What is the oxidation number of chromium in chromate, CrO42-

What is the pressure of CO2 in the reaction below, given that the equilibrium constant of pressure (Kp) is 3.0? Assume that the temperature remains constant. CaCO3(s) ↔ CaO(s) + CO2(g)

What is the pH of a buffer solution made from 0.30 M HF and 0.20 M NaF if the pKa of the acid is 3.8?

Which description best fits the titration curve below?

What is the relationship between Ksp and molar solubility (s) for this dissociation: Al(OH)3 (s) → Al3+ (aq) + 3OH⁻(aq)

Calculate the equilibrium constant (K) of a reaction if the standard change in Gibbs energy (ΔGo) is -23.8 kJ/mol at 298 K. Report your answer to 3 significant figuresΔGo = -RTlnK                  R = 8.314 J/mol*K

Which of the following is true of weak bases?

Suppose that for a reaction the equilibrium constant was found to be 4.17 x 10-5. Which of the following best describes the concentration of products at equilibrium of this reaction?

What would happen to a saturated CaCO3 solution if aqueous CaCl2 was added?

Consider the general reaction: A ↔ B. The equilibrium constant in concentration (Kc) of a reaction is known to be 2.1 x 10-3. After the initial concentrations of the reactants were changed the reaction quotient (Qc) was found to be 0.78. In what direction will this reaction proceed to reach equilibrium?