What the Eq??
Write the equilibrium expression for the reaction:
2NO(g)+O2(g)⇌ 2NO2(g)
What is Kc=[NO2]^2/[NO]^2*[O2]?
What is the main role of a buffer in a solution?
What is the main role of a buffer is to resist changes in pH when small amounts of acid or base are added?
What is the pH of a 0.025 M HCl solution?
What is pH=−log[H+]=−log(0.025)=1.60?
A weak acid HA has an initial concentration of 0.30 M. If its pH at equilibrium is 3.0, what is its dissociation constant Ka?
What is 3.34×10−6?
A weak acid has a pKa of 4.8. What is the ratio of its conjugate base to acid when the solution pH is 5.8?
What is the ratio of conjugate base to acid is 10:1, meaning the solution contains 10 times more conjugate base than weak acid?
The equilibrium constant for a reaction is K=4.2×10^-7. Is the reaction product or reactant favored?
What is since K is much less than 1, the reaction is reactant-favored?
What happens to the pH of a buffer solution when a small amount of a strong acid is added?
What is adding a strong acid will decrease the pH slightly, but the buffer will resist large changes in pH?
A solution has a pH of 9.2. Is it acidic, neutral, or basic?
What is since the pH is greater than 7, the solution is basic?
For the reaction CO(g)+Cl2(g)⇌COCl2, initial concentrations are 0.40 M CO and 0.60 M Cl₂. At equilibrium, [COCl₂] = 0.20 M. What is Kc?
What is Kc=2.5?
Each member of the group has to name one strong acid
What is HCl, HBr, HI, HNO₃,H₂SO₄,HClO₄,HClO₃?
If the reaction quotient Q is greater than K, what happens to the equilibrium position?
What is Q>K the reaction will shift to the left, favoring the reactants to reach equilibrium?
Which of the following pairs could be used to prepare a buffer solution?
a) HNO₃ and NaNO₃
b) NH₃ and NH₄Cl
c) NaOH and NaCl
What is b) NH₃ and NH₄Cl is a valid buffer pair since it is a weak base and its conjugate acid?
Calculate the hydroxide ion concentration [OH−] in a solution with a pH of 3.5.
What is 3.16x10^-11M?
FREE POINTS
What is FREE POINTS???
A solution is 0.10 M in NH₄Cl and 0.10 M in NH₃. If 0.01 M NaOH is added, what happens to the pH?
What is the pH will increase?
For the reaction H2(g)+I2(g)⇌2HI(g), the initial concentrations are [H₂] = 0.50 M, [I₂] = 0.50 M, and [HI] = 0.20 M. If Kc=50.2, which direction will the reaction proceed?
What is Q=0.16M?
Since Q<Kc, the reaction will proceed toward the right (products).
A buffer solution is composed of CH₃COOH and CH₃COO⁻. If more CH₃COOH is added, what happens to the pH?
What is adding more CH₃COOH (the weak acid) will decrease the pH slightly but will not significantly change it because of the buffer's capacity?
What is the pH of a solution with a hydrogen ion concentration of 2.5×10−8M?
What is pH=7.60?
What is the molar solubility of BaSO₄ in a 0.15 M Na₂SO₄ solution at 25°C? The Ksp for BaSO₄ is 1.1×10−10
What is 7.33 × 10⁻¹⁰ M?
What is the equilibrium constant expression for the Ksp of silver carbonate (Ag2CO3)?
What is Ksp=[Ag+]2[CO32−]?
Consider the following reaction at equilibrium:
CH4(g)+H2O(g)⇌CO(g)+3H2(g)
What effect will removing CO(g) have on the system?
What is the reaction will shift in the direction of products?
A buffer solution is prepared using 0.50 M HF and 0.50 M NaF. If the Ka of HF is 6.6×10−4, what is the pH?
*Use the Henderson-Hasselbalch equation
What is pH=3.18?
In a titration curve, this point is reached when the amount of acid equals the amount of base, causing a sharp change in pH.
What is the equivalence point?
Calculate the pH of a 0.020 M solution of diprotic acid (H₂A) with the stepwise dissociation constants Ka1=1.2×10−4 and Ka2=3.6×10−7
What is ph=2.81?
Draw a titration curve of a weak acid and identify the half-equivalence point and equivalence point.