Calculate pBa when 50.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100 M Ba2+. For the buffered pH of 10, the fraction of EDTA in its fully deprotonated form is 0.30. Kf = 7.59 x 107 for BaY2-.

a) 7.36

b) 7.88

c) 1.30

d) 4.33

The following data was collected in a laboratory experiment conducted at 305.2 K.

A.) Determine the complete rate law for this simple chemical process A → B

B.) For the set of kinetic data in the problem above, if the rate doubles when the temperature increases to 415.4 K, what is the activation energy for the process?

Barium chloride and potassium carbonate combine to form barium carbonate and potassium chloride. The equation for this chemical reaction is shown below.

BaCl₂ + K₂CO₃--> BaCO₃ + KCl

An unknown compound contains only C, H, and O. Combustion of 6.10 g of this compound produced 14.9 g of CO2 and 6.10 g of H2O. What is the empirical formula of the unknown compound?

Ignoring activities, determine the molar solubility (S) of Zn(CN)2 in a solution with a pH = 1.34. Ksp (Zn(CN)2) = 3.0 × 10-16; Ka (HCN) = 6.2 × 10-10.

How much heat is released when 85.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ⋅ °C), and the molar heat capacity of ice is 36.4 J/(mol ⋅ °C).

Part A

Calculate the pH in 1.00MCH3CO2H.

Part B

Calculate the concentrations of all species present (H3O+, CH3CO2?, CH3CO2H, and OH?) in 1.00M CH3CO2H.

Answer the following questions based on the reaction: K2CrO4 + AgNO3 ---> red solid. A: What is the formula for the solid produced? B: Using the reaction above, a chemestry student has 35 mL of a .250 M solution of silver nitrate. How many milliliters of .105 M K2CrO4 will be required to react completely with the silver ion present. C: Considering the reaction in part b, how many grams of product will be formed?

A 0.380 m aqueous solution of NaCl is prepared at 20.0∘C. Assume that the density of the solution at 20.0∘C is 1.082 g/mL.

Calculate the molarity of the salt solution.

Describe why high pressures but low temperatures cause substances to deviate from ideal gas conditions. Make sure to discuss the assumptions we made to come to the ideal gas law and how high pressures and low temperatures negate those assumptions.

Using electronegativity arguments, classify the following diatomic molecules as nonpolar (N), polar (P), or ionic (I).

NaF

GaAs

H2

RbO

CO

for a linear molecule of polyethelyne of molar mass 11980 g mole ^- calculate :

The contour length of the molecule

B) the end to end distance in thr fully extended molecule and

C) the root mean square end to end distance according to the valence angle model .

In the calculation, end group can be neglected and it may be assumed that the c-c bonds are of length 0.154 nm your reasoning, which of the very large number of possible conformations of the molecyle is the most stable

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.170 M HClO(aq) with 0.170 M KOH(aq).

(a) before addition of any KOH

(b) after addition of 25.0 mL of KOH

(c) after addition of 30.0 mL of KOH

(d) after addition of 50.0 mL of KOH

(e) after addition of 60.0 mL of KOH

Match each element with the full ground-state electron configuration of the monatomic ion it is most likely to form. (Enter the 6 correct letters, in order: BABCEG, FBAGCC, etc.).

1) K A. 1s22s22p63s23p64s1

2) Cl B. 1s22s22p6

3) Na C. 1s22s22p63s23p64s23d104p65s1

4) Al D. 1s22s22p63s23p1

5) N E. 1s22s22p63s23p6

6) Rb F. 1s2

G. 1s22s22p63s23p64s23d104p6