For the titration of 10.0 mL of 0.200 M HCl with 0.100 M NaOH. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) a) What is the initial pH? pH =  [a] b) What is the pH after the addition of 5.00 mL of NaOH ? pH =  [b] c) What is the pH after the addition of 20.0 mL of NaOH? pH =  [c] d) What is the pH after the addition of 25.0 mL of NaOH? pH =  [d]

Calculate the pH of a solution with a hydroxide ion concentration of 5.25

Calculate the pH of a buffer containing 2.50 M formic acid, HCOOH (Ka = 1.8 × 10-4) and 1.25 M sodium formate, HCOONa.You must show all of your work for credit.

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

Which of the following sets of compounds, when dissolved in the same solution, form a buffer solution?

Given the following data, determine the rate law for the following reaction. 2A  + 3B → 2D Experiment [A] [B] Rate (M/s) 1 2.21 1.00 0.619 2 4.42 1.00 1.24 3 3.36 2.40 2.26

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.

At 298 K , ∆H = 179.2 kJ and ∆S = 160.2 J/K for the reaction shown below. CaCO3(s)  ⟶ CaO(s) + CO2(g) (a) Use the data to decide if this reaction is spontaneous at 298 K. [a] (b) What is the temperature above which the reaction is spontaneous? [b]

Write the cell notation based on the description of the following voltaic cell: Silver ions are reduced to silver metal, and copper metal is oxidized to Cu2+ under standard conditions. Show your work including the two half-reactions.

1.00 mol SO3 is placed in a 1.00 L vessel at 425 K and allowed to come to equilibrium at which time 0.250 mol SO3 remains. 2SO3(g) ⇌ 2SO2(g) + O2(g) A) Calculate the equilibrium concentration of SO2(g) [a] mol/L B) Calculate the equilibrium concentration of O2(g) [b] mol/L C) Calculate KC [c] D) Calculate KP [d]