Chemical Equilibrium
Adding a catalyst to a reaction at equilibrium will:
A) Shift equilibrium to products
B) Shift equilibrium to reactants
C) Increase the rate of reaching equilibrium
D) Decrease the rate of reaching equilibrium
What is C) Increase the rate of reaching equilibrium
Which of the following is a Lewis acid?
A) NH3
B) BF3
C) OH−
D) H2O
What is B) BF3
What tool is used to indicate when a titration has reached its endpoint
What is an indicator
Which of the following solubility product (Ksp) expressions is NOT correct?
A) BaF₂: Ksp = [Ba²⁺][F⁻]²
B) Al(OH)₃: Ksp = [Al³⁺][OH⁻]³
C) Ca₃(PO₄)₂: Ksp = [Ca²⁺]₃[PO₄³⁻]₂
D) PbCl₂: Ksp = [Pb²⁺][Cl⁻]
What D) PbCl₂: Ksp = [Pb²⁺][Cl⁻]
Who is Haneefa :p
Explain the X is small approx.
What is the assumption that the change in concentration (x) is so small that you can disregard it in equations - check with 5% rule
Calculate the pH of an aqueous solution of sodium hydroxide if the [OH−]=4.5×10−3 M
What is pH = 11.65
Which indicator would be most suitable for a strong acid–weak base titration?
A) Methyl red
B) Phenolphthalein
C) Bromothymol blue
D) Both B and C
What is A) Methyl red
Which of the following barium salts is the least soluble in water?
a) BaSO₄, Ksp = 1.1 × 10⁻¹⁰
b) BaCO₃, Ksp = 5.1 × 10⁻⁹
c) Ba(OH)₂, Ksp = 2.5 × 10⁻⁴
d) BaF₂, Ksp = 1.7 × 10⁻⁶
What is a) BaSO₄, Ksp = 1.1 × 10⁻¹⁰
What are the tables she will provide you with for the exam
What is a Periodic Table, Electronegativity Table, and Polyatomic Ions Table.
Consider the following reaction at equilibrium in a closed container:
CO (g) + O₂ (g) ⇌ 2 CO₂ (g):
At the beginning, 1.4 moles of CO and 0.90 moles of O₂ are present in the container. After the system reaches equilibrium, the concentration of CO₂ is measured to be 0.40 M. The total volume of the container is 4.0 L. Determine the equilibrium constant.
What is Kc = 42.7
Is this solution of AlBr3 salts acidic, basic, or neutral
What is acidic
A 25.0 mL sample of 0.200 M HBr is titrated with 0.150 M KOH. Calculate the volume of KOH needed to reach the equivalence point
What is 33.3 mL
What is [Pb2+] when [SO42−]=0.020 M just begins to precipitate from a solution? Ksp = 1.3×10−5
What is 6.5×10−4M
What are the TAs names
Who are Patrick and Alex
Find Kc for the reaction;2SO2(g)+O2(g)⇌2SO3(g) at 25C
- Kp=5.0×108, R = 0.08206
What is Kc = 1.2x10^10
A 0.300 M solution of HNO₂ has a measured pH of 3.15. Calculate The Ka of nitrous acid and the pKa of nitrous acid
What is Ka = 1.67×10−6, pKa = 5.78
A 50.0 mL sample of 0.120 M HC2H3O2 is titrated with 0.150 M NaOH. Calculate the pH after adding 10.0 mL of NaOH (before the equivalence point).
Ka=1.8×10−5
What is pH = 4.26
The molar solubility of AgCl in water at 25 °C is 1.2×10−5 M.Calculate the solubility product, Ksp of AgCl.
What is Ksp≈1.44×10−10
When and where are my sessions
What isMonday: 2-3 CAR 1210, Thursday 5-6 WAL 3520
At 600 K, 0.800 mol of N2O4 is placed in a 2.00 L container and allowed to reach equilibrium. The reaction is: N2O4(g)⇌2NO2(g). If Kc=0.50 at 600 K, calculate the equilibrium concentrations of N2O4 and NO2
What is [N2O4] = 0.230M and [NO2] = 0.340M
A buffer solution contains 0.150 M acetic acid and 0.100 M sodium acetate. The Ka of acetic acid is 1.8×10−5 Calculate the pH of the buffer
What is pH=4.56
A 40.0 mL sample of 0.120 M HNO₂ is titrated with 0.200 M NaOH. Calculate the pH after adding 35.0 mL of NaOH (after the equivalence point).
What is pH ≈ 12.47
What is the molar solubility of Fe(OH)3 in pure water at 25 °C? Ksp=2.8×10−39
What is s=1.0x10^-10
What type of tiger was RITs first Mascot