Are the following solutions acidic, basic, or neutral? a) KBr(aq) b) NH4Br(aq) c) NaNO2(aq)

Calculate ΔSsurr at 298 K. 2NO(g) +  O2(g) → 2NO2(g) ΔH = -114 kJ

Determine the Kb for CN- at 25°C. The Ka for HCN is 4.9 × 10-10.

1. Select the strongest acid from the following: A) HNO3 or HNO2 B) HCl or HBr 2. Select the strongest base from the following: C) ClO- or ClO2- 3. Which will be more soluble in an acidic solution? D) PbCl2 or PbF2

For the titration of 15.0 mL of 0.200 M HCl with 0.200 M NaOH. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) a) What is the initial pH? pH =  b) What is the pH after the addition of 5.00 mL of NaOH ? pH =  c) What is the pH after the addition of 15.0 mL of NaOH? pH =  d) What is the pH after the addition of 20.0 mL of NaOH? pH = 

Consider the following reaction: 2HI(g) → H2(g) + I2(g) If the initial concentration of HI was 0.350 M and the concentration of HI was 0.025 M after 0.100 s, what is the rate of the reaction?

The vapor pressure of a liquid is 47.1 kPa at 269 K and 10.5 kPa at 264 K. What is the enthalpy of vaporization of the liquid ? You must show all of your work including units for credit.

A 0.150 M solution of a weak base, B, has a pH of 8.80. Calculate the value of Kb for the base. Hint: Write the reaction between the base B and water (B + H2O → BH+ + OH-), and use on ICE Table. You must show all of your work for credit.

1. Select the strongest acid from the following: A) HClO3 or HClO2 B) HBr or HF 2. Select the strongest base from the following: C) BrO- or BrO2- 3. Which will be more soluble in an acidic solution? D) CuCl2 or CuF2

A reaction vessel is charged with COF2, which partially decomposes to carbon dioxide and carbon tetrafluoride. 2COF2(g) ⇌ CO2(g) + CF4(g) When the system comes to equilibrium at 1000oC,  partial pressure of COF2 = 1.50 atm, partial pressure of CO2 = 0.135 atm and partial pressure of CF4 = 0.255 atm. Show all your work and setup for credit. A) Calculate KP for this reaction. B) Calculate KC for this reaction.