical yield of water formed from the reaction of 88.0 g of octane and 166.g of oxygen gas?

Be sure your answer has the correct number of significant digits in it.

A weak acid was HA (pKa=5.00) was titrated with 1.00M KOH. The acid solution had a volume of 100ml and a molarity of 0.100M. Find the pH at the following volumes of base added Vb= 0, 1, 5, 9, 9.9, 10, 10.1 and 12.