Multiple Choice
A 230.0 mL buffer solution initially contains 3.0×10⁻² M of HCHO₂ and 3.0×10⁻² M of NaCHO₂. In order to adjust the buffer pH to 4.20, what mass of NaOH should you add?
17. Acid and Base Equilibrium
Acids Introduction
Back17. Acid and Base Equilibrium
Acids Introduction
- Multiple ChoiceA 370.0 mL buffer solution is 0.150 M in HF and 0.150 M in NaF. What mass of NaOH can this buffer neutralize before the pH rises above 4.00? (Ka(HF) = 3.5 × 10⁻⁴.)
- Multiple ChoiceWhich of the following represents the ionic equation when H+ is added to a solution of acetic acid (CH3COOH) in water?
- Multiple ChoiceIn a 0.10 M KF solution, what is the concentration of H₃O⁺ given that the Ka for HF is 6.8 × 10⁻⁴?
- Multiple ChoiceWhich of the following equations correctly shows how the Cr^{3+} cation acts as an acid in water?
- Multiple ChoiceWhich of the following represents the correct equilibrium expression for the first dissociation of Malonic Acid (H2C3H2O4) in water?
- Multiple ChoiceWhich of the following is the conjugate acid of the base CO3^2-?
- Multiple ChoiceWhich of the following is the conjugate acid of the base H2PO4⁻?
- Multiple ChoiceWhat is the conjugate acid of the base PO4^3-?
- Multiple ChoiceWhich of the following is a stronger acid?
- Multiple ChoiceIs ZnO + H2O -> Zn(OH)₂ an example of an acidic anhydride or a basic anhydride?
- Multiple ChoiceThe titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126.0 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)?
- Multiple ChoiceWhich of the following statements correctly describes strong acids and bases in aqueous solution?
- Multiple ChoiceWhich substances are always produced in an acid-base neutralization reaction?
- Multiple ChoiceWhich of the following best describes acid-base equilibrium?